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A Complete Resource Book in Chemistry for JEE Main

A.K. Singhal

Chapter 5

Solutions - all with Video Answers

Educators

Chapter Questions

00:53

Problem 1

Which of the following colligative properties can provide molar mass of proteins (or polymers or col loids) with greatest precision?
(a) osmotic pressure
(b) elevation of boiling point
(c) depression of freezing point
(d) relative lowing of vapour pressure

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01:20

Problem 2

The beans are cooked sooner in a pressure cooker, because
(a) boiling point increase with increasing pressure
(b) boiling point decrease with increasing pressure
(c) extra pressure of pressure cooker, softens the beans
(d) internal energy is not lost while cooking in pressure cooker.

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01:37

Problem 3

When a saturated solution of sodium chloride is heated, it
(a) becomes remains saturated
(b) becomes unsaturated
(c) becomes supersaturated
(d) achieves equilibrium state

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01:32

Problem 4

Which of these curves represents Henry Law?

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01:21

Problem 5

A solution containing components A and B follows Raoult's law
(a) $\mathrm{A}-\mathrm{B}$ attraction force is greater than $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$
(b) $\mathrm{A}-\mathrm{B}$ attraction force is less than $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$
(c) A - B attraction force remains same as $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$
(d) volume of solution is different from sum of volume of solute and solvent.

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01:34

Problem 6

In liquid $\mathrm{CCl}_{4}$ which of the following has maximum solubility?
(a) $\mathrm{I}_{2}$
(b) $\mathrm{Br}_{2}$
(c) $\mathrm{NaCl}$
(d) $\mathrm{Cl}_{2}^{2}$

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01:25

Problem 7

During osmosis, flow of water through a semipermeable membrane is
(a) from both sides of semi-permeable membrane with unequal flow rates
(b) from solution having lower concentration only
(c) from solution having higher concentration only
(d) from both sides of semi-permeable membrane with equal flow rates

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01:51

Problem 8

A solution of acetone in ethanol
(a) behaves like a near ideal solution
(b) obeys Raoult's law
(c) shows a negative deviation from Raoult's law
(d) shows a positive deviation from Raoult's law

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01:15

Problem 9

Which of the following represents a metastable system?
(a) an unsaturated solution
(b) a dilute solution
(c) a saturated solution
(d) a supersaturated solution

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00:50

Problem 10

According to Raoult's law, relative lowering of vapour pressure for a solution is equal to
(a) mole fraction of the solute
(b) mole fraction of a solvent
(c) moles of a solute
(d) moles of a solvent

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01:08

Problem 11

When non-zero volatile solute is dissolved in a solvent, the relative lowering of vapour pressure is equal to
(a) molar fraction of solute
(b) molar fraction of solvent
(c) concentration of the solute in grams per liter
(d) concentration of the solute in gram per $100 \mathrm{~mL}$.

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01:09

Problem 12

Van't Hoff factor is
(a) more than one in case of association
(b) less than one in case of dissociation normal molecular mass
observed molecular mass
(d) equal to $\frac{\text { ODselkul molecular mass }}{\text { normal molecular mass }}$

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01:14

Problem 13

The solubility of a gas in a liquid increases with
(a) increase of temperature
(b) amount of liquid taken
(c) decrease in temperature
(d) reduction of gas pressure

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01:06

Problem 14

Which of the following solution would exhibit abnormal colligative properties?
(a) $1 \mathrm{M}$ glucose
(b) $0.1 \mathrm{M} \mathrm{NaCl}$
(c) $0.1 \mathrm{M}$ sucrose
(d) 10 gram glass powder in water

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01:16

Problem 15

Which one of the statements given below concerning properties of solutions, describe a colligative effect?
(a) boiling point of pure water decreases by the addition of ethanol
(b) vapour pressure of pure water decreases by the addition of nitric acid
(c) vapour pressure of pure benzene decreases by the addition of naphthalene
(d) boiling point of pure benzene increases by the addition of toluene

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01:35

Problem 16

$V$ litres of a solution contains $m_{2} g$ of non-volatile solute of molecular mass $\mathrm{M}_{2}$. Which of the following can be used to calculate the molecular mass of solute in terms of osmotic pressure?
(a) $\frac{\mathrm{M}_{2}}{\mathrm{~V}}=\frac{\mathrm{M}_{2}}{\pi} \mathrm{VRT}$
(b) $\frac{\mathrm{M}_{2}}{\mathrm{~V}}=\frac{\mathrm{m}_{2}}{\pi} \mathrm{RT}$
(c) $\mathrm{M}_{2}=\frac{\mathrm{M}_{2}}{\mathrm{~V}} \pi \mathrm{RT}$
(d) $\mathrm{M}_{2}=\frac{\mathrm{m}_{2}}{\mathrm{~V}} \frac{\pi}{\mathrm{RT}}$

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01:07

Problem 17

The number of moles of sodium hydroxide present in $2.5 \mathrm{~L}$ and $0.5 \mathrm{M}$ aqueous solution will be
(a) $1.25$
(b) $0.5$
(c) $12.5$
(d) 5

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01:19

Problem 18

Highest boiling point is found in
(a) $0.1 \mathrm{M}$ Sucrose
(b) $0.1 \mathrm{M} \mathrm{BaCl}_{2}$
(c) $0.1 \mathrm{M} \mathrm{NaCl}$
(d) $0.1 \mathrm{M} \mathrm{KCl}$

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01:22

Problem 19

Maximum freezing point will be for 1 molal solution of, assuming equal ionization in each case:
(a) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}$
(b) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}$
(c) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl} .2 \mathrm{H}_{2} \mathrm{O}$
(d) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3} \mathrm{Cl}_{3}\right] \cdot 3 \mathrm{H}_{2} \mathrm{O}^{2}$

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01:42

Problem 20

The solution which has the lowest freezing point is
(a) $0.1 \mathrm{M}$ potassium nitrate
(b) $0.1 \mathrm{M}$ aluminium sulphate
(c) $0.1 \mathrm{M}$ potassium chloride
(d) $0.1 \mathrm{M}$ potassium sulphate

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01:13

Problem 21

The vant Hoff factor 'i' accounts for
(a) the extent of dissociation of solute
(b) the extent of dissolution of solute
(c) the degree of decomposition of solution
(d) degree of solubilization of solute

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01:36

Problem 22

The azeotropic mixture of water and ethonal boils at $78.15^{\circ} \mathrm{C}$. When this mixture is distilled, it is possible to obtain
(a) pure $\mathrm{H}_{2} \mathrm{O}$
(b) pure $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
(c) pure $\mathrm{H}_{2} \mathrm{O}$ as well as pure $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
(d) neither $\mathrm{H}_{2} \mathrm{O}$ nor $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ in their pure state

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00:57

Problem 23

The solution of sugar in water contains
(a) free ions
(b) free atoms
(c) free molecules
(d) free atoms and molecules

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00:51

Problem 24

Which of the following changes with change in temperature?
(a) mole fraction
(b) formality
(c) $\%(\mathrm{w} / \mathrm{W})$
(d) molality

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01:09

Problem 25

When the solute is present in trace quantities the following expression is used
(a) gram per million
(b) nanogram per cent
(c) microgram per cent
(d) parts per million

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01:35

Problem 26

The vapour pressure of a solution (P) and the vapour pressure of the solvent $\left(\mathrm{P}^{\circ}\right)$ are related to each other as
(a) $\mathrm{P}=\mathrm{P}^{0} \mathrm{x}_{2}$
(b) $\mathrm{P}=\mathrm{P}^{0} \mathrm{x}_{1}$
(c) $\mathrm{P}^{0}=\mathrm{Px}_{2}$
(d) $\mathrm{P}^{0}=\mathrm{Px}_{1}$

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01:17

Problem 27

Increasing the temperature of an aqueous solution will cause
(a) decrease in molality
(b) decrease in molarity
(c) decrease in mole fraction
(d) decrease in \% (w/w)

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01:07

Problem 28

During depression in freezing point in a solution, the following are in equilibrium
(a) liquid solvent, solid solvent
(b) liquid solvent, solid solute
(c) liquid solute, solid solute
(d) liquid solute, solid solvent

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01:22

Problem 29

When attraction between $\mathrm{A}-\mathrm{B}$ is more than that of $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$, the solution will show deviation from Raoult's law
(a) positive
(b) negative
(c) no
(d) cannot be predicted

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01:39

Problem 30

People add sodium chloride to water while boiling eggs. This is to
(a) decrease the boiling point of water
(b) increase the boiling point of water
(c) prevent breaking of eggs
(d) make eggs tasty

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01:36

Problem 31

$\mathrm{FeCl}_{3}$ reacts with $\mathrm{K}_{4} \mathrm{Fe}(\mathrm{CN})_{6}$ in aqueous solution to give blue colour if these two are separated by a semipermeable membrance (as shown in the figure), then due to osmosis
(a) blue colour is formed towards side $\mathrm{A}$
(b) blue colour is formed towards side B
(c) blue colour is formed on both the sides side
(d) no blue colouration

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01:37

Problem 32

Which pair of the following will not form an ideal solution?
(a) $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Br}+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{I}$
(b) $\mathrm{H}_{2} \mathrm{O}+\mathrm{C}_{4} \mathrm{H}_{9} \mathrm{OH}$
(c) $\mathrm{CCl}_{4}+\mathrm{SiCl}_{4}$
(d) $\mathrm{C}_{6} \mathrm{H}_{14}+\mathrm{C}_{7} \mathrm{H}_{16}$

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01:01

Problem 33

A molal solution is one that contains one mole of a solute in
(a) $1000 \mathrm{~g}$ of the solvent
(b) one litre of solvent
(c) one litre of solution
(d) $22.4$ litre of the solution

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01:35

Problem 34

A liquid is in equilibrium with its vapour at its boiling point. On the average, the molecules in the two phase have equal
(a) intermolecular forces
(b) potential energy
(c) temperature
(d) kinetic energy

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01:25

Problem 35

The molecular weight of benzoic acid in benzene as determined by depression in freezing point method corresponds to
(a) ionization of benzoic acid
(b) dimerization of benzoic acid
(c) trimerization of benzoic acid
(d) solvation of benzoic acid

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01:10

Problem 36

Which of the following is correct for a solution showing positive deviations from Raoult's law?
(a) $\Delta \mathrm{V}=+\mathrm{ve}, \Delta \mathrm{H}=+\mathrm{ve}$
(b) $\Delta \mathrm{V}=-\mathrm{ve}, \Delta \mathrm{H}=+\mathrm{ve}$
(c) $\Delta \mathrm{V}=+\mathrm{ve}, \Delta \mathrm{H}=-\mathrm{ve}$
(d) $\Delta \mathrm{V}=-\mathrm{ve}, \Delta \mathrm{H}=-\mathrm{ve}$

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01:30

Problem 37

Which one of the following solution has least vapour pressure?
(a) $0.01 \mathrm{M} \mathrm{CaCl}_{2}$
(b) $0.01 \mathrm{M}$ glucose
(c) $0.01 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$
(d) $0.01 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}$

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01:05

Problem 38

Which is true about enthalpy of solution containing benzene and toluene?
(a) $\Delta \mathrm{H}_{\mathrm{sol}}<0$
(b) $\Delta \mathrm{H}_{\text {sol }}=0$
(c) $\Delta \mathrm{H}_{\mathrm{sod}}>0$
(d) $\Delta \mathrm{H}_{\text {sol }}$ may be zero or greater than zero

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01:55

Problem 39

A $5 \%$ solution of sugarcane $($ Mol $w t=342)$ is isotonic with $1 \%$ solution of $X$ under similar conditions. The mol. Wt of $X$ is:
(a) $136.2$
(b) $68.4$
(c) $34.2$
(d) $171.2$

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01:04

Problem 40

Which of the following statement is true about ideal solutions?
(a) the volume of mixing is zero
(b) the enthalpy of mixing is zero
(c) both $\mathrm{A}$ and $\mathrm{B}$
(d) none of these

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01:23

Problem 41

The relationship between osmotic pressure at 273 $\mathrm{K}$ when $10 \mathrm{~g}$ glucose $\left(\mathrm{P}_{1}\right) 10 \mathrm{~g}$ urea $\left(\mathrm{P}_{2}\right)$ and $10 \mathrm{~g}$
sucrose $\left(\mathrm{P}_{3}\right)$ are dissolved in $250 \mathrm{~mL}$ of water is
(a) $\mathrm{P}_{1}>\mathrm{P}_{2}>\mathrm{P}_{3}$
(b) $\mathrm{P}_{3}>\mathrm{P}_{2}>\mathrm{P}_{1}$
(c) $\mathrm{P}_{2}>\mathrm{P}_{1}>\mathrm{P}_{3}$
(d) $\mathrm{P}_{2}>\mathrm{P}_{3}>\mathrm{P}_{1}$

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01:05

Problem 42

Which of the following salt will have the same volume of vant Hoff factor 'i'as that of $\mathrm{K}_{4}[\mathrm{Fe}(\mathrm{CN})] ?$
(a) $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$
(b) $\mathrm{NaCl}$
(c) $\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}$
(d) $\mathrm{Na}_{2} \mathrm{SO}_{4}$

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01:33

Problem 43

Which of the following $0.1 \mathrm{M}$ aqueous solutions will have the lowest freezing point?
(a) $\mathrm{K}_{2} \mathrm{SO}_{4}$
(b) $\mathrm{NaCl}$
(c) urea
(d) glucose

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01:05

Problem 44

Consider this figure and select the correct statement.
(a) $\mathrm{BaCl}_{2}$ flows towards the $\mathrm{KCl}$ solution
(b) $\mathrm{KCl}$ flows towards the $\mathrm{BaCl}_{2}$ solution
(c) there will be no movement of any solution
(d) first $\mathrm{KCl}$ flows towards $\mathrm{BaCl}_{2}$ then reverse process takes place

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00:46

Problem 45

Camphor is used as a solvent to determine molecular weight of non-volatile solute by Rast method because for camphor
(a) its molal depression constant is high
(b) being very cheap
(c) high melting point
(d) all of these

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01:33

Problem 46

3. 65 grams of $\mathrm{HCl}$ is dissolved in $16.2$ grams of water The mole fraction of $\mathrm{HCl}$ in the resulting solution is
(a) $0.4$
(b) $0.3$
(c) $0.2$
(d) $0.1$

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01:19

Problem 47

By dissolving $5 \mathrm{~g}$ substance in $50 \mathrm{~g}$ of water, the decrease in freezing point is $1.2^{\circ} \mathrm{C}$. The molal depression constant is $1.85^{\circ} \mathrm{kg} \mathrm{mol}^{-1} .$ The molecular weight of substance is
(a) $105.4$
(b) $118.2$
(c) $137.2$
(d) $154.2$

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02:07

Problem 48

If the molarity of $20 \%$ solution of sulphuric acid is $2.55 \mathrm{M}$. The density of the solution will be
(a) $2.55 \mathrm{gem}^{-3}$
(b) $1.25 \mathrm{~g} \mathrm{~cm}^{-3}$
(c) $0.125 \mathrm{~g} \mathrm{~L}^{-1}$
(d) $3.25 \mathrm{~g} \mathrm{~L}^{-1}$

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01:15

Problem 49

If the molarity of $20 \%$ solution of sulphuric acid is $2.55 \mathrm{M}$. The density of the solution will be
(a) $2.55 \mathrm{gem}^{-3}$
(b) $1.25 \mathrm{~g} \mathrm{~cm}^{-3}$
(c) $0.125 \mathrm{~g} \mathrm{~L}^{-1}$
(d) $3.25 \mathrm{~g} \mathrm{~L}^{-1}$

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01:48

Problem 50

${ }^{4} \mathbf{x}$ ' grams of water is mixed in 69 grams of ethanol Mole fraction of ethanol in the resultant solution is 0.6. what is the value of ' $x$ ' in grams?
(a) 54
(b) 36
(c) 180
(d) 18

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02:03

Problem 51

The vapours pressure of water at $23^{\circ} \mathrm{C}$ is $19.8 \mathrm{~mm}$. of $\mathrm{Hg} .0 .1$ mole of glucose is dissolved in $178.2 \mathrm{~g}$ of water. What is the vapour pressure (in $\mathrm{mm}$ of $\mathrm{Hg}$ ) of the resultant solution?
(a) $19.0$
(b) $19.602$
(c) $19.402$
(d) $19.202$

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02:20

Problem 52

A molal solution of sodium chloride has a density of $1.21 \mathrm{~g} \mathrm{~mL}^{-1}$. The molarity of this solution is
(a) $3.15$
(b) $1.143$
(c) $2.95$
(d) $4.15$

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01:04

Problem 53

$0.5 \mathrm{M}$ of $\mathrm{H}_{2} \mathrm{SO}_{4}$ is diluted from 1 litre to 10 litre, normaliy of the resulting solution is
(a) $1 \mathrm{~N}$
(b) $10 \mathrm{~N}$
(c) $11 \mathrm{~N}$
(d) $0.1 \mathrm{~N}$

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01:16

Problem 54

Which of the following solutions are isotonic with respect to one another?
1. $0.15 \mathrm{M}$ urea
2. $0.05 \mathrm{M} \mathrm{CaCl}_{2}$
3. $0.1 \mathrm{M} \mathrm{MgSO}_{4}$
4. $0.15 \mathrm{M}$ glucose
Select the correct answer using the codes given below:
(a) 1 and 4
(b) 1,2 and 4
(c) 2 and 3
(d) 2,3 and 4

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01:07

Problem 55

At room temperature, the mole fraction of a solute is $0.25$ and the vapour pressure of a solvent is $0.80 \mathrm{~atm}$. The lowering of vapour pressure is
(a) $0.60$
(b) $0.75$
(c) $0.20$
(d) $0.80$.

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01:22

Problem 56

$50 \mathrm{~mL}$ of $10 \mathrm{~N} \mathrm{H}_{2} \mathrm{SO}_{4}, 25 \mathrm{~mL}$ of $12 \mathrm{~N} \mathrm{HCl}$ and $40 \mathrm{~mL}$
of $5 \mathrm{~N} \mathrm{HNO}_{3}$ are mixed and the volume of the mixture is made $1000 \mathrm{~mL}$ by adding water. The normality of resulting solution will be
(a) $9 \mathrm{~N}$
(b) $4 \mathrm{~N}$
(c) $1 \mathrm{~N}$
(d) $2 \mathrm{~N}$

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01:58

Problem 57

Equal volumes of ethylene glycol (molar mass $=62$ ) and water (molar mass $=18$ ) are mixed. The depression in freezing point of water is (given $\mathrm{K}_{f}$ of water $=$ $1.86 \mathrm{~K}$ mor $^{-1} \mathrm{~kg}$ and specific gravity of ethylene glycol is $1.11$ )
(a) $0.0033$
(b) $0.033$
(c) $0.33$
(d) $33.3$

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01:03

Problem 58

The elevation in boiling point for $13.44 \mathrm{~g}$ of $\mathrm{CuCl}_{2}$ dissolved in $1 \mathrm{~kg}$ of water as solvent will be $\left(\mathrm{K}_{\mathrm{b}}=0.52 \mathrm{~kg} / \mathrm{J}\right.$, molar mass of $\left.\mathrm{CuCl}_{2}=134.4 \mathrm{~g} / \mathrm{mol}\right)$
(a) $0.05$
(b) $0.10$
(c) $0.16$
(d) $0.20$.

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02:04

Problem 59

The temperature at which $10 \%$ aqueous solution of glucose will show the osmotic pressure of $14 \mathrm{~atm}$ is
(a) $34 \mathrm{~K}$
(b) $307.3^{\circ} \mathrm{C}$
(c) $307.3 \mathrm{~K}$
(d) $34^{\circ} \mathrm{C}$

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02:33

Problem 60

The mass of glucose that should be dissolved in $50 \mathrm{~g}$ of water in order to produce the same lowering of vapour pressure as is produced by dissolving $1 \mathrm{~g}$ of urea in the same quantity of water is
(a) $1 \mathrm{~g}$
(b) $3 \mathrm{~g}$
(c) $6 \mathrm{~g}$
(d) $18 \mathrm{~g}$

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01:18

Problem 61

Osmotic pressure observed when benzoic acid is dissolved in benzene is less than that expected from theoretical considerations. This is because
(a) benzoic acid is an organic solute
(b) benzoic acid has higher molar mass than benzene
(c) benzoic acid gets associated in benzene
(d) benzoic acid gets dissociated in benzene

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01:10

Problem 62

The rise in the boiling point of a solution containing $1.8 \mathrm{~g}$ of glucose in $100 \mathrm{~g}$ of solvent is $0.1^{\circ} \mathrm{C}$. The molal elevation constant of the liquid is
(a) $1 \mathrm{~K} / \mathrm{m}$
(b) $0.1 \mathrm{~K} / \mathrm{m}$
(c) $0.01 \mathrm{~K} / \mathrm{m}$
(d) $10 \mathrm{~K} / \mathrm{m}$

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01:14

Problem 63

Which of the following solutions will exhibit highest boiling point?
(a) $0.01 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$ (aq)
(b) $0.01 \mathrm{M} \mathrm{KNO}_{3}$ (aq)
(c) $0.015 \mathrm{M}$ urea (aq)
(d) $0.015 \mathrm{M}$ glucose (aq)

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01:04

Problem 64

At same temperature, which pair of the following solutions are isotonic solutions?
(a) $0.2 \mathrm{M} \mathrm{BaCl}_{2}$ and $0.2 \mathrm{M}$ urea
(b) $0.1 \mathrm{M}$ urea and $0.1 \mathrm{MNaCl}$
(c) $0.1 \mathrm{M} \mathrm{NaCl}$ and $0.1 \mathrm{M} \mathrm{K}_{2} \mathrm{SO}_{4}$
(d) $0.1 \mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ and $0.1 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$

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01:36

Problem 65

At certain temperature, a 5.12\% solution of cane sugar is isotonic with a $0.9 \%$ solution of an unknown solute. The molar mass of solute is
(a) 60
(b) $46.17$
(c) 120
(d) 90

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02:47

Problem 66

The freezing point of $0.1 \mathrm{M}$ solution of glucose is $-1.86^{\circ} \mathrm{C}$. If an equal volume of $0.3 \mathrm{M}$ glucose solution is added, the freezing point of the mixture will be
(a) $-5.58^{\circ} \mathrm{C}$
(b) $-7.44^{\circ} \mathrm{C}$
(c) $-3.72^{\circ} \mathrm{C}$
(d) $-2.79^{\circ} \mathrm{C}$

Raghvendra Singh
Raghvendra Singh
Numerade Educator
01:01

Problem 67

KBr is $80 \%$ dissociated in aqueous solution of $0.5 \mathrm{M}$ concentration. (Given $\mathrm{K}_{t}$ for water $=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ ). The solution freezes at
(a) $271.326 \mathrm{~K}$
(b) $272 \mathrm{~K}$
(c) $270.5 \mathrm{~K}$
(d) $268.5 \mathrm{~K}$

Raghvendra Singh
Raghvendra Singh
Numerade Educator
01:18

Problem 68

If at certain temperature the vapour pressure of pure water is $25 \mathrm{~mm}$ of $\mathrm{Hg}$ and that of a very dilute aqueous urea solution is $24.5 \mathrm{~mm}$ of $\mathrm{Hg}$, the molality of the solution is
(a) $0.02$
(b) $1.2$
(c) $1.11$
(d) $0.08$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:49

Problem 69

Benzoic acid undergoes dimerization in benzene solution, the van't Hoff factor 'i' is related to the degree of association ' $\mathrm{x}$ ' of to the acid as
(a) $\mathrm{i}=(1+\mathrm{x})$
(b) $\mathrm{i}=(1-\mathrm{x})$
(c) $\mathrm{i}=(1-\mathrm{x} / 2)$
(d) $\mathrm{i}=(1+\mathrm{x} / 2)$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:11

Problem 70

The vapour pressure of water at $300 \mathrm{~K}$ in a closed container is $0.4 \mathrm{~atm}$. If the volume of the container is doubled, its vapour pressure at $300 \mathrm{~K}$ will be
(a) $0.8 \mathrm{~atm}$
(b) $0.2 \mathrm{~atm}$
(c) $0.4 \mathrm{~atm}$
(d) $0.6 \mathrm{~atm}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:00

Problem 71

A solution is obtained by dissolving $6 \mathrm{~g}$ of urea (mol. wt $=60$ ) in a litre solution, another solution is prepared by dissolving $34.2 \mathrm{~g}$ of cane sugar (mol. $\mathrm{wt}=342$ ) in a litre of solution at the same temperature The lowering of vapour pressure in the first solution is
(a) same as that of second solution
(b) double that of second solution
(c) half that of second solution
(d) nearly one fifth of the second solution

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:33

Problem 72

The aqueous solution that has the lowest vapour pressure at a given temperature is
(a) $0.1$ molal sodium phosphate
(b) $0.1$ molal barium chloride
(c) $0.1$ molal sodium chloride
(d) $0.1$ molal glucose

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:58

Problem 73

Van't Hoff factor for a dilute solution of sodium argento cyanide is
(a) 2
(b) $0.25$
(c) $3.0$
(d) $0.50$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:10

Problem 74

What is the density (in $\mathrm{g} \mathrm{L}^{-1}$ ) of $\mathrm{CO}_{2}$ at $400 \mathrm{~K}$ and exerting a pressure of $0.0821 \mathrm{~atm} ?(\mathrm{R}=0.0821 \mathrm{~L} \mathrm{~atm}$
$\left.\mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)$
(a) $0.01$
(b) $0.11$
(c) $2.5$
(d) 44

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:21

Problem 75

The vapour pressure of two liquids ' $\mathrm{P}$ ' and ' $\mathrm{Q}$ ' are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of $\mathrm{P}$ and $2 \mathrm{~mol}$ of Q would be
(a) 20 torr
(b) 72 torr
(c) 68 torr
(d) 140 torr

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:25

Problem 76

A solution containing $10 \mathrm{~g}$ per $\mathrm{dm}^{3}$ of urea (molecular mass $=60 \mathrm{~g} \mathrm{~mol}^{-1}$ ) is isotonic with a $5 \%$ solution of a nonvolatile solute. The molecular mass of this non volatile solute is
(a) $350 \mathrm{~g} \mathrm{~mol}^{-1}$
(b) $200 \mathrm{~g} \mathrm{~mol}^{-1}$
(c) $250 \mathrm{~g} \mathrm{~mol}^{-\mathrm{t}}$
(d) $300 \mathrm{~g} \mathrm{~mol}^{-1}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:00

Problem 77

$1.00 \mathrm{~g}$ of a non-electrolyte solute (molar mass $250 \mathrm{~g} \mathrm{~mol}^{-1}$ ) was dissolved in $51.2 \mathrm{~g}$ of benzene. If the freezing point depression constant, $K_{f}$ of benzene is $5.12 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$, the freezing point of benzene will be lowered by
(a) $0.5 \mathrm{~K}$
(b) $0.2 \mathrm{~K}$
(c) $0.4 \mathrm{~K}$
(d) $0.3 \mathrm{~K}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:00

Problem 78

If $0.44 \mathrm{~g}$ of substance dissolved in $22.2 \mathrm{~g}$ of benzene lowers the freezing point of benzene by $0.567^{\circ} \mathrm{C}$, then the molecular mass of substance is, (the molal depression constant $\left.=5.12^{\circ} \mathrm{C} \mathrm{mol}^{-1} \mathrm{~kg}\right)$
(a) $128.4$
(b) $156.6$
(c) $178.9$
(d) $232.4$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:00

Problem 79

The osmotic pressure at $17^{\circ} \mathrm{C}$ of an aqueous solution containing $1.75 \mathrm{~g}$ of sucrose per $150 \mathrm{~mL}$ solution is
(a) $0.08 \mathrm{~atm}$
(b) $8.1 \mathrm{~atm}$
(c) $0.81$
(d) $9.1 \mathrm{~atm}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:02

Problem 80

Two solutions containing $0.75 \mathrm{~g}$ of urea (molecular weight 60 ) and $1.5 \mathrm{~g}$ of compound $\mathrm{A}$ in $100 \mathrm{~g}$ water, freeze at the same temperature. The molecular weight of $\mathrm{A}$ is
(a) 60
(b) 30
(c) 120
(d) 240

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:03

Problem 81

By dissolving $10 \mathrm{~g}$ of a non-volatile solute in $100 \mathrm{~g}$ of benzene, the boiling point rises by $1^{\circ} \mathrm{C}$. The molecular mass of solute is $\left[\mathrm{K}_{\mathrm{b}}\right.$ for benzene $\left.=2.53 \mathrm{~K} \mathrm{~m}^{-1}\right]$
(a) $235 \mathrm{~g}$
(b) $352 \mathrm{~g}$
(c) $250 \mathrm{~g}$
(d) $253 \mathrm{~g}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:12

Problem 82

Among the following aqueous solutions, the correct order of increasing boiling point can be given as
(i) $10^{-4} \mathrm{M} \mathrm{KCl}$
(ii) $10^{-3} \mathrm{M}$ urea
(iii) $10^{-3} \mathrm{M} \mathrm{CaCl}_{2}$
(iv) $10^{-3} \mathrm{M} \mathrm{KCl}$
(a) $\mathrm{I}<\mathrm{IV}<\mathrm{II}<\mathrm{III}$
(b) $\mathrm{I}<\mathrm{II}<\mathrm{IV}<\mathrm{III}$
(c) $\mathrm{IV}<\mathrm{II}<\mathrm{I}<\mathrm{III}$
(d) $\mathrm{I}<\mathrm{II}<\mathrm{III}<\mathrm{IV}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:13

Problem 83

If $\mathrm{P}^{\circ}$ and $\mathrm{P}$ are the vapour pressure of solvent and solution and $\mathrm{n}_{1}$ and $\mathrm{n}_{2}$ are the moles of solute and solvent respectively

Hast Aggarwal
Hast Aggarwal
Numerade Educator
00:54

Problem 84

Two liquids having vapour pressures $\mathrm{P}_{1}^{0}$ and $\mathrm{P}_{2}^{0}$ in pure state in the ratio of $2: 1$ are mixed in a molar ratio of $1: 2$. The ratio of their moles in the vapour state can be
(a) $2: 1$
(b) $1: 2$
(c) $1: 1$
(d) $3: 3$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:40

Problem 85

The molal elevation constant of water is $0.51$. The boiling point of $0.1$ molal aqueous $\mathrm{NaCl}$ solution is nearly
(a) $100.05^{\circ} \mathrm{C}$
(b) $100.1^{\circ} \mathrm{C}$
(c) $100.2^{\circ} \mathrm{C}$
(d) $101.0^{\circ} \mathrm{C}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
04:38

Problem 86

An aqueous solution containing $1 \mathrm{~g}$ of urea boils at $100.25^{\circ} \mathrm{C}$. The aqueous solution containing $3 \mathrm{~g}$ of glucose in the same volume will boil at
(a) $100.75^{\circ} \mathrm{C}$
(b) $100.5^{\circ} \mathrm{C}$
(c) $100^{\circ} \mathrm{C}$
(d) $100.25^{\circ} \mathrm{C}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:09

Problem 87

Equal volumes of $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ and $0.2 \mathrm{M} \mathrm{NaCl}$ are mixed. The concentration of nitrate ions in the mixture will be
(a) $0.1 \mathrm{M}$
(b) $0.05 \mathrm{M}$
(c) $0.2 \mathrm{M}$
(d) $0.15 \mathrm{M}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:20

Problem 88

A solution obtained by dissolving $0.2 \mathrm{~g}$ of solute in $100 \mathrm{~cm}^{3}$ of solution in benzene at $21^{\circ} \mathrm{C}$ develops a rise of $2.4 \mathrm{~mm}$ Hg osmotic equilibrium. Find molarity and molality in the solution. (If density of solution is $0.88$ $\left.\mathrm{g} / \mathrm{cm}^{3}\right)$
(a) $8.3 \times 10^{-3} \mathrm{~mol} / \mathrm{L}$
(b) $4.15 \times 10^{-6} \mathrm{~mol} / \mathrm{L}$
(c) $8.3 \times 10^{-4}$
(d) none

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:12

Problem 89

In a depression in freezing point experiment, it is found that
(1) the vapour pressure of the solution is less than that of pure solvent
(2) the vapour pressure of the solution is more than that of pure solvent
(3) only solute molecules solidify at the freezing point
(4) only solvent molecules solidify at the freezing point
(a) 1,2
(b) 2,3
(c) 1,4
(d) 1,3

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:16

Problem 90

On mixing $3 \mathrm{~g}$ of non-volatile solute in $200 \mathrm{~mL}$ of water its boiling point $\left(100^{\circ} \mathrm{C}\right)$ becomes $100.52^{\circ} \mathrm{C}$. If $\mathrm{K}_{b}$ for water is $0.6 \mathrm{~K} / \mathrm{m}$ then molecular weight of the solute is
(a) $10.5 \mathrm{~g} \mathrm{~mol}^{-1}$
(b) $12.6 \mathrm{~g} \mathrm{~mol}^{-1}$
(c) $15.7 \mathrm{~g} \mathrm{~mol}^{-1}$
(d) $17.3 \mathrm{~g} \mathrm{~mol}^{-1}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:35

Problem 91

$20 \mathrm{~g}$ of a substance were dissolved in $500 \mathrm{~mL}$ of water and the osmotic pressure of the solution was found to be $600 \mathrm{~mm}$ of mercury at $15^{\circ} \mathrm{C}$. The molecular weight of substance is
(a) 998
(b) 1028
(c) 1098
(d) 1198

Hast Aggarwal
Hast Aggarwal
Numerade Educator
03:12

Problem 92

The freezing point of equimolal aqueous solution will be highest for
(a) $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{~N}^{+} \mathrm{H}_{3} \mathrm{Cl}^{-}$(aniline hydrochloride)
(b) $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$
(c) $\mathrm{La}\left(\mathrm{NO}_{3}\right)_{3}$
(d) $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ (glucose)

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:13

Problem 93

A sugar syrup weighing $214.2 \mathrm{~g}$, contains $34.2 \mathrm{~g}$ of water. The molal concentration is
(a) $0.55$
(b) $5.5$
(c) 55
(d) $0.1$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
04:01

Problem 94

When mercuric iodide is added to the aqueous solution of potassium iodide, the
(a) freezing point is raised
(b) freezing point does not change
(c) freezing point is lowered
(d) boiling point does not change

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:54

Problem 95

The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is $0.0125$. The molarity of the solution is
(a) $0.70$
(b) $0.45$
(c) $0.34$
(d) $0.50$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:58

Problem 96

The depression in freezing point of $0.01 \mathrm{M}$ aqueous solution of urea, sodium chloride and sodium sulphate is in the ratio
(a) $1: 1: 1$
(b) $1: 2: 3$
(c) $1: 2: 4$
(d) $2: 2: 3$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:12

Problem 97

Osmotic pressure of a solution is $0.0821 \mathrm{~atm}$ at a temperature of $300 \mathrm{~K}$. The concentration in moles/litre will be
(a) $0.33$
(b) $0.066$
(c) $0.3 \times 10^{-2}$
(d) 3

Mahendra Rathore
Mahendra Rathore
Numerade Educator
00:49

Problem 98

Osmotic pressure of a solution is $0.0821 \mathrm{~atm}$ at a temperature of $300 \mathrm{~K}$. The concentration in moles/litre will be
(a) $0.33$
(b) $0.066$
(c) $0.3 \times 10^{-2}$
(d) 3

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:24

Problem 99

A $1.02 \%$ solution of glycerine is isotopic with $2 \%$ solution of glucose. What will be the molecular mass of glycerine?
(a) $91.8$
(b) $93.0$
(c) $90.2$
(d) $96.4$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:07

Problem 100

The osmotic pressure of a solution containing $4.0$ $\mathrm{g}$ of solute (molar mass 246 ) per litre at $27^{\circ} \mathrm{C}$ is $\left(\mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $0.1 \mathrm{~atm}$
(b) $0.3 \mathrm{~atm}$
(c) $0.4 \mathrm{~atm}$
(d) $0.9 \mathrm{~atm}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:24

Problem 101

A solution of urea (mol. mass $56 \mathrm{~g} \mathrm{~mol}^{-\mathrm{t}}$ ) boils at $100.18^{\circ} \mathrm{C}$ at atmospheric pressure. If $\mathrm{K}_{\mathrm{f}}$ and $\mathrm{K}_{b}$ for water are $1.86$ and $0.512 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ respectively, the above solution will freeze at
(a) $6.54^{\circ} \mathrm{C}$
(b) $-6.54^{\circ} \mathrm{C}$
(c) $-0.654^{\circ} \mathrm{C}$
(d) $0.654^{\circ} \mathrm{C}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:14

Problem 102

An aqueous solution of sucrose $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$, containing $34.2 \mathrm{~g} / \mathrm{L}$, has an osmotic pressure of $2.38$ atmospheres at $17^{\circ} \mathrm{C}$. For an aqueous solution of glucose $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ to be isotonic with this solution, it would have
(a) $18.0 \mathrm{~g} / \mathrm{L}$
(b) $16.2 \mathrm{~g} / \mathrm{L}$
(c) $36.6 \mathrm{~g} / \mathrm{L}$ of glucose
(d) $14.0 \mathrm{~g} / \mathrm{L}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
05:46

Problem 103

A $5 \%$ solution (by mass) of cane sugar in water has a freezing point of $271 \mathrm{~K}$ and freezing point of pure water is $273.15 \mathrm{~K}$. The freezing point of a $5 \%$ solution (by mass) of glucose in water is
(a) $271 \mathrm{IK}$
(b) $273.15 \mathrm{~K}$
(c) $269.07 \mathrm{~K}$
(d) $277.23 \mathrm{~K}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:53

Problem 104

A decimolar solution of potassium ferrocyanide is $50 \%$ dissociated at $300 \mathrm{~K}$. Calculate the osmotic pressure of the solution. $\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $0.07389 \mathrm{~atm}$
(b) $7.389 \mathrm{~atm}$
(c) $738.89 \mathrm{~atm}$
(d) $73.89 \mathrm{~atm}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:18

Problem 105

A decimolar solution of potassium ferrocyanide is $50 \%$ dissociated at $300 \mathrm{~K}$. Calculate the osmotic pressure of the solution. $\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $0.07389 \mathrm{~atm}$
(b) $7.389 \mathrm{~atm}$
(c) $738.89 \mathrm{~atm}$
(d) $73.89 \mathrm{~atm}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
04:31

Problem 106

$\mathrm{pH}$ of $0.1 \mathrm{M}$ monobasic acid solution is found to be $2 .$ Thus its osmotic pressure at T. K. is
(a) $11.11 \mathrm{ST}$
(b) $0.11 \mathrm{ST}$
(c) $0.011 \mathrm{ST}$
(d) $1.11 \mathrm{ST}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:43

Problem 107

The elevation in boiling point for $13.44 \mathrm{~g}$ of $\mathrm{CuCl}_{2}$ dissolved in $1 \mathrm{~kg}$ of water as solvent will be $\left(\mathrm{K}_{\mathrm{b}}=0.52\right.$ $\mathrm{kg} / \mathrm{J}$, molar mass of $\mathrm{CuCl}_{2}=134.4 \mathrm{~g} / \mathrm{mol}$ )
(a) $0.05$
(b) $0.10$
(c) $0.16$
(d) $0.20$.

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:46

Problem 108

A $0.004 \mathrm{M}$ solution of $\mathrm{Na}_{2} \mathrm{SO}_{4}$ is isotonic with a $0.010$ M solution of glucose at same temperature. The apparent degree of dissociation of $\mathrm{Na}_{2} \mathrm{SO}_{4}$ is
(a) $25 \%$
(b) $50 \%$
(c) $75 \%$
(d) $85 \%$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:19

Problem 109

What is the freezing point of one litre of an aqueous solution of a non-electrolyte having an osmotic pressure of $2 \mathrm{~atm}$ at $300 \mathrm{~K}$.
(a) $273.349 \mathrm{~K}$
(b) $263.159 \mathrm{~K}$
(c) $215.569 \mathrm{~K}$
(d) $272.849 \mathrm{~K}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:31

Problem 110

The molality of 1 litre solution of $93 \% \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{w} / \mathrm{v})$ having density $1.84 \mathrm{~g} / \mathrm{mL}$ is
(a) $10.43$
(b) $1.043$
(c) $0.1043$
(d) $100.43$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:51

Problem 111

The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour phase in contact with equimolar solution of benzene and toluene is
(a) $0.6$
(b) $0.50$
(c) $0.27$
(d) $0.74$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:15

Problem 112

An aqueous solution of $6.3 \mathrm{~g}$ oxalic acid dihydrate is made up to $250 \mathrm{~mL}$. The volume of $0.1 \mathrm{~N} \mathrm{NaOH}$ required to completely neutralize $10 \mathrm{~mL}$ of this solution is
(a) $40 \mathrm{~mL}$
(b) $20 \mathrm{~mL}$
(c) $10 \mathrm{~mL}$
(d) $4 \mathrm{~mL}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:58

Problem 113

An aqueous solution of $6.3 \mathrm{~g}$ oxalic acid dihydrate is made up to $250 \mathrm{~mL}$. The volume of $0.1 \mathrm{~N} \mathrm{NaOH}$ required to completely neutralize $10 \mathrm{~mL}$ of this solution is
(a) $40 \mathrm{~mL}$
(b) $20 \mathrm{~mL}$
(c) $10 \mathrm{~mL}$
(d) $4 \mathrm{~mL}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
03:05

Problem 114

The van't Hoff factor for $0.1 \mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ solution is 2.74. The degree of dissociation is
(a) $91.4 \%$
(b) $87 \%$
(c) $100 \%$
(d) $75 \%$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:06

Problem 115

The van't Hoff factor for $0.1 \mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ solution is 2.74. The degree of dissociation is
(a) $91.4 \%$
(b) $87 \%$
(c) $100 \%$
(d) $75 \%$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:41

Problem 116

A $0.2$ molal aqueous solution of a weak acid $(\mathrm{HX})$ is $20 \%$ ionized. The freezing point of this solution is (Given $\mathrm{K}_{\mathrm{f}}=1.86^{\circ} \mathrm{C} \mathrm{kg} \mathrm{mol}^{-1}$ for water $)$
(a) $-0.45^{\circ} \mathrm{C}$
(b) $-0.90^{\circ} \mathrm{C}$
(c) $-0.21^{\circ} \mathrm{C}$
(d) $-0.43^{\circ} \mathrm{C}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
03:33

Problem 117

The osmotic pressure of urea solution is $500 \mathrm{~mm}$ of $\mathrm{Hg}$ at $10^{\circ} \mathrm{C}$. If the solution is diluted and temperature is raised to $25^{\circ} \mathrm{C}$, the osmotic pressure decreases to $105.3 \mathrm{~mm}$ of $\mathrm{Hg}$, what is the extent of dilution?
(a) 10 times
(b) $2.5$ times
(c) 5 times
(d) $7.5$ times

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:41

Problem 118

The molality of a $15 \%(\mathrm{w} / \mathrm{v})$ solution of $\mathrm{H}_{2} \mathrm{SO}_{4}$ of density $1.1 \mathrm{~g} / \mathrm{cm}^{3}$ is nearly
(a) $1.3$
(b) $1.6$
(c) $1.46$
(d) $1.86$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:30

Problem 119

The vapour pressure of a solution of $5 \mathrm{~g}$ of non electrolyte in $100 \mathrm{~g}$ of water at a particular temperature is $2985 \mathrm{Nm}^{-2}$. The vapour pressure of pure water at that temperature is $3000 \mathrm{Nm}^{-2}$. The molecular weight of the solute is
(a) 180
(b) 90
(c) 270
(d) 360

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:08

Problem 120

A current of dry air was bubbled through a bulb containing $26 \mathrm{~g}$ of an organic substance in $200 \mathrm{~g}$ of water, then through a bulb at the same temperature, containing pure water and finally through a tube containing fused $\mathrm{CaCl}_{2}$. The loss of weight of water bulb is $0.013$ $\mathrm{g}$ and the gain of the weight of $\mathrm{CaCl}_{2}$ tube is $4 \mathrm{~g}$. The molecular weight of organic substance is
(a) 820
(b) 740
(c) 720
(d) 840

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:36

Problem 121

Organic liquids A and B have vapour pressures $\mathrm{p}_{1}^{0}$ and $\mathrm{p}_{2}^{\circ}$ as pure liquids at $80^{\circ} \mathrm{C}$. A mixture of the two liquids behaving ideally and boiling at $80^{\circ} \mathrm{C}$ has mole fraction of $\mathrm{A}=0.16$. If $\left(\mathrm{p}_{2}^{\circ}-\mathrm{p}_{1}^{\circ}\right)=472 \mathrm{~mm}$ of $\mathrm{Hg}$, what is the
value of $p_{1}^{0}$ (in $\mathrm{mm} \mathrm{Hg}$ )?
(a) $263.6 \mathrm{~mm}$
(b) $463.5 \mathrm{~mm}$
(c) $663.3 \mathrm{~mm}$
(d) $363.5 \mathrm{~mm}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:09

Problem 122

When 2 moles each of Hexane and heptane are mixed and if $\mathrm{P}_{\text {Hexane }}^{\text {and }} \mathrm{P}_{\text {Hepane }}^{\circ}$ are $50 \mathrm{~mm} \mathrm{Hg}$ and $60 \mathrm{~mm} \mathrm{Hg}$ respectively than?
(a) $\mathrm{P}_{\text {Total }}=55 \mathrm{~mm} \mathrm{Hg}$
(b) $\mathrm{P}_{\text {Hevans }}=25 \mathrm{~mm} \mathrm{Hg}$
(c) $\mathrm{P}_{\text {Hepene }}=30 \mathrm{~mm} \mathrm{Hg}$
(d) None-Ideal solution

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:56

Problem 123

When 2 moles each of Hexane and heptane are mixed and if $\mathrm{P}_{\text {Hexane }}^{\text {and }} \mathrm{P}_{\text {Hepane }}^{\circ}$ are $50 \mathrm{~mm} \mathrm{Hg}$ and $60 \mathrm{~mm} \mathrm{Hg}$ respectively than?
(a) $\mathrm{P}_{\text {Total }}=55 \mathrm{~mm} \mathrm{Hg}$
(b) $\mathrm{P}_{\text {Hevans }}=25 \mathrm{~mm} \mathrm{Hg}$
(c) $\mathrm{P}_{\text {Hepene }}=30 \mathrm{~mm} \mathrm{Hg}$
(d) None-Ideal solution

Rajesh Singh
Rajesh Singh
Numerade Educator
00:50

Problem 124

In the freezing point depression experiment, it is observed that
(a) at the freezing point the solvent begins to freeze.
(b) relative lowering of vapour pressure of solution $(\mathrm{X})$ is more than $(\mathrm{Y})$.
(c) the decrease in freezing point of $0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}$ (X) in $\mathrm{C}_{6} \mathrm{H}_{6}$ is lower than that of $0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}$
(Y) in water.
(d) the decrease in freezing point in the two solutions is same.

Mishal Gul
Mishal Gul
Numerade Educator
01:21

Problem 125

I mole benzene $\left(p_{\text {bename }}^{o}=42 \mathrm{~mm}\right.$ ) and 2 mole toluene $\left(p_{\text {hemene }}^{o}=36 \mathrm{~mm}\right.$ ) will have:
(a) Mole fraction of benzene in vapour phase above liq. Mixture is $1 / 3$.
(b) Mole fraction of toluene in vapour phase above liq. Mixture is $8 / 19$
(c) Total vapour pressure of solution is $38 \mathrm{~mm}$
(d) Mole fraction of benzene in vapour phase above liquid mixture is $7 / 19$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:33

Problem 126

An aqueous solution of a solute which nerther assoc1ates nor dissociates has a freezing point depression of $\mathrm{X}^{\circ} \mathrm{C}$. An equimolar solution of a second has a freezing point depression of $4 \mathrm{X}^{\circ} \mathrm{C}$. The second solution could be a salt of formula (assuming $100 \%$ dissociation )
(a) $\mathrm{AB}_{2}$
(b) $\mathrm{A}_{2} \mathrm{~B}_{2}$
(c) $\mathrm{A}_{3} \mathrm{~B}$
(d) $\mathrm{AB}_{3}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:26

Problem 127

A solution containing $0.1$ mole of naphthalene and $0.9$ mole of benzene is cooled out until some benzene freezes out. The solution is then decanted off from the solid and warmed upto $353 \mathrm{~K}$ where its vapour pressure was found to be 670 torr. The freezing point and boiling point of benzene are $278.5 \mathrm{~K}$ and $353 \mathrm{~K}$ respectively and its enthalpy of fusion is $10.67 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Which of the following statement (s) is /are correct?
(a) Temperature to which solution is frozen is $269.7 \mathrm{~K}$
(b) Weight of naphthalene that freezes is $0.025 \mathrm{~g}$.
(c) Weight of benzene frozen out is $12.13 \mathrm{~g}$
(d) The depression in freezing point is $8.92 \mathrm{~g}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:07

Problem 128

The amount of dissolved oxygen in 1 litre water in equilibrium with air at 1 atm pressure at $25^{\circ} \mathrm{C}$ will be (assume that air contains 20 mole \% oxygen, Henry's constant $(\mathrm{kH})$ for oxygen is $3.04 \times 10^{7} \mathrm{~mm} \mathrm{Hg}$ and density of $\mathrm{H}_{2} \mathrm{O}$ at $25^{\circ} \mathrm{C}$ is $1 \mathrm{~g} / \mathrm{cc}$ )
(a) the mole fraction of $\mathrm{O}_{2}$ in solution is $5 \times 10^{-6}$
(b) the mole fraction of $\mathrm{O}_{2}^{2}$ in solution is $5 \times 10^{-7}$
(c) the molarity of $\mathrm{O}_{2}$ in solution is $2.77 \times 10^{-5} \mathrm{M}$
(d) the molarity of $\mathrm{O}_{2}$ in solution is $2.77 \times 10^{4} \mathrm{M}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:16

Problem 129

Which of the following can form minimum boiling point azeotropic mixture?
(a) Ethyl alcohol + water
(b) Carbon tetrachloride + chloroform
(c) Ethyl alcohol + water
(d) Acetone + chloroform

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:30

Problem 130

Correct mathematical equations for the Raoult's law are
(a) $\frac{P^{o}-P_{S}}{P_{s}}=$ mole fraction of solvent
(b) $\frac{P^{O_{S}}-P_{S}}{P_{o}}=$ mole fraction of a nonvolatile solute
(c) $P_{s} \propto$ mole fraction of solvent
(d) $P_{s} \propto$ mole fraction of a non volatile solute

Mahendra Rathore
Mahendra Rathore
Numerade Educator
03:17

Problem 131

For the binary ideal solution having 1 mole of $\mathrm{A}$ and 2 moles of B at $298 \mathrm{~K}$ which one is correct?
(a) $\Delta \mathrm{S}_{\operatorname{mix}}=-\mathrm{R} \sum \mathrm{x}_{1} \ln \mathrm{x}_{\mathrm{i}}$
(b) $\Delta \mathrm{H}_{\operatorname{mix}}=0$
(c) $\Delta \mathrm{G}_{\operatorname{mix}}=\mathrm{RT} \sum \mathrm{x}_{\mathrm{i}} \ln \mathrm{x}_{\mathrm{i}}$
(d) $\Delta \mathrm{H}_{\operatorname{mix}}=(+)$ ve

Nikhil Choudhary
Nikhil Choudhary
Numerade Educator
01:44

Problem 132

The van't Hoff factor (i), is a measure of association or dissociation. The van't Hoff factor for $0.1 \mathrm{M}$ aqueous sodium chloride is $1.87 .$ In magnesium sulphate the ionic interactions
(a) Are weaker than that observed in sodium chloride.
(b) Are same as that observed in sodium chloride
(c) Are stronger than that observed in sodium chloride.
(d) Are not responsible for the (i) value.

Mahendra Rathore
Mahendra Rathore
Numerade Educator
04:01

Problem 133

Mercuric iodide is added to an aqueous solution of potassium iodide. Identify the correct statement(s)
(a) Freezing point is raised.
(b) Freezing point is lowered.
(c) Freezing point and boiling point does not change.
(d) Boiling point is raised.
(a) 1 and 4
(b) 3 and 4
(c) Only 1
(d) 2 and 4

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:21

Problem 134

Mercuric iodide is added to an aqueous solution of potassium iodide. Identify the correct statement(s)
(a) Freezing point is raised.
(b) Freezing point is lowered.
(c) Freezing point and boiling point does not change.
(d) Boiling point is raised.
(a) 1 and 4
(b) 3 and 4
(c) Only 1
(d) 2 and 4

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:39

Problem 135

The colligative properties of electrolytes require a slightly different approach than the one used for the colligative properties of non- electrolytes. The electrolytes dissociate into ions in solution. It is the number of solute particles that determine the colligative properties of a solution. The electrolyte solutions, therefore show abnormal colligative properties. To account for this effect we define a quantity; called the van't Hoff factor which is given by [solution]
$i=$
$\frac{\text { Actual number of particles in solution after dissociation }}{\text { Number of formula units initally dissolved in solution }}$ $\mathrm{i}=1$ (for non - electrolytes); $\mathrm{i}>1$ (for electrolytes, undergoing dissociation) $\mathrm{i}<1$ (for solute, undergoing association)
Benzoic acid undergoes dimerisation in benzene solution. The van't Hoff factor 'i' is related to the degree of association ' $\alpha$ ' of the acid as
(a) $i=1+\alpha$
(b) $i=1-\alpha$
(c) $i=1+\frac{\alpha}{2}$
(d) $i=1-\frac{\alpha}{2}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:00

Problem 136

The colligative properties of electrolytes require a slightly different approach than the one used for the colligative properties of non- electrolytes. The electrolytes dissociate into ions in solution. It is the number of solute particles that determine the colligative properties of a solution. The electrolyte solutions, therefore show abnormal colligative properties. To account for this effect we define a quantity; called the van't Hoff factor which is given by [solution]
$i=$
$\frac{\text { Actual number of particles in solution after dissociation }}{\text { Number of formula units initally dissolved in solution }}$ $\mathrm{i}=1$ (for non - electrolytes); $\mathrm{i}>1$ (for electrolytes, undergoing dissociation) $\mathrm{i}<1$ (for solute, undergoing association)
For a solution of a non electrolyte in water, the van't Hoff factor is
(a) Always equal to 2
(b) Always equal to 0
(c) $>1$ but $<2$
(d) $\leq 1$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:33

Problem 137

The colligative properties of electrolytes require a slightly different approach than the one used for the colligative properties of non- electrolytes. The electrolytes dissociate into ions in solution. It is the number of solute particles that determine the colligative properties of a solution. The electrolyte solutions, therefore show abnormal colligative properties. To account for this effect we define a quantity; called the van't Hoff factor which is given by [solution]
$i=$
$\frac{\text { Actual number of particles in solution after dissociation }}{\text { Number of formula units initally dissolved in solution }}$ $\mathrm{i}=1$ (for non - electrolytes); $\mathrm{i}>1$ (for electrolytes, undergoing dissociation) $\mathrm{i}<1$ (for solute, undergoing association)
$0.1 \mathrm{M} \mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$ is $60 \%$ ionized. What will be its
van't Hoff factor?
(a) $3.4$
(b) $1.7$
(c) $2.4$
(d) $2.2$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:23

Problem 138

Match the following

Hitendra Singh
Hitendra Singh
Numerade Educator
03:09

Problem 139

A molecule Bn dissolves in water and is non- volatile. A solution of certain molality showed a depression of $0.93 \mathrm{~K}$ in freezing point. The same solution boiled at $100.26^{\circ} \mathrm{C}$. When $7.9 \mathrm{~g}$ of Bn was dissolved in $100 \mathrm{~g}$ water, the solution boiled at $100.44^{\circ} \mathrm{C}$. Given $\mathrm{K}_{\mathrm{f}}$ for water $=1.86 \mathrm{~K} \mathrm{~mol}^{-1} \mathrm{~kg}$ and Atomic mass of $\mathrm{B}=31$
The value of ' $n$ ' is

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:51

Problem 140

Assuming $100 \%$ polymerisation of phenol in its aqueous solution, the number of phenol molecules undergoing polymerization containing $9.4 \mathrm{~g}$ of phenol per $100 \mathrm{~g}$ of the solution is

Freezing point of the solution is $0.93^{\circ} \mathrm{C}$.

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:41

Problem 141

A $0.001$ molal solution of $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{4}\right]$ in water had a freezing point depression, $0.0056^{\circ} \mathrm{C} . \mathrm{K}_{\mathrm{f}}$ for water is $1.86^{\circ} \mathrm{cm}^{-1} .$ The number of moles of $\mathrm{AgNO}_{3}$ required to react with one mole of the complex in aqueous solution is

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:22

Problem 142

Relationship between molarity (M) and molality (m) of a solution is given as $m=\frac{M}{\left(1000 \times d-M \times M_{B}\right)} \times 10^{n}$
where $\mathrm{n}$ is (Given: d- density of the solution in $\mathrm{g}$.
$\mathrm{cm}^{-3} ; \mathrm{MB}-$ molar mass of solute)

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:54

Problem 143

$\mathrm{K}_{2} \mathrm{HgI}_{4}$ is $50 \%$ ionized in aqueous solution. Find the value of $i$.

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:59

Problem 144

What would be the $\mathrm{pH}$ of a $0.1$ molal aqueous solution of a monoprotic acid 'HA', that freezes at $-0.2046^{\circ} \mathrm{C}$ ? $\left[\mathrm{K}_{\mathrm{f}}\left(\mathrm{H}_{2} \mathrm{O}\right)=1.86^{\circ} \mathrm{mol}^{-1} \mathrm{~kg} ;\right.$ assuming molality $=$
molarity]

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:59

Problem 145

What would be the $\mathrm{pH}$ of a $0.1$ molal aqueous solution of a monoprotic acid 'HA', that freezes at $-0.2046^{\circ} \mathrm{C}$ ? $\left[\mathrm{K}_{\mathrm{f}}\left(\mathrm{H}_{2} \mathrm{O}\right)=1.86^{\circ} \mathrm{mol}^{-1} \mathrm{~kg} ;\right.$ assuming molality $=$
molarity]

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:20

Problem 146

An aqueous solution containing ionic salt having molality equal to $0.1892$ freezes at $-0.704^{\circ} \mathrm{C}$. The van't Hoff factor of the ionic salt will be equal to $\left(\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{Km}^{-1}\right)$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:29

Problem 147

Which of the following concentration factor is affected by change in temperature?
(a) molarity
(b) molality
(c) mole fraction
(d) weight fraction

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:40

Problem 148

In a mixture of $\mathrm{A}$ and $\mathrm{B}$, components show negative deviation when:
(a) $\mathrm{A}-\mathrm{B}$ interaction is stronger than $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$ interaction
(b) $\mathrm{A}-\mathrm{B}$ interaction is weaker than $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$ interaction
(c) $\Delta \mathrm{V}_{\text {mix }}>0, \Delta \mathrm{S}_{\operatorname{mix}}>0$
(d) $\Delta \mathrm{V}_{\operatorname{mix}}=0, \Delta \mathrm{S}_{\operatorname{mix}}>0$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:50

Problem 149

For an aqueous solution, freezing point is $-0.186^{\circ} \mathrm{C}$. Elevation of the boiling point of the same solution is $$
\left(\mathrm{K}_{\ell}=1.86^{\circ} \mathrm{mol}^{-1} \mathrm{~kg} \text { and } \mathrm{K}_{\mathrm{b}}=0.512^{\circ} \mathrm{mol}^{-1} \mathrm{~kg}\right)
$$
(a) $0.186^{\circ}$
(b) $0.0512^{\circ}$
(c) $1.86^{\circ}$
(d) $5.12^{\circ}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:29

Problem 150

In a $0.2$ molal aqueous solution of a weak acid HX, the degree of ionization is $0.3 .$ Taking $K_{f}$ for water as $1.85 \mathrm{k} \mathrm{kg}$ melt, the freezing point of the solution will be nearest to
(a) $-0.480^{\circ} \mathrm{C}$
(b) $-0.360^{\circ} \mathrm{C}$
(c) $-0.260^{\circ} \mathrm{C}$
(d) $+0.480^{\circ} \mathrm{C}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:03

Problem 151

If liquids A and B form an ideal solution, the
(a) enthalpy of mixing is zero
(b) entropy of mixing is zero
(c) free energy of mixing is zero
(d) free energy as well as the entropy of mixing are each zero

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:18

Problem 152

If liquids A and B form an ideal solution, the [2003]
(a) enthalpy of mixing is zero(b) entropy of mixing is zero
(c) free energy of mixing is zero
(d) free energy as well as the entropy of mixing are each zero

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:49

Problem 153

Which one of the following aqueous solutions will exhibit highest boiling point?
(a) $0.05 \mathrm{M}$ glucose
(b) $0.01 \mathrm{M} \mathrm{KNO}_{3}$
(c) $0.015 \mathrm{M}$ urea
(d) $0.01 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:18

Problem 154

Which of the following liquid pairs shows a positivedeviation from Raoult' law?
(a) water-nitric acid
(b) water-hydrochloric acid
(c) benzene-methanol
(d) acetone-chloroform

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:03

Problem 155

Which one of the following statements is false?
(a) two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression
(b) the osmotic pressure ( $\pi$ ) of a solution is given by the equation $\pi=\mathrm{MRT}$, where $\mathrm{M}$ is the molarity of the solution
(c) Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction
(d) the correct order of osmotic pressure for $0.01 \mathrm{M}$ aqueous solution of each compound is $\mathrm{BaCl}_{2}>$ $\mathrm{KCl}<\mathrm{CH}_{3} \mathrm{COOH}>$ Sucrose

Mishal Gul
Mishal Gul
Numerade Educator
01:21

Problem 156

If a is the degree of dissociation of $\mathrm{Na}_{2} \mathrm{SO}_{4}$ the van't Hoff factor (i) used for calculating the molecular mass is
(a) $1+\alpha$
(b) $1-\alpha$
(c) $1+2 \alpha$
(d) $1-2 \alpha$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:39

Problem 157

Benzene and toluene form nearly ideal solutions. At $20^{\circ} \mathrm{C}$, the vapour pressure of benzene is 75 torr and that of toluene is 22 torr. The partial vapour pressure of benzene at $20^{\circ} \mathrm{C}$ for a solution containing $78 \mathrm{~g}$ of benzene and $46 \mathrm{~g}$ of toluene in torr is
(a) 25
(b) 50
(c) $37.5$
(d) $53.5$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:16

Problem 158

Two solutions of a substance (non-electrolyte) are mixed in the following manner. $480 \mathrm{~mL}$ of $1.5 \mathrm{M}$ first solution $+520 \mathrm{~mL}$ of $1.2 \mathrm{M}$ second solution. What is the molarity of the final mixture?
(a) $1.344 \mathrm{M}$
(b) $2.70 \mathrm{M}$
(c) $1.50 \mathrm{M}$
(d) $1.20 \mathrm{M}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:35

Problem 159

Density of a $2.05 \mathrm{M}$ solution of acetic acid in water is $1.02 \mathrm{~g} / \mathrm{mL}$. The molality of the solution is
(a) $1.14 \mathrm{~mol} \mathrm{~kg}^{-1}$
(b) $3.28 \mathrm{~mol} \mathrm{~kg}^{-1}$
(c) $2.28 \mathrm{~mol} \mathrm{~kg}^{-1}$
(d) $0.44 \mathrm{~mol} \mathrm{~kg}^{-1}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:44

Problem 160

$18 \mathrm{~g}$ of glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ is added to $178.2 \mathrm{~g}$ of water.
The vapour pressure of water for this aqueous solution at $100^{\circ} \mathrm{C}$ is
(a) $759.00$ torr
(b) $7.60$ torr
(c) $76.00$ torr
(d) $752.40$ torr

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:37

Problem 161

A $5.25 \%$ solution of a substance is isotonic with a $1.5 \%$ solution of urea (molar mass $=60 \mathrm{~g} \mathrm{~mol}^{-1}$ ) in the same solvent. If the densities of both the solutions are assumed to be equal to $1.0 \mathrm{~g} \mathrm{~cm}^{-3}$, molar mass of the substance will be
(a) $115.0 \mathrm{~g} \mathrm{~mol}^{-1}$
(b) $105.0 \mathrm{~g} \mathrm{~mol}^{-1}$
(c) $210.0 \mathrm{~g} \mathrm{~mol}^{-1}$
(d) $90.0 \mathrm{~g} \mathrm{~mol}^{-1}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:40

Problem 162

A mixture of ethyl alcohol and propyl alcohol has a vapour pressure of $290 \mathrm{~mm}$ at $300 \mathrm{~K}$. The vapour pressure of propyl alcohol is $200 \mathrm{~mm}$. If the mole fraction of ethyl alcohol is $0.6$, its vapour pressure (in $\mathrm{mm}$ ) at the same temperature will be
(a) 300
(b) 700
(c) 360
(c) 350

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:49

Problem 163

At $80^{\circ} \mathrm{C}$, the vapour pressure of pure liquid 'A' is 520 $\mathrm{mm} \mathrm{Hg}$ and that of pure liquid 'B' is $1000 \mathrm{~mm} \mathrm{Hg}$. If a mixture solution of 'A' and 'B' boils at $80^{\circ} \mathrm{C}$ and $\mathrm{I}$ atm pressure, the amount of 'A' in the mixture is ( $1 \mathrm{~atm}=$ $760 \mathrm{~mm} \mathrm{Hg}$ ).
(a) $52 \mathrm{~mol}$ per cent
(b) 34 mol per cent
(c) 48 mol per cent
(d) $50 \mathrm{~mol}$ per cent

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:27

Problem 164

At $80^{\circ} \mathrm{C}$, the vapour pressure of pure liquid 'A' is 520 $\mathrm{mm} \mathrm{Hg}$ and that of pure liquid 'B' is $1000 \mathrm{~mm} \mathrm{Hg}$. If a mixture solution of 'A' and 'B' boils at $80^{\circ} \mathrm{C}$ and $\mathrm{I}$ atm pressure, the amount of 'A' in the mixture is ( $1 \mathrm{~atm}=$ $760 \mathrm{~mm} \mathrm{Hg}$ ).
(a) $52 \mathrm{~mol}$ per cent
(b) 34 mol per cent
(c) 48 mol per cent
(d) $50 \mathrm{~mol}$ per cent

Hast Aggarwal
Hast Aggarwal
Numerade Educator
02:35

Problem 165

Two liquids $\mathrm{X}$ and $\mathrm{Y}$ form an ideal solution. At $300 \mathrm{~K}$, vapour pressure of the solutions containing 1 mol of $\mathrm{X}$ and $3 \mathrm{~mol}$ of $\mathrm{Y}$ is $550 \mathrm{mmHg}$. At the same temperature, if $1 \mathrm{~mol}$ of $\mathrm{Y}$ is further added to this solu-

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:28

Problem 166

A binary liquid solution is prepared by mixing n-heptane and ethanol. Which on of the following statement is correct regarding the behavior of the solution?
(a) The solution in non-ideal, showing +ve deviation from Raoult's Law.
(b) The solution in non-ideal, showing -ve deviation from Raoult's Law.
(c) n-heptane shows tre deviation while ethanol shows -ve deviation from Raoult's Law.
(d) The solution formed is an ideal solution.

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:05

Problem 167

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water $\left(\Delta \mathrm{T}_{\mathrm{p}}\right)$, when $0.01 \mathrm{~mol}$ of sodium sulphate is dissolved in $1 \mathrm{Kg}$ of water, is $\left(\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$
(a) $0.0372 \mathrm{~K}$
(b) $0.0558 \mathrm{~K}$
(c) $0.0744 \mathrm{~K}$
(d) $0.0186 \mathrm{~K}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:20

Problem 168

On mixing, heptane and octane form an ideal solution. At $373 \mathrm{~K}$, the vapour pressures of the two liquid components (heptane and octane) are $105 \mathrm{kPa}$ and $45 \mathrm{kPa}$ respectively. Vapour pressure of the solution obtained by mixing $25.0 \mathrm{~g}$ of heptane and $35 \mathrm{~g}$ of octane will be (molar mass of heptane $=100 \mathrm{~g} \mathrm{~mol}^{-1}$ and of octane $=$ $114 \mathrm{~g} \mathrm{~mol}^{-1}$ )
(a) $72.0 \mathrm{kPa}$
(b) $36.1 \mathrm{kPa}$
(c) $96.2 \mathrm{kPa}$
(d) $144.5 \mathrm{kPa}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
02:36

Problem 169

The degree of dissociation $(\alpha)$ of a weak electrolyte, $\mathrm{A}_{\mathrm{x}} \mathrm{B}_{\mathrm{y}}$ is related to van't Hoff factor (i) by the expression:
(a) $\alpha=\frac{x+y-1}{i-1}$
(b) $\alpha=\frac{x+y+1}{i-1}$
(c) $\alpha=\frac{1-1}{(x+y-1)}$
(d) $\alpha=\frac{1-1}{x+y+1}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:40

Problem 170

Ethylene glycol is used as antifreeze in a cold climate. Mass of ethylene glycol which should be added to $4 \mathrm{~kg}$ of water to prevent it form freezing at $-6^{\circ} \mathrm{C}$ will be: $\left(\mathrm{K}_{f}\right.$ for water $=1.86 \mathrm{~kg} \mathrm{~mol}^{-1}$, and molar mass of ethylene glycol $=62 \mathrm{~g} \mathrm{~mol}^{-1}$ )
(a) $204.11 \mathrm{~g}$
(b) $804.32 \mathrm{~g}$
(c) $600.20 \mathrm{~g}$
(d) $302.40 \mathrm{~g}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:34

Problem 171

$K_{t}$ for water is $1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} .$ If your automobile radiator holds $1.0 \mathrm{~kg}$ of water, how many grams of ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ must you add to get the freezing point of the solution lowered to $-2.8^{\circ} \mathrm{C}$ ?
(a) $39 \mathrm{~g}$
(b) $93 \mathrm{~g}$
(c) $72 \mathrm{~g}$
(d) $27 \mathrm{~g}$

Mahendra Rathore
Mahendra Rathore
Numerade Educator
01:15

Problem 172

$K_{t}$ for water is $1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1} .$ If your automobile radiator holds $1.0 \mathrm{~kg}$ of water, how many grams of ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ must you add to get the freezing point of the solution lowered to $-2.8^{\circ} \mathrm{C}$ ?
(a) $39 \mathrm{~g}$
(b) $93 \mathrm{~g}$
(c) $72 \mathrm{~g}$
(d) $27 \mathrm{~g}$

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:04

Problem 173

The vapour pressure of acetone at $20^{\circ} \mathrm{C}$ is 185 torr. When $1.2 \mathrm{~g}$ of a non-volatile substance was dissolved in $100 \mathrm{~g}$ of acetone at $20^{\circ} \mathrm{C}$, its vapour pressure was 183 torr. The molar mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right)$ of the substance is
(a) 32
(b) 64
(c) 128
(d) 488

Hast Aggarwal
Hast Aggarwal
Numerade Educator
01:35

Problem 174

18 g glucose (C6H12O6) is added to $178.2 \mathrm{~g}$ water. The vapour pressure of water (in torr) for this aqueous solution is:
(a) $76.0$
(b) $752.4$
(c) $759.0$
(d) $7.6$

Hast Aggarwal
Hast Aggarwal
Numerade Educator