Introductory Chemistry

Problem 7

Explain the difference between a strong electrolyte solution and a nonelectrolyte solution. What kinds of solutes form strong electrolyte solutions?

David C.

Numerade Educator

00:13

Problem 8

How does gas solubility depend on temperature?

David C.

Numerade Educator

Problem 9

Explain recrystallization.

David C.

Numerade Educator

00:33

Problem 10

How is rock candy made?

David C.

Numerade Educator

Problem 11

When you heat water on a stove, bubbles form on the bottom of the pot before the water boils. What are these bubbles? Why do they form?

David C.

Numerade Educator

00:16

Problem 12

Explain why warm soda pop goes flat faster than cold soda pop.

David C.

Numerade Educator

Problem 13

How does gas solubility depend on pressure? How does this relationship explain why a can of soda pop fizzes when opened?

David C.

Numerade Educator

00:19

Problem 14

What is the difference between a dilute solution and a concentrated solution?

David C.

Numerade Educator

Problem 15

Define the concentration units mass percent and molarity.

David C.

Numerade Educator

Problem 16

What is a stock solution?

David C.

Numerade Educator

00:23

Problem 17

How does the presence of a nonvolatile solute affect the boiling point and melting point of a solution relative to the boiling point and melting point of the pure solvent?

David C.

Numerade Educator

00:43

Problem 18

What are colligative properties?

Amy J.

Numerade Educator

00:14

Problem 19

Define molality.

David C.

Numerade Educator

00:52

Problem 20

What is osmosis?

David C.

Numerade Educator

Two shipwreck survivors were rescued from a life raft. One had drunk seawater while the other had not. The one who had drunk the seawater was more severely dehydrated than the one who did not. Explain.

David C.

Numerade Educator

Problem 22

Why are intravenous fluids always isoosmotic saline solutions? What would happen if pure water were administered intravenously?

David C.

Numerade Educator

Problem 23

Determine whether or not each mixture is a solution.
(a) sand and water mixture
(b) oil and water mixture
(c) salt and water mixture
(d) sterling silver cup

David C.

Numerade Educator

01:05

Problem 24

Determine whether or not each mixture is a solution.
(a) air
(b) carbon dioxide and water mixture
(c) a blueberry muffin
(d) a brass buckle

David C.

Numerade Educator

00:26

Problem 25

Identify the solute and solvent in each solution.
(a) salt water
(b) sugar water
(c) soda water

David C.

Numerade Educator

01:20

Problem 26

Identify the solute and solvent in each solution.
(a) 80 -proof vodka $(40 \%$ ethyl alcohol)
(b) oxygenated water
(c) antifreeze (ethylene glycol and water)

David C.

Numerade Educator

01:12

Problem 27

Pick an appropriate solvent from Table 13.2 to dissolve:
(a) motor oil (nonpolar)
(b) sugar (polar)
(c) lard (nonpolar)
(d) potassium chloride (ionic)

David C.

Numerade Educator

Problem 28

Pick an appropriate solvent from Table 13.2 to dissolve:
(a) glucose (polar)
(b) salt (ionic)
(c) vegetable oil (nonpolar)
(d) sodium nitrate (ionic)

David C.

Numerade Educator

00:17

Problem 29

What are the dissolved particles in a solution containing an ionic solute? What is the name for this kind of solution?

David C.

Numerade Educator

00:17

Problem 30

What are the dissolved particles in a solution containing a molecular solute? What is the name for this kind of solution?

David C.

Numerade Educator

00:36

Problem 31

A solution contains $35 \mathrm{g}$ of $\mathrm{NaCl}$ per $100 \mathrm{g}$ of water at $25^{\circ} \mathrm{C}.$ Is the solution unsaturated, saturated, or supersaturated? (See Figure 13.4.)

David C.

Numerade Educator

00:36

Problem 32

A solution contains $28 \mathrm{g}$ of $\mathrm{KNO}_{3}$ per $100 \mathrm{g}$ of water at $25^{\circ} \mathrm{C} .$ Is the solution unsaturated, saturated, or supersaturated? (See Figure 13.4.)

David C.

Numerade Educator

00:38

Problem 33

A KNO $_{3}$ solution containing $45 \mathrm{g}$ of $\mathrm{KNO}_{3}$ per $100 \mathrm{g}$ of $\mathrm{wa}$ ter is cooled from $40^{\circ} \mathrm{C}$ to $0^{\circ} \mathrm{C}$. What happens during cooling? (See Figure 13.4.)

David C.

Numerade Educator

Problem 34

A KCl solution containing 42 g of KCl per 100 g of water is cooled from $60^{\circ} \mathrm{C}$ to $0^{\circ} \mathrm{C} .$ What happens during cooling? (See Figure 13.4.)

David C.

Numerade Educator

01:31

Problem 35

Refer to Figure 13.4 to determine whether each of the given amounts of solid will completely dissolve in the given amount of water at the indicated temperature.
(a) $30.0 \mathrm{g} \mathrm{KClO}_{3}$ in $85.0 \mathrm{g}$ of water at $35^{\circ} \mathrm{C}$
(b) $65.0 \mathrm{g} \mathrm{NaNO}_{3}$ in $125 \mathrm{g}$ of water at $15^{\circ} \mathrm{C}$
(c) $32.0 \mathrm{g} \mathrm{KCl}$ in $70.0 \mathrm{g}$ of water at $82^{\circ} \mathrm{C}$

David C.

Numerade Educator

01:41

Problem 36

Refer to Figure 13.4 to determine whether each of the given amounts of solid will completely dissolve in the given amount of water at the indicated temperature.
(a) $45.0 \mathrm{g} \mathrm{CaCl}_{2}$ in $105 \mathrm{g}$ of water at $5^{\circ} \mathrm{C}$
(b) $15.0 \mathrm{g} \mathrm{KClO}_{3}$ in $115 \mathrm{g}$ of water at $25^{\circ} \mathrm{C}$
(c) $50.0 \mathrm{g} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$ in $95.0 \mathrm{g}$ of water at $10^{\circ} \mathrm{C}$

David C.

Numerade Educator

00:12

Problem 37

Some laboratory procedures involving oxygen-sensitive reactants or products call for using preboiled (and then cooled) water. Explain why this is so.

David C.

Numerade Educator

Problem 38

A person preparing a fish tank uses preboiled (and then cooled) water to fill it. When the fish is put into the tank, it dies. Explain.

David C.

Numerade Educator

00:27

Problem 39

Scuba divers breathing air at increased pressure can suffer from nitrogen narcosis-a condition resembling drunkenness-when the partial pressure of nitrogen exceeds about 4 atm. What property of gas/water solutions causes this to happen? How could the diver reverse this effect?

David C.

Numerade Educator

00:25

Problem 40

Scuba divers breathing air at increased pressure can suffer from oxygen toxicity-too much oxygen in the bloodstream-when the partial pressure of oxygen exceeds about 1.4 atm. What happens to the amount of oxygen in a diver's bloodstream when he or she breathes oxygen at elevated pressures? How can this be reversed?

David C.

Numerade Educator

01:10

Problem 41

Calculate the concentration of each solution in mass percent.
(a) $41.2 \mathrm{g} \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$ in $498 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$
(b) $178 \mathrm{mg} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ in $4.91 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$
(c) $7.55 \mathrm{g} \mathrm{NaCl}$ in $155 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$

David C.

Numerade Educator

01:10

Problem 42

Calculate the concentration of each solution in mass percent.
(a) $132 \mathrm{g} \mathrm{KCl}$ in $598 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$
(b) $22.3 \mathrm{mg} \mathrm{KNO}_{3}$ in $2.84 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$
(c) $8.72 \mathrm{g} \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ in $76.1 \mathrm{g} \mathrm{H}_{2} \mathrm{O}$

David C.

Numerade Educator

00:20

Problem 43

A soft drink contains $42 \mathrm{g}$ of sugar in $311 \mathrm{g}$ of $\mathrm{H}_{2} \mathrm{O}$. What is the concentration of sugar in the soft drink in mass percent?

David C.

Numerade Educator

00:30

Problem 44

A soft drink contains 32 mg of sodium in 309 g of $\mathrm{H}_{2} \mathrm{O}$. What is the concentration of sodium in the soft drink in mass percent?

David C.

Numerade Educator

02:53

Problem 45

Complete the table.

David C.

Numerade Educator

03:52

Problem 46

Complete the table.

David C.

Numerade Educator

00:20

Problem 47

Ocean water contains $3.5 \%$ NaCl by mass. How much salt can be obtained from 254 g of seawater?

David C.

Numerade Educator

00:25

Problem 48

A saline solution contains $1.1 \%$ NaCl by mass. How much $\mathrm{NaCl}$ is present in $96.3 \mathrm{g}$ of this solution?

David C.

Numerade Educator

Problem 49

Determine the amount of sucrose in each solution.
(a) $48 \mathrm{g}$ of a solution containing $3.7 \%$ sucrose by mass
(b) $103 \mathrm{mg}$ of a solution containing $10.2 \%$ sucrose by mass
(c) $3.2 \mathrm{kg}$ of a solution containing $14.3 \%$ sucrose by mass

David C.

Numerade Educator

Problem 50

Determine the amount of potassium chloride in each solution.
(a) $19.7 \mathrm{g}$ of a solution containing $1.08 \% \mathrm{KCl}$ by mass
(b) $23.2 \mathrm{kg}$ of a solution containing $18.7 \%$ KCl by mass
(c) $38 \mathrm{mg}$ of a solution containing $12 \% \mathrm{KCl}$ by mass

David C.

Numerade Educator

01:04

Problem 51

Determine the mass (in g) of each NaCl solution that contains $1.5 \mathrm{g}$ of $\mathrm{NaCl}.$
(a) $0.058 \%$ NaCl by mass
(b) $1.46 \% \mathrm{NaCl}$ by mass
(c) $8.44 \%$ NaCl by mass

David C.

Numerade Educator

01:13

Problem 52

Determine the mass (in g) of each sucrose solution that contains $12 \mathrm{g}$ of sucrose.
(a) $4.1 \%$ sucrose by mass
(b) $3.2 \%$ sucrose by mass
(c) $12.5 \%$ sucrose by mass

David C.

Numerade Educator

01:28

Problem 53

$\mathrm{AgNO}_{3}$ solutions are often used to plate silver onto other metals. What is the maximum amount of silver in grams that can be plated out of $4.8 \mathrm{L}$ of an $\mathrm{AgNO}_{3}$ solution containing $3.4 \%$ Ag by mass? (Assume that the density of the solution is $1.01 \mathrm{g} / \mathrm{mL} .)$

David C.

Numerade Educator

Problem 54

A dioxin-contaminated water source contains $0.085 \%$ dioxin by mass. How much dioxin is present in 2.5 Lof this water? (Assume that the density of the solution is $1.01 \mathrm{g} / \mathrm{mL}$.)

David C.

Numerade Educator

Problem 55

Ocean water contains $3.5 \%$ NaCl by mass. What mass of ocean water in grams contains $45.8 \mathrm{g}$ of $\mathrm{NaCl}$ ?

David C.

Numerade Educator

00:38

Problem 56

A hard water sample contains $0.0085 \%$ Ca by mass (in the form of $\mathrm{Ca}^{2+}$ ions). What mass of water in grams contains
1.2 $\mathrm{g}$ of $\mathrm{Ca} ?(1.2 \mathrm{g} \text { of } \mathrm{Ca}$ is the recommended daily allowance of calcium for 19 - to 24 -year-olds.)

David C.

Numerade Educator

00:31

Problem 57

Lead is a toxic metal that affects the central nervous system. A Pb-contaminated water sample contains 0.0011\% Pb by mass. What volume of the water in milliliters contains
$115 \mathrm{mg}$ of $\mathrm{Pb} ?$ (Assume that the density of the solution is 1.0 g/mL.)

David C.

Numerade Educator

00:51

Problem 58

Benzene is a carcinogenic (cancer-causing) compound. A benzene-contaminated water sample contains $0.000037 \%$ benzene by mass. What volume of the water in liters contains $175 \mathrm{mg}$ of benzene? (Assume that the density of the solution is $1.0 \mathrm{g} / \mathrm{mL} .)$

David C.

Numerade Educator

Problem 59

Calculate the molarity of each solution.
(a) 0.127 mol of sucrose in 655 mL of solution
(b) $0.205 \mathrm{mol}$ of $\mathrm{KNO}_{3}$ in 0.875 L of solution
(c) $1.1 \mathrm{mol}$ of $\mathrm{KCl}$ in 2.7 L of solution

David C.

Numerade Educator

00:55

Problem 60

Calculate the molarity of each solution.
(a) 1.54 mol of $\mathrm{LiCl}$ in 22.2 L of solution
(b) $0.101 \mathrm{mol}$ of $\mathrm{LiNO}_{3}$ in 6.4 Lof solution
(c) 0.0323 mol of glucose in 76.2 mL of solution

David C.

Numerade Educator

01:50

Problem 61

Calculate the molarity of each solution.
(a) $22.6 \mathrm{g}$ of $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$ in $0.442 \mathrm{L}$ of solution
(b) $42.6 \mathrm{g}$ of $\mathrm{NaCl}$ in $1.58 \mathrm{L}$ of solution
(c) $315 \mathrm{mg}$ of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ in $58.2 \mathrm{mL}$ of solution

David C.

Numerade Educator

01:36

Problem 62

Calculate the molarity of each solution.
(a) $33.2 \mathrm{g}$ of $\mathrm{KCl}$ in 0.895 L of solution
(b) $61.3 \mathrm{g}$ of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$ in 3.4 L of solution
(c) $38.2 \mathrm{mg}$ of $\mathrm{KI}$ in $112 \mathrm{mL}$ of solution

David C.

Numerade Educator

00:33

Problem 63

A 205 -mL sample of ocean water contains $6.8 \mathrm{g}$ of $\mathrm{NaCl}$. What is the molarity of the solution with respect to NaCl?

David C.

Numerade Educator

00:31

Problem 64

A 355 -mL can of soda pop contains $41 \mathrm{g}$ of sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) .$ What is the molarity of the solution with respect to sucrose?

David C.

Numerade Educator

Problem 65

How many moles of $\mathrm{NaCl}$ are contained in each solution?
(a) 1.5 L of a $1.2 \mathrm{M} \mathrm{NaCl}$ solution
(b) $0.448 \mathrm{L}$ of a $0.85 \mathrm{M} \mathrm{NaCl}$ solution
(c) $144 \mathrm{mL}$ of a $1.65 \mathrm{M} \mathrm{NaCl}$ solution

David C.

Numerade Educator

00:56

Problem 66

How many moles of sucrose are contained in each solution?
(a) 3.4 L of a 0.100 M sucrose solution
(b) $0.952 \mathrm{L}$ of a $1.88 \mathrm{M}$ sucrose solution
(c) $21.5 \mathrm{mL}$ of a $0.528 \mathrm{M}$ sucrose solution

David C.

Numerade Educator

00:55

Problem 67

What volume of each solution contains 0.15 mol of KCl?
(a) $0.255 \mathrm{M} \mathrm{KCl}$
(b) $1.8 \mathrm{M} \mathrm{KCl}$
(c) $0.995 \mathrm{M} \mathrm{KCl}$

David C.

Numerade Educator

01:06

Problem 68

What volume of each solution contains 0.325 mol of NaI?
(a) $0.152 \mathrm{M} \mathrm{NaI}$
(b) 0.982 M NaI
(c) 1.76 M NaI

David C.

Numerade Educator

02:53

Problem 69

Complete the table.

David C.

Numerade Educator

03:20

Problem 70

Complete the table.

David C.

Numerade Educator

Problem 71

Calculate the mass of $\mathrm{NaCl}$ in a $35-\mathrm{mL}$ sample of a $1.3 \mathrm{M}$ NaCl solution.

David C.

Numerade Educator

00:26

Problem 72

Calculate the mass of glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ in a $105-\mathrm{mL}$ sample of a $1.02 \mathrm{M}$ glucose solution.

David C.

Numerade Educator

00:27

Problem 73

A chemist wants to make $2.5 \mathrm{L}$ of a $0.100 \mathrm{M} \mathrm{KCl}$ solution. How much KCl in grams should the chemist use?

David C.

Numerade Educator

Problem 74

A laboratory procedure calls for making $500.0 \mathrm{mL}$ of a $1.4 \mathrm{M}$ $\mathrm{KNO}_{3}$ solution. How much $\mathrm{KNO}_{3}$ in grams is needed?

David C.

Numerade Educator

00:35

Problem 75

How many liters of a $0.500 \mathrm{M}$ sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)$ solution contain $1.5 \mathrm{kg}$ of sucrose?

David C.

Numerade Educator

00:33

Problem 76

What volume of a $0.35 \mathrm{M} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ solution contains $87 \mathrm{g}$ of $\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2} ?$

David C.

Numerade Educator

00:51

Problem 77

Determine the concentration of $\mathrm{Cl}^{-}$ in each aqueous solution. (Assume complete dissociation of each compound.)
(a) $0.15 \mathrm{M} \mathrm{NaCl}$
(b) $0.15 \mathrm{M} \mathrm{CuCl}_{2}$
(c) $0.15 \mathrm{M} \mathrm{AlCl}_{3}$

David C.

Numerade Educator

01:11

Problem 78

Determine the concentration of $\mathrm{NO}_{3}^{-}$ in each aqueous solution. (Assume complete dissociation of each compound.)
(a) $0.10 \mathrm{M} \mathrm{KNO}_{3}$
(b) $0.10 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$
(c) $0.10 \mathrm{M} \mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}$

David C.

Numerade Educator

00:59

Problem 79

Determine the concentration of the cation and anion in each aqueous solution. (Assume complete dissociation of each compound.)
(a) $0.12 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$
(b) $0.25 \mathrm{M} \mathrm{K}_{2} \mathrm{CO}_{3}$
(c) $0.11 \mathrm{M} \mathrm{RbBr}$

David C.

Numerade Educator

01:14

Problem 80

Determine the concentration of the cation and anion in each aqueous solution. (Assume complete dissociation of each compound.)
(a) $0.20 \mathrm{M} \mathrm{SrSO}_{4}$
(b) $0.15 \mathrm{M} \mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}$
(c) $0.12 \mathrm{M} \mathrm{SrI}_{2}$

David C.

Numerade Educator

00:19

Problem 81

A 122 -mL sample of a $1.2 \mathrm{M}$ sucrose solution is diluted to $500.0 \mathrm{mL} .$ What is the molarity of the diluted solution?

David C.

Numerade Educator

00:21

Problem 82

A 3.5 -L sample of a $5.8 \mathrm{M} \mathrm{NaCl}$ solution is diluted to $55 \mathrm{L}.$ What is the molarity of the diluted solution?

David C.

Numerade Educator

00:39

Problem 83

Describe how you would make 2.5 L of a 0.100 M KCl solution from a $5.5 \mathrm{M}$ stock $\mathrm{KCl}$ solution.

David C.

Numerade Educator

00:26

Problem 84

Describe how you would make $500.0 \mathrm{mL}$ of a $0.200 \mathrm{M}$ NaOH solution from a $15.0 \mathrm{M}$ stock $\mathrm{NaOH}$ solution.

David C.

Numerade Educator

00:28

Problem 85

To what volume should you dilute $25 \mathrm{mL}$ of a $12 \mathrm{M}$ stock HCl solution to obtain a $0.500 \mathrm{M} \mathrm{HCl}$ solution?

David C.

Numerade Educator

00:24

Problem 86

To what volume should you dilute $75 \mathrm{mL}$ of a $10.0 \mathrm{M}$ $\mathrm{H}_{2} \mathrm{SO}_{4}$ solution to obtain a $1.75 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ solution?

David C.

Numerade Educator

Problem 87

How much of a $12.0 \mathrm{M} \mathrm{HNO}_{3}$ solution should you use to make $850.0 \mathrm{mL}$ of a $0.250 \mathrm{M} \mathrm{HNO}_{3}$ solution?

David C.

Numerade Educator

00:18

Problem 88

How much of a $5.0 \mathrm{M}$ sucrose solution should you use to make $85.0 \mathrm{mL}$ of a $0.040 \mathrm{M}$ solution?

David C.

Numerade Educator

01:24

Problem 89

Determine the volume of $0.150 \mathrm{M} \mathrm{NaOH}$ solution required to neutralize each sample of hydrochloric acid. The neutralization reaction is:
$$\mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaCl}(a q)$$
(a) $25 \mathrm{mL}$ of a $0.150 \mathrm{M} \mathrm{HCl}$ solution
(b) $55 \mathrm{mL}$ of a $0.055 \mathrm{M} \mathrm{HCl}$ solution
(c) $175 \mathrm{mL}$ of a $0.885 \mathrm{M} \mathrm{HCl}$ solution

David C.

Numerade Educator

01:41

Problem 90

Determine the volume of $0.225 \mathrm{M}$ KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is:
$$\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{KOH}(a q) \longrightarrow \mathrm{K}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)$$
(a) $45 \mathrm{mL}$ of $0.225 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$
(b) $185 \mathrm{mL}$ of $0.125 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$
(c) $75 \mathrm{mL}$ of $0.100 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$

David C.

Numerade Educator

00:57

Problem 91

Consider the reaction:
$2 \mathrm{K}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{NiCl}_{2}(a q) \longrightarrow \mathrm{Ni}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+6 \mathrm{KCl}(a q)$
What volume of $0.225 \mathrm{M} \mathrm{K}_{3} \mathrm{PO}_{4}$ solution is necessary to completely react with $134 \mathrm{mL}$ of $0.0112 \mathrm{M} \mathrm{NiCl}_{2} ?$

David C.

Numerade Educator

00:44

Problem 92

Consider the reaction:
$$\mathrm{K}_{2} \mathrm{S}(a q)+\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow 2 \mathrm{KNO}_{3}(a q)+\cos (s)$$
What volume of $0.225 \mathrm{M} \mathrm{K}_{2} \mathrm{S}$ solution is required to completely react with $175 \mathrm{mL}$ of $0.115 \mathrm{M} \mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2} ?$

David C.

Numerade Educator

01:05

Problem 93

A 10.0 -mL sample of an unknown $\mathrm{H}_{3} \mathrm{PO}_{4}$ solution requires $112 \mathrm{mL}$ of $0.100 \mathrm{M}$ KOH to completely react with the $\mathrm{H}_{3} \mathrm{PO}_{4}$. What was the concentration of the unknown $\mathrm{H}_{3} \mathrm{PO}_{4}$ solution?
$$\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{KOH}(a q) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{K}_{3} \mathrm{PO}_{4}(a q)$$

David C.

Numerade Educator

01:04

Problem 94

A 25.0 -mL sample of an unknown $\mathrm{HClO}_{4}$ solution requires $45.3 \mathrm{mL}$ of $0.101 \mathrm{M} \mathrm{NaOH}$ for complete neutralization. What was the concentration of the unknown $\mathrm{HClO}_{4}$ solution? The neutralization reaction is:
$$\mathrm{HClO}_{4}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaClO}_{4}(a q)$$

David C.

Numerade Educator

00:45

Problem 95

What is the minimum amount of $6.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ necessary to produce $15.0 \mathrm{g}$ of $\mathrm{H}_{2}(\mathrm{g})$ according to the reaction:
$$2 \mathrm{Al}(s)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+3 \mathrm{H}_{2}(g)$$

David C.

Numerade Educator

00:49

Problem 96

What is the molarity of $\mathrm{ZnCl}_{2}(a q)$ that forms when $15.0 \mathrm{g}$ of zinc completely reacts with $\mathrm{CuCl}_{2}(a q)$ according to the following reaction? (Assume a final volume of $175 \mathrm{mL}$. )
$$\mathrm{Zn}(s)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{ZnCl}_{2}+\mathrm{Cu}(s)$$

David C.

Numerade Educator

00:39

Problem 97

Calculate the molality of each solution.
(a) 0.25 mol solute; 0.250 kg solvent
(b) $0.882 \mathrm{mol}$ solute; $0.225 \mathrm{kg}$ solvent
(c) 0.012 mol solute; $23 . \overline{1}$ g solvent

David C.

Numerade Educator

00:44

Problem 98

Calculate the molality of each solution.
(a) 0.455 mol solute; 1.97 kg solvent
(b) 0.559 mol solute; 1.44 kg solvent
(c) 0.119 mol solute; 488 g solvent

David C.

Numerade Educator

00:35

Problem 99

Calculate the molality of a solution containing $12.5 \mathrm{g}$ of ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ dissolved in $135 \mathrm{g}$ of water.

David C.

Numerade Educator

00:37

Problem 100

Calculate the molality of a solution containing $257 \mathrm{g}$ glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ dissolved in 1.62 L of water. (Assume a density of $1.00 \mathrm{g} / \mathrm{mL}$ for water.)

David C.

Numerade Educator

01:34

Problem 101

Calculate the freezing point of a water solution at each concentration.
(a) $0.85 \mathrm{m}$
(b) $1.45 m$
(c) $4.8 \mathrm{m}$
(d) $2.35 \mathrm{m}$

David C.

Numerade Educator

01:15

Problem 102

Calculate the freezing point of a water solution at each concentration.
(a) $0.100 m$
(b) $0.469 m$
(c) $1.44 m$
(d) $5.89 \mathrm{m}$

David C.

Numerade Educator

01:18

Problem 103

Calculate the boiling point of a water solution at each concentration.
(a) $0.118 m$
(b) $1.94 m$
(c) $3.88 m$
(d) $2.16 m$

David C.

Numerade Educator

01:17

Problem 104

Calculate the boiling point of a water solution at each concentration.
(a) $0.225 \mathrm{m}$
(b) $2.58 m$
(c) $4.33 \mathrm{m}$
(d) $6.77 \mathrm{m}$

David C.

Numerade Educator

01:28

Problem 105

A glucose solution contains $55.8 \mathrm{g}$ of glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ in 455 g of water. Calculate the freezing point and boiling point of the solution. (Assume a density of $1.00 \mathrm{g} / \mathrm{mL}$ for water.)

David C.

Numerade Educator

01:38

Problem 106

An ethylene glycol solution contains $21.2 \mathrm{g}$ of ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ in $85.4 \mathrm{mL}$ of water. Calculate the freezing point and boiling point of the solution. (Assume a density of $1.00 \mathrm{g} / \mathrm{mL}$ for water.)

David C.

Numerade Educator

01:26

Problem 107

An NaCl solution is made using $133 \mathrm{g}$ of $\mathrm{NaCl}$ and diluting to a total solution volume of 1.00 L. Calculate the molarity and mass percent of the solution. (Assume a density of $1.08 \mathrm{g} / \mathrm{mL}$ for the solution.)

David C.

Numerade Educator

00:56

Problem 108

A $\mathrm{KNO}_{3}$ solution is made using $88.4 \mathrm{g}$ of $\mathrm{KNO}_{3}$ and diluting to a total solution volume of 1.50 L. Calculate the molarity and mass percent of the solution. (Assume a density of $1.05 \mathrm{g} / \mathrm{mL}$ for the solution.)

David C.

Numerade Educator

01:22

Problem 109

A 125 -mL sample of an $8.5 \mathrm{M} \mathrm{NaCl}$ solution is diluted to 2.5 L. What volume of the diluted solution contains $10.8 \mathrm{g}$ of NaCl?

David C.

Numerade Educator

Problem 110

A 45.8 -mL sample of a $5.8 \mathrm{M} \mathrm{KNO}_{3}$ solution is diluted to 1.00 L. What volume of the diluted solution contains 15.0
$g$ of $\mathrm{KNO}_{3} ?$

David C.

Numerade Educator

00:54

Problem 111

To what final volume should you dilute $50.0 \mathrm{mL}$ of a 5.00 M KI solution so that $25.0 \mathrm{mL}$ of the diluted solution contains $3.25 \mathrm{g}$ of $\mathrm{KI}$ ?

David C.

Numerade Educator

01:07

Problem 112

To what volume should you dilute $125 \mathrm{mL}$ of an $8.00 \mathrm{M}$ $\mathrm{CuCl}_{2}$ solution so that $50.0 \mathrm{mL}$ of the diluted solution contains $5.9 \mathrm{g} \mathrm{CuCl}_{2} ?$

David C.

Numerade Educator

01:04

Problem 113

What is the molarity of an aqueous solution that is $5.88 \%$ NaCl by mass? (Assume a density of $1.02 \mathrm{g} / \mathrm{mL}$ for the solution.)

David C.

Numerade Educator

00:54

Problem 114

What is the molarity of an aqueous solution that is $6.75 \%$ glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ by mass? (Assume a density of $1.03 \mathrm{g} /$ mL for the solution.)

David C.

Numerade Educator

01:23

Problem 115

Consider the reaction:
$$2 \mathrm{Al}(s)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+3 \mathrm{H}_{2}(g)$$
What minimum volume of $4.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ is required to produce $15.0 \mathrm{L}$ of $\mathrm{H}_{2}$ at STP?

David C.

Numerade Educator

01:19

Problem 116

Consider the reaction:
$$\mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)$$
What minimum amount of $1.85 \mathrm{M} \mathrm{HCl}$ is necessary to produce $28.5 \mathrm{L}$ of $\mathrm{H}_{2}$ at STP?

David C.

Numerade Educator

Problem 117

How much of a 1.25 M sodium chloride solution in milliliters is required to completely precipitate all of the silver in $25.0 \mathrm{mL}$ of a $0.45 \mathrm{M}$ silver nitrate solution?

David C.

Numerade Educator

00:58

Problem 118

How much of a 1.50 M sodium sulfate solution in milliliters is required to completely precipitate all of the barium in $150.0 \mathrm{mL}$ of a $0.250 \mathrm{M}$ barium nitrate solution?

David C.

Numerade Educator

01:29

Problem 119

Nitric acid is usually purchased in concentrated form with
a $70.3 \%$ HNO $_{3}$ concentration by mass and a density of 1.41 $\mathrm{g} / \mathrm{mL} .$ How much of the concentrated stock solution in milliliters should you use to make 2.5 L of $0.500 \mathrm{M} \mathrm{HNO}_{3} ?$

David C.

Numerade Educator

01:03

Problem 120

Hydrochloric acid is usually purchased in concentrated form with a $37.0 \%$ HCl concentration by mass and a density of $1.20 \mathrm{g} / \mathrm{mL} .$ How much of the concentrated stock solution in milliliters should you use to make $2.5 \mathrm{L}$ of $0.500 \mathrm{M} \mathrm{HCl} ?$

David C.

Numerade Educator

01:39

Problem 121

An ethylene glycol solution is made using $58.5 \mathrm{g}$ of ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ and diluting to a total volume of 500.0 mL. Calculate the freezing point and boiling point of the solution. (Assume a density of $1.09 \mathrm{g} / \mathrm{mL}$ for the solution.)

David C.

Numerade Educator

01:31

Problem 122

A sucrose solution is made using $144 \mathrm{g}$ of sucrose $\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)$ and diluting to a total volume of 1.00 L. Calculate the freezing point and boiling point of the solution. (Assume a density of $1.06 \mathrm{g} / \mathrm{mL}$ for the final solution.)

David C.

Numerade Educator

03:13

Problem 123

A 250.0 -mL sample of a $5.00 \mathrm{M}$ glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ solution is diluted to 1.40 L. What are the freezing and boiling points of the final solution? (Assume a density of 1.06 $\mathrm{g} / \mathrm{mL}$ for the final solution.)

David C.

Numerade Educator

03:06

Problem 124

A 135 -mL sample of a $10.0 \mathrm{M}$ ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ solution is diluted to 1.50 L. What are the freezing and boiling points of the final solution? (Assume a density of $1.05 \mathrm{g} / \mathrm{mL}$ for the final solution.)

David C.

Numerade Educator

01:17

Problem 125

An aqueous solution containing $17.5 \mathrm{g}$ of an unknown molecular (nonelectrolyte) compound in $100.0 \mathrm{g}$ of water has a freezing point of $-1.8^{\circ} \mathrm{C}$. Calculate the molar mass of the unknown compound.

Amy J.

Numerade Educator

05:03

Problem 126

An aqueous solution containing $35.9 \mathrm{g}$ of an unknown molecular (nonelectrolyte) compound in $150.0 \mathrm{g}$ of water has a freezing point of $-1.3^{\circ} \mathrm{C}$. Calculate the molar mass of the unknown compound.

Qiao R.

Numerade Educator

Problem 127

What is the boiling point of an aqueous solution that freezes at $-6.7^{\circ} \mathrm{C} ?$

David C.

Numerade Educator