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World of Chemistry

Steven S.Zumdahl, Susan L.Zumdahl, Donald J.DeCoste

Chapter 15

Solutions - all with Video Answers

Educators

Chapter Questions

01:43

Problem 1

Explain why a solution is a homogeneous mixture. Give two examples of homogeneous mixtures.

Marissa Turner
Marissa Turner
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00:52

Problem 2

In a solution, the substance present in the largest amount is called the ______ , whereas the other substances present are called the _______.

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Marissa Turner
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02:00

Problem 3

Discuss how an ionic solute dissolves in water. How are the strong interionic forces in the solid overcome to permit the solid to dissolve? How are the dissolved positive and negative ions shielded from one another, preventing them from recombining to form the solid?

SH
Shanie Holman
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01:42

Problem 4

Why are some molecular solids (such as sugar or ethyl alcohol) soluble in water, while other molecular solids (such as petroleum) are insoluble in water? What structural features(s) of some molecular solids may tend to make them soluble in water?

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00:54

Problem 5

A solution that contains as much solute as will dissolve at a given temperature is said to be ________.

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Marissa Turner
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01:04

Problem 6

A solution that has not reached its limit of dissolved solute is said to be ______.

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Marissa Turner
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01:28

Problem 7

A solution is a homogeneous mixture and, unlike a compound, has ______ composition.

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Marissa Turner
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01:27

Problem 8

The label "concentrated $\mathrm{H}_{2} \mathrm{SO}_{4}^{\prime \prime}$ on a bottle means that there is a relatively ______ amount of $\mathrm{H}_{2} \mathrm{SO}_{4}$ present in the solution.

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Marissa Turner
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01:05

Problem 9

What does it mean to increase the surface area of a solid? Explain why this change causes an increase in the rate of dissolving.

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Marissa Turner
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00:55

Problem 10

Use a molecular explanation to explain why increasing the temperature speeds up the rate of dissolving a solid in a liquid.

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Marissa Turner
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01:03

Problem 11

Explain why the solubility of a gas generally decreases with an increase in temperature.

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Marissa Turner
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04:15

Problem 12

Calculate the mass percent of calcium chloride in each of the following solutions.
a. 5.00 g of calcium chloride in 95.0 $\mathrm{g}$ of water
b. 1.00 $\mathrm{g}$ of calcium chloride in 19.0 $\mathrm{g}$ of water
c. 15.0 $\mathrm{g}$ of calcium chloride in 285 $\mathrm{g}$ of water
d. 2.00 $\mathrm{mg}$ of calcium chloride in 0.0380 $\mathrm{g}$ of water

Marissa Turner
Marissa Turner
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03:33

Problem 13

Calculate the mass, in grams, of NaCl present in each of the following solutions.
a. 11.5 g of 6.25$\%$ NaCl solution
b. 6.25 g of 11.5$\%$ NaCl solution
c. 54.3 g of 0.91$\%$ NaCl solution
d. 452 g of 12.3$\%$ NaCl solution

Marissa Turner
Marissa Turner
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01:43

Problem 14

A laboratory assistant prepared a potassium chloride solution for her class by dissolving 5.34 g of $\mathrm{KCl}$ in 152 $\mathrm{g}$ of water. What is the mass percent of the solution she prepared?

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01:27

Problem 15

If 67.1 g of $\mathrm{CaCl}_{2}$ is added to 275 $\mathrm{g}$ of water, calculate the mass percent of $\mathrm{CaCl}_{2}$ in the solution.

Marissa Turner
Marissa Turner
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02:19

Problem 16

What mass of each solute is present in 285 g of a solution that contains 5.00$\%$ by mass $\mathrm{NaCl}$ and 7.50$\%$ by mass $\mathrm{Na}_{2} \mathrm{CO}_{3} ?$

Marissa Turner
Marissa Turner
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03:02

Problem 17

A hexane solution contains as impurities 5.2$\%$ (by mass) heptane and 2.9$\%$ (by mass) pentane.
Calculate the mass of each component present in 93 g of the solution.

Marissa Turner
Marissa Turner
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01:04

Problem 18

A solution that is labeled "0.105 $M \mathrm{NaOH}^{\prime \prime}$ would contain _______ mol of NaOH per liter of solution.

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01:10

Problem 19

How many moles of each ion are present, per liter, in a solution that is labeled "0.221 $M$ $\mathrm{CaCl}_{2}^{\prime \prime \prime}$

Marissa Turner
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01:09

Problem 20

If you were to prepare exactly 1.00 $\mathrm{L}$ of a 5 $\mathrm{M}$ NaCl solution, you would not need exactly 1.00 $\mathrm{L}$ of water. Explain.

Marissa Turner
Marissa Turner
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02:26

Problem 21

For each of the following solutions, the number of moles of solute is given, followed by the total volume of solution prepared. Calculate the molarity.
a. 0.50 mol $\mathrm{KBr} ; 250 \mathrm{mL}$
b. 0.50 mol $\mathrm{KBr} ; 500 . \mathrm{mL}$
c. 0.50 mol $\mathrm{KBr} ; 750 \mathrm{mL}$
d. 0.50 mol $\mathrm{KBr} ; 1.0 \mathrm{L}$

Marissa Turner
Marissa Turner
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09:42

Problem 22

For each of the following solutions, the mass of the solute is given, followed by the total volume of the solution prepared. Calculate the molarity.
a. $4.25 \mathrm{g} \mathrm{CuCl}_{2} ; 125 \mathrm{mL}$
b. $0.101 \mathrm{g} \mathrm{NaHCO}_{3} ; 11.3 \mathrm{mL}$
c. $52.9 \mathrm{g} \mathrm{Na}_{2} \mathrm{CO}_{3} ; 1.15 \mathrm{L}$
d. $0.14 \mathrm{mg} \mathrm{KOH} ; 1.5 \mathrm{mL}$

Marissa Turner
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03:08

Problem 23

If a $45.3-$ -g sample of potassium nitrate is dissolved in enough water to make 225 $\mathrm{mL}$ of
solution, what will be the molarity?

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02:10

Problem 24

An alcoholic iodine solution (“tincture” of iodine) is prepared by dissolving 5.15 g of iodine crystals in enough alcohol to make a volume of 225 mL. Calculate the molarity of iodine in the solution.

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04:01

Problem 25

Suppose 1.01 $\mathrm{g}$ of $\mathrm{FeCl}_{3}$ is placed in a 10.0$\cdot \mathrm{mL}$ volumetric flask, water is added, the mixture is shaken to dissolve the solid, and then water is added to the calibration mark of the flask. Calculate the molarity of each ion present in the solution.

Marissa Turner
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01:31

Problem 26

If 495 g of $\mathrm{NaOH}$ is dissolved to a final total volume of $20.0 \mathrm{L},$ what is the molarity of the solution?

Anand Jangid
Anand Jangid
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06:07

Problem 27

Calculate the number of moles and the number of grams of the indicated solutes present in each
of the following solution samples.
(TABLE IS NOT AVAILABLE TO COPY)

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02:02

Problem 28

What mass (in grams) of $\mathrm{NH}_{4} \mathrm{Cl}$ is needed to prepare $450 . \mathrm{mL}$ of 0.251 $\mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}$ solution?

Marissa Turner
Marissa Turner
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07:15

Problem 29

Calculate the number of moles of each ion present in each of the following solutions.
a. 10.2 $\mathrm{mL}$ of 0.451 $\mathrm{M} \mathrm{AlCl}_{3}$ solution
b. 5.51 $\mathrm{L}$ of 0.103 $\mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}$ solution
c. 1.75 $\mathrm{mL}$ of 1.25 $\mathrm{M} \mathrm{CuCl}_{2}$ solution
d. 25.2 $\mathrm{mL}$ of 0.00157 $\mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}$ solution

Marissa Turner
Marissa Turner
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01:56

Problem 30

Standard silver nitrate solutions are used in the analysis of samples containing chloride ion. How many grams of silver nitrate are needed to prepare $250 . \mathrm{mL}$ of a 0.100 $\mathrm{M} \mathrm{AgNO}_{3}$ solution?

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07:57

Problem 31

Calculate the new molarity that results when 250. mL of water is added to each of the following solutions.
a. 125 $\mathrm{mL}$ of 0.251 $\mathrm{MCl}$
b. 445 $\mathrm{mL}$ of 0.499 $\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$
c. 5.25 $\mathrm{L}$ of 0.101 $\mathrm{M} \mathrm{HNO}_{3}$
d. 11.2 $\mathrm{mL}$ of 14.5 $\mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$

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05:50

Problem 32

Many laboratories keep bottles of 3.0 $\mathrm{M}$ solutions of the common acids on hand. Given the following molarities of the concentrated acids, determine how many milliliters of each concentrated acid
would be required to prepare 225 $\mathrm{mL}$ of a 3.0 $\mathrm{M}$ solution of the acid.
(TABLE IS NOT AVAILABLE TO COPY)

Marissa Turner
Marissa Turner
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01:59

Problem 33

A chemistry student needs 125 $\mathrm{mL}$ of 0.150 $\mathrm{M}$
NaOH solution for an experiment, but the only solution available in the laboratory is 3.02 $\mathrm{M}$ .
Describe how the student could prepare the solution he needs.

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02:42

Problem 34

How much water must be added to 500 . mL of 0.200$M$ HCl to produce a 0.150 M solution?
(Assume that the volumes are additive.)

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02:10

Problem 35

One way to determine the amount of chloride ion in a water sample is to react the sample with standard $\mathrm{AgNO}_{3}$ solution to produce solid AgCl.
$$\mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \operatorname{AgCl}(s)$$
If a 25.0 -mL. water sample requires 27.2 $\mathrm{mL}$ of 0.104 $\mathrm{M} \mathrm{AgNO}_{3}$ in such a reaction, what is the concentration of $\mathrm{Cl}^{-}$ in the sample?

Marissa Turner
Marissa Turner
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02:29

Problem 36

What volume (in mL) of 0.25 $\mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$ solution is needed to precipitate all the barium, as $\mathrm{BaSO}_{4}(s),$ from 12.5 $\mathrm{mL}$ of 0.15 $\mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ solution?
$$
\begin{array}{l}{\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) \rightarrow} \\ {\quad \mathrm{BaSO}_{4}(s)+2 \mathrm{NaNO}_{3}(a q)}\end{array}
$$

Marissa Turner
Marissa Turner
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02:52

Problem 37

If 36.2 $\mathrm{mL}$ of 0.158 $\mathrm{M} \mathrm{CaCl}_{2}$ solution is added to 37.5 $\mathrm{mL}$ of $0.149 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3},$ what mass of calcium carbonate, $\mathrm{CaCO}_{3},$ will be precipitated? The reaction is
$$
\begin{array}{l}{\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow} \\ {\quad \mathrm{CaCO}_{3}(s)+2 \mathrm{NaCl}(a q)}\end{array}
$$

Marissa Turner
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03:20

Problem 38

When aqueous solutions of lead(II) ion are treated with potassium chromate solution, a bright yellow precipitate of lead(II) chromate, $\mathrm{PbCrO}_{4}$ , forms. How many grams of lead chromate form when a $1.00-\mathrm{g}$ sample of $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$ is added to 25.0 $\mathrm{mL}$ of 1.00 $\mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}$ solution?

Marissa Turner
Marissa Turner
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02:16

Problem 39

What volume of 0.200 $\mathrm{M}$ HCl solution is needee to neutralize 25.0 $\mathrm{mL}$ of 0.150 $\mathrm{M} \mathrm{NaOH}$ solution?

Marissa Turner
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01:54

Problem 40

The concentration of a sodium hydroxide solution is to be determined. A 50.0-mL sample of 0.104 M HCl solution requires 48.7 mL of the sodium hydroxide solution to reach the point of neutralization. Calculate the molarity of the NaOH solution.

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03:40

Problem 41

What volume of 1.00 $\mathrm{M} \mathrm{NaOH}$ is required to neutralize each of the following solutions?
a. 25.0 $\mathrm{mL}$ of 0.154 $\mathrm{M}$ acetic acid, $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$
b. 35.0 $\mathrm{mL}$ of 0.102 $\mathrm{M}$ hydrofluoric acid, HF
c. 10.0 $\mathrm{mL}$ of 0.143 $\mathrm{M}$ phosphoric acid,
$\mathrm{H}_{3} \mathrm{PO}_{4}$
d. 35.0 $\mathrm{mL}$ of 0.220 $\mathrm{M}$ sulfuric acid, $\mathrm{H}_{2} \mathrm{SO}_{4}$

Marissa Turner
Marissa Turner
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00:42

Problem 42

Explain why the equivalent weight of $\mathrm{H}_{2} \mathrm{SO}_{4}$ is half the molar mass of this substance. How many hydrogen ions does each $\mathrm{H}_{2} \mathrm{SO}_{4}$ molecule produce when reacting with an excess of OH- ions?

Marissa Turner
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00:59

Problem 43

How many equivalents of hydroxide ion are needed to react with 1.53 equivalents of hydrogen ion? How can you tell when no balanced chemical equation is given for the reaction?

Marissa Turner
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05:49

Problem 44

For each of the following solutions, the mass of solute taken is indicated, along with the total volume of solution prepared. Calculate the normality of each solution.
$\begin{array}{ll}{\text { a. } 113 \mathrm{g} \mathrm{NaOH} ;} & {10.2 \mathrm{mL}} \\ {\text { b. } 12.5 \mathrm{mg} \mathrm{Ca}(\mathrm{OH})_{2} ;} & {100 . \mathrm{mL}} \\ {\text { c. } 12.4 \mathrm{g} \mathrm{H}_{2} \mathrm{SO}_{4} ;} & {155 \mathrm{mL}}\end{array}$

Marissa Turner
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01:33

Problem 45

Calculate the normality of each of the following solutions.
a. 0.134 $\mathrm{M} \mathrm{NaOH}$
b. 0.00521 $\mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}$
c. 4.42 $\mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}$

Marissa Turner
Marissa Turner
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02:04

Problem 46

A solution of phosphoric acid, $\mathrm{H}_{3} \mathrm{PO}_{4}$ , is found to contain 35.2 $\mathrm{g}$ of $\mathrm{H}_{3} \mathrm{PO}_{4}$ per liter of solution. Calculate the molarity and normality of the solution.

Marissa Turner
Marissa Turner
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02:15

Problem 47

What volume of 0.172 $\mathrm{N} \mathrm{H}_{2} \mathrm{SO}_{4}$ is required to neutralize 56.2 $\mathrm{mL}$ of 0.145 $\mathrm{M} \mathrm{NaOH} ?$

Marissa Turner
Marissa Turner
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02:36

Problem 48

What volume of 0.151 $\mathrm{N} \mathrm{NaOH}$ is required to neutralize 24.2 $\mathrm{mL}$ of 0.125 $\mathrm{N} \mathrm{H}_{2} \mathrm{SO}_{4} ?$ What volume of 0.151 $\mathrm{N} \mathrm{NaOH}$ is required to neutralize 24.1 $\mathrm{mL}$ of 0.125 $\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4} ?$

Marissa Turner
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00:40

Problem 49

What is meant by the term “colligative property”?

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00:41

Problem 50

Explain on a molecular level why the increase in boiling point is a colligative property.

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00:38

Problem 51

Antifreeze that you use in your car could also be called “antiboil.” Explain why.

Marissa Turner
Marissa Turner
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05:47

Problem 52

Suppose 50.0 $\mathrm{mL}$ of 0.250 $\mathrm{M} \mathrm{CoCl}_{2}$ solution is added to 25.0 $\mathrm{mL}$ of 0.350 $\mathrm{M} \mathrm{NiCl}_{2}$ solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive.

Marissa Turner
Marissa Turner
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04:18

Problem 53

Calculate the mass of AgCl formed, and the concentration of silver ion remaining in solution, when 10.0 g of solid $\mathrm{AgNO}_{3}$ is added to 50. mL of $1.0 \times 10^{-2} \mathrm{M}$ NaCl solution. Assume there is no volume change upon addition of the solid.

Marissa Turner
Marissa Turner
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02:19

Problem 54

What mass of BaSO $_{4}$ will be precipitated from a large container of concentrated Baa $\mathrm{NO}_{3} )_{2}$ solution if 37.5 $\mathrm{mL}$ of 0.221 $\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ is added?

Marissa Turner
Marissa Turner
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02:04

Problem 55

Strictly speaking, the solvent is the component of a solution that is present in the largest amount on a mole basis. For solutions involving water, water is almost always the solvent because there tend to be many more water molecules present than molecules of any conceivable solute. To see why this is so, calculate the number of moles of water present in 1.0 $\mathrm{L}$ of water. Recall that the density of water is very nearly 1.0 $\mathrm{g} / \mathrm{mL}$ under most conditions.

Marissa Turner
Marissa Turner
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02:32

Problem 56

A $14.2-$ g sample of $\mathrm{CaCl}_{2}$ is added to a $50.0-\mathrm{mL}$ volumetric flask. After dissolving the salt, water is added to the calibration mark of the flask. Calculate the molarity of the solution.

Marissa Turner
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06:04

Problem 57

Calculate the new molarity when 150. mL of water is added to each of the following solutions.
a. 125 $\mathrm{mL}$ of 0.200 $\mathrm{M} \mathrm{HBr}$
b. 155 $\mathrm{mL}$ of 0.250 $\mathrm{M} \mathrm{Ca}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}$
c. 0.500 $\mathrm{L}$ of 0.250 $\mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}$
d. 15 $\mathrm{mL}$ of 18.0 $\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$

Marissa Turner
Marissa Turner
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02:34

Problem 58

Calculate the normality of each of the following solutions.
a. 0.50 $\mathrm{M}$ acetic acid, $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$
b. 00250 $\mathrm{M}$ sulfuric acid, $\mathrm{H}_{2} \mathrm{SO}_{4}$
c. 0.10 $\mathrm{M}$ potassium hydroxide, $\mathrm{KOH}$

David Collins
David Collins
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02:09

Problem 59

If 27.5 $\mathrm{mL}$ of $3.5 \times 10^{-2} \mathrm{N} \mathrm{Ca}(\mathrm{OH})_{2}$ solution
is needed to neutralize 10.0 $\mathrm{mL}$ of nitric acid solution of unknown concentration, what is
the normality of the nitric acid?

Marissa Turner
Marissa Turner
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02:37

Problem 60

The figures below are molecular-level representations of four aqueous solutions of the same solute. Arrange the solutions from most to least concentrated.
(IMAGE IS NOT AVAILABLE TO COPY)

Marissa Turner
Marissa Turner
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