Deck 15: Solutions

Question 1

You have 250.0 mL of 4.00 M sugar solution. You add 376.3 mL of water to this solution. Determine the concentration of the sugar solution after the water has been added.

A) 4.00 M
B) 1.85 M
C) 2.34 M
D) 1.60 M
E) 1.93 M

Answer 1

1.60 M

Question 2

Which of the following aqueous solutions contains the greatest number of ions in solution?

A) 2.0 L of 2.00 M sodium phosphate
B) 2.0 L of 2.00 M magnesium chloride
C) 3.0 L of 2.00 M sodium bromide
D) 2.0 L of 2.50 M sodium chloride
E) 1.0 L of 4.00 M potassium carbonate

Answer 2

2.0 L of 2.00 M sodium phosphate

Question 3

You have 100.0 mL of a 0.2500 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it is now 0.4142M. How much water must have evaporated?

A) 60.4 mL
B) 39.6 mL
C) 16.4 mL
D) 100.0 mL
E) The concentration will not change because of evaporation.

Answer 3

39.6 mL

Question 4

You have 25.00 mL of a 0.1000 M sugar solution. How much water must be added to make a 0.01809M solution?

A) 138.2 mL
B) 4.52 mL
C) 20.5 mL
D) 113.2 mL
E) 45.2 mL

Question 5

A nitric acid solution containing 71.0% HNO₃ (by mass) has a density of 1.42 g/mL. How many moles of HNO₃ are present in 2.36 L of this solution?

A) 74.9 mol
B) 37.8 mol
C) 26.6 mol
D) mol
E) none of these

Question 6

Determine the concentration of a solution made by dissolving 31.6 g of sodium chloride in 750.0 mL of solution.

A) 0.406 M
B) 42.1 M
C) 0.541 M
D) 0.721 M
E) 23.7 M

Question 7

What term is used by chemists to quantitatively describe a solution in which a relatively small amount of solute is dissolved?

A) dilute
B) saturated
C) supersaturated
D) concentrated
E) unsaturated

Question 8

One mole of each of the following compounds is added to water in separate flasks to make 1.0 L of solution in each flask. Which flask has the largest total ion concentration?

A) sodium phosphate
B) barium sulfate
C) silver chloride
D) calcium hydroxide
E) sodium bromide

Question 9

A nitric acid solution that is 80.0% HNO₃ (by mass) contains

A) 80.0 g HNO₃ and 100.0 g water
B) 80.0 g HNO₃ and 20.0 g water
C) 80.0 mol HNO₃
D) 80.0 g HNO₃ and 80.0 g water
E) none of these

Question 10

What is the minimum volume of a 3.88 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?

A) 42.9 mL
B) 375 mL
C) mL
D) 15.5 mL
E) 30.9 mL

Question 11

Calculate the concentration of chloride ions when 100.0 mL of 0.205 M sodium chloride is mixed with 250.0 mL of 0.150 M calcium chloride.

A) 0.955 M
B) 0.382 M
C) 0.273 M
D) M
E) none of these

Question 12

You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 5.00 M solution. You have much more of the 5.00 M solution, and you add the solutions together. Which of the following could be the concentration of the final solution?

A) 4.80 M
B) 3.50 M
C) 2.90 M
D) 7.00 M
E) 7.20 M

Question 13

A mixture of sand and water is a(n) ______________.

A) solution
B) solvent
C) solute
D) aqueous solution
E) none of these

Question 14

A solution is prepared by dissolving 8.29 g of Na₂SO₄ in enough water to make 225 mL of solution. Calculate the solution molarity.

A) 0.0584 M
B) 1.87 M
C) 0.603 M
D) 0.259 M
E) 0.484 M

Question 15

Approximately 38 g of NaCl can be dissolved in 100 g of water at 25°C. A solution prepared by adding 35 g of NaCl to 100 g of water at 25°C is unsaturated.

Question 16

When a solvent has dissolved all the solute it can at a particular temperature, it is said to be

A) diluted
B) unsaturated
C) supersaturated
D) saturated
E) none of these

Question 17

If you mix 20.0 mL of a 3.00 M sugar solution with 30.0 mL of a 5.57 M sugar solution, you will end up with a sugar solution of ________.

A) 4.29 M
B) 0.171 M
C) 7.57 M
D) 4.54 M
E) 11.36 M

Question 18

In soda pop, CO₂(g) is a ______________, and water is the ______________.

A) solute; solvent
B) solvent; solute
C) solution; solute
D) solute; solution
E) solvent; solution

Question 19

An oven-cleaning solution is 40.0% (by mass) NaOH. If one jar of this product contains 457.0 g of solution, how much NaOH does it contain?

A) g
B) 11.4 g
C) 183 g
D) 18.3 g
E) none of these

Question 20

A 116.9-g sample of nitric acid solution that is 70.0% HNO₃ (by mass) contains

A) 81.8 mol HNO₃
B) 1.30 mol HNO₃
C) 1.86 mol HNO₃
D) mol HNO₃
E) none of these

Question 21

A 0.216-g sample of NaCl (molar mass = 58.44 g/mol) is dissolved in enough water to make 5.20 mL of solution. Calculate the molarity of the resulting solution.

A) 0.711 M
B) M
C) 0.823 M
D) 1.41 M
E) 0.567 M

Question 22

What volume of a 0.176 M Na₂S solution contains 1.01 g of Na⁺ ions?

A) 0.250 L
B) 8.01 L
C) 4.01 L
D) 0.425 L
E) 0.125 L

Question 23

A 27.9-g sample of HF is dissolved in enough water to give 2.0 * 10² mL of solution. The concentration of the solution is

A) 27.9 M
B) 1.39 M
C) 0.28 M
D) 7.0 M
E) 5.58 M

Question 24

What mass of solute is contained in 64.9 mL of a 2.00 M sodium bromide solution?

A) 13.4 g
B) 3.34 g
C) 0.0649 g
D) 0.130 g
E) 0.206 g

Question 25

What volume of 18.0 M sulfuric acid is required to prepare 26.2 L of 0.126 M H₂SO₄?

A) 5.45 mL
B) 0.183 L
C) 472 mL
D) 3.30 L
E) 208 mL

Question 26

To make 98.1 mL of a 0.405 M solution of NaCl, what mass of NaCl is required?

A) 39.7 g
B) 14.2 g
C) 2.32 g
D) 4.14 g
E) none of these

Question 27

How many grams of NaCl are contained in 350. mL of a 0.238 M solution of sodium chloride?

A) 83.3 g
B) 4.87 g
C) 13.9 g
D) 1.43 g
E) none of these

Question 28

What mass of solute is contained in 27.9 mL of a 1.56 M potassium bromide solution?

A) 17.9
B) 5.18
C) 43.5
D) 2.73
E) none of these

Question 29

Calculate the molarity of a solution prepared by dissolving 6.24 g of NaI in enough water to prepare 312 mL of solution.

A) M
B) M
C) 1.95 M
D) 20.0 M
E) M

Question 30

What mass of solute is contained in 256 mL of a 0.909 M ammonium chloride solution?

A) 12.4 g
B) 48.6 g
C) 0.282 g
D) 233 g
E) none of these

Question 31

What volume of a 0.550 M solution of potassium hydroxide can be made with 14.3 g of potassium hydroxide? (Ignore significant figures for this problem.)

A) 26.0 mL
B) 463 mL
C) 255 mL
D) 2158 mL
E) 2.16 mL

Question 32

A chemist needs 225 mL of 3.1 M HCl. What volume of 12 M HCl must be dissolved in water to form this solution? (Ignore significant figures for this problem.)

A) mL
B) 15 mL
C) 6.0 mL
D) 17 mL
E) 58 mL

Question 33

A 71.08-g sample of NaCl is dissolved in 250.0 mL of solution. Calculate the molarity of this solution.

A) 1.216 M
B) 284.3 M
C) 4.865 M
D) 6.098 M
E) none of these

Question 34

How many grams of CaCl₂ (molar mass = 111.0 g/mol) are needed to prepare 5.17 L of 0.500 M CaCl₂ solution?

A) 299 g
B) 287 g
C) 312 g
D) 410 g
E) 337 g

Question 35

What mass of solute is contained in 417 mL of a 0.151 M magnesium fluoride solution?

A) 3.92 g
B) 63 g
C) 9.4 g
D) 1.01 g
E) none of these

Question 36

A 47.7-g sample of SrCl₂ is dissolved in 112.5 mL of solution. Calculate the molarity of this solution.

A) 0.301 M
B) 2.67 M
C) 0.0339 M
D) 3.99 M
E) none of these

Question 37

What mass of calcium chloride, CaCl₂, is needed to prepare 2.657 L of a 1.56 M solution?

A) 4.14 g
B) 313 g
C) 189 g
D) 65.2 g
E) 460 g

Question 38

A 14.8-g sample of potassium sulfate is dissolved in 350.0 mL of solution. Calculate the molarity of this solution.

A) 11.8 M
B) 5.18 M
C) 0.0297 M
D) 0.243 M
E) none of these

Question 39

The molarity of Cl^- in 110. mL of a solution containing 3.22 g of CaCl₂ is

A) 0.264 M
B) 0.0290 M
C) 0.00319 M
D) 0.528 M
E) 0.354 M

Question 40

Calculate the mass of silver nitrate (in grams) in a 145 mL solution of 4.26 M AgNO₃. (Ignore significant figures for this problem.)

A) 0.724 g
B) 105 g
C) 34.0 g
D) 724 g
E) none of these

Question 41

To prepare 20.0 mL of a 2.00 M solution of hydrochloric acid from a 10.0 M stock solution, you should take 4.00 mL of the stock solution and add 20.0 mL of water.

Question 42

You mix 100.0 mL of a 0.100 M NaOH solution and 150.0 mL of a 0.104 M HCl solution. Determine the concentration of H⁺ in the final mixture after the reaction is complete.

A) 0.0624 M
B) 0.104 M
C) 0.156 M
D) 0.204 M
E) 0.0224 M

Question 43

You have 3.00 L of a 3.48 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO₃(aq) called solution B. You mix these solutions together, making solution C. Calculate the concentration (in M) of Na⁺ ions in solution C.

A) 0 M
B) 3.48 M
C) 5.22 M
D) 1.10 M
E) 2.09 M

Question 44

You have 3.00 L of a 3.67 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO₃(aq) called solution B. You mix these solutions together, making solution C. Calculate the concentration (in M) of Ag⁺ ions in solution C.

A) 0 M
B) 1.40 M
C) 2.20 M
D) 0.800 M
E) 3.51 M

Question 45

Calculate the volume of 0.164 M HNO₃ required to neutralize 25.0 mL of 0.250 M NaOH.

A) 16.4 mL
B) 38.1 mL
C) 4.10 mL
D) 26.2 mL
E) none of these

Question 46

What volume of 17.4 M H₂SO₄ is required to prepare 12.0 L of 0.156 M sulfuric acid? (Ignore significant figures for this problem.)

A) 226 mL
B) 2.71 L
C) 112 mL
D) 108 mL
E) 1.34 L

Question 47

What volume of 12.0 M nitric acid is required to prepare 6.71 L of 0.100 M nitric acid?

A) 0.179 L
B) 17.9 L
C) 0.671 L
D) 0.0559 L
E) 1.79 L

Question 48

You have 3.00 L of a 3.77 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO₃(aq) called solution B. You mix these solutions together, making solution C. Calculate the concentration (in M) of Cl^- ions in solution C.

A) 0 M
B) 2.26 M
C) 1.46 M
D) 2.44 M
E) 0.800 M

Question 49

Magnesium metal reacts with hydrochloric acid to form magnesium chloride and hydrogen gas. Suppose we react an excess of magnesium metal with 19.8 mL of a 3.00 M solution of hydrochloric acid and collect all of the hydrogen in a balloon at 25^oC and 1.00 atm. What is the expected volume of the balloon?

A) 0.0609 L
B) 0.726 L
C) 1.45 L
D) 0.323 L
E) 60.9 L

Question 50

You have 3.00 L of a 3.00 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 1.84 M solution of AgNO₃(aq) called solution B. You mix these solutions together, making solution C. Calculate the concentration (in M) of ions in solution C.

A) 0 M
B) 0.736 M
C) 1.06 M
D) 1.84 M
E) 1.80 M

Question 51

If you mix 40.0 mL of a 0.389 M solution of K₂CrO₄ with 40.0 mL of a 0.389 M solution of AgNO₃, what mass of solid forms?

A) 5.16 g
B) 2.58 g
C) 3.02 g
D) 15.6 g
E) 7.78 g

Question 52

What is the normality of 1.00 L of a sodium hydroxide solution that contains 18.2 g of NaOH?

A) 2.20 N
B) 18.2 N
C) 0.228 N
D) 0.455 N
E) none of these

Question 53

In the following acid-base neutralization, 1.61 g of the solid acid HC₆H₅O neutralized 11.61 mL of aqueous NaOH solution base by the reaction NaOH(aq) + HC₆H₅O(aq) $\rightarrow$ H₂O(l) + NaC₆H₅O(aq)
Calculate the molarity of the base solution.

A) 1.47 M
B) 17.1 M
C) 7.21 M
D) 0.139 M
E) 0.199 M

Question 54

Determine the normality of a base if 93.0 mL of 1.8 M HCl is required to neutralize 52.0 mL of it.

A) 1.01 N
B) 0.31 N
C) 1.0 N
D) 94 N
E) 3.2 N

Question 55

Calculate the volume of 0.581 M KOH required to neutralize 150. mL of 0.100 M HCl.

A) 87.2 mL
B) 25.8 mL
C) 872 mL
D) 38.7 mL
E) none of these

Question 56

You have two HCl solutions, labeled solution A and solution B. Solution A has a greater concentration than solution B. Which of the following statements is/are true?

A) If you have equal volumes of both solutions, solution B must contain more moles of HCl.
B) If you have equal moles of HCl in both solutions, solution B must have a greater volume.
C) To obtain equal concentrations of both solutions, you must add a certain amount of water to solution B.
D) Adding more moles of HCl to both solutions will make them less concentrated.
E) At least two of the above statements are true.

Question 57

What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.121 M H₂SO₄? (Ignore significant figures for this problem.)

A) 104 mL
B) 141 mL
C) 1.88 L
D) 128.1 mL
E) none of these

Question 58

For the reaction between 200.0 mL of 0.100 M silver nitrate and 95.00 mL of 0.100 M sodium chloride, the concentration of silver ions in solution after the reaction is complete is

A) 0.00 M. All of the silver ions are used up to make the precipitate.
B) 0.100 M. The silver ions do not participate in the chemical reaction and are considered spectator ions.
C) greater than 0.100 M. For every 1.0 mol of silver nitrate there are 2.0 mol of silver ions in solution.
D) less than 0.100 M. Even though silver ions do not react, they are diluted when mixed with the sodium chloride solution.
E) less than 0.100 M. Some, but not all, of the silver ions are used to make the precipitate.

Question 59

Assume that vinegar is a 0.852 M solution of acetic acid (HC₂H₃O₂) in water. What volume of 0.2136 M NaOH would be needed to completely neutralize 6.89 mL of vinegar?

A) 5.87 mL
B) 1.47 mL
C) 1.73 mL
D) 27.5 mL
E) 4.00 mL

Question 60

A 50.93-g sample of Ba(OH)₂ is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 M Ba(OH)₂?

A) 61.1 mL
B) 248 mL
C) 297 mL
D) 509 mL
E) 404 mL

Question 61

You have three sodium carbonate solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M sodium carbonate. Solution 1 contains 148.6 mL of the 3.00 M solution.
Solution 2 contains 58.2 mL of the 3.00 M solution.
Solution 3 contains 33.4 mL of the 3.00 M solution.
How many moles of ions does Solution 1 contain?

A) 1.34 mol
B) 0.446 mol
C) mol
D) 0.892 mol
E) 0.669 mol

Question 62

You have three sodium carbonate solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M sodium carbonate. Solution 1 contains 100.0 mL of the 3.00 M solution.
Solution 2 contains 50.0 mL of the 3.00 M solution.
Solution 3 contains 10.0 mL of the 3.00 M solution.
What is the new concentration of Solution 2 if 13.2 g of solid sodium carbonate is added and dissolved? (Assume no volume change.)

A) 2.49 M
B) 11.5 M
C) 1.72 M
D) 5.49 M
E) 0.549 M

Question 63

You have three ammonium sulfate solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M ammonium sulfate. Solution 1 contains 127.2 mL of the 3.00 M solution.
Solution 2 contains 68.7 mL of the 3.00 M solution.
Solution 3 contains 32.4 mL of the 3.00 M solution.
How many moles of ions does Solution 2 contain?

A) 0.206 mol
B) 1.44 mol
C) 0.618 mol
D) 0.412 mol
E) 0.309 mol

Question 64

If a 74.6-g sample of ammonium nitrate is dissolved in enough water to make 315 mL of solution, what will be the molarity?

A) 0.932 M
B) 2.96 M
C) 0.294 M
D) 3.41 M
E) none of these

Question 65

What mass of solute is contained in 50.0 mL of a 1.49 M potassium chloride solution?

A) 33.6 g
B) 2.50 g
C) 74.5 g
D) 5.55 g
E) 50.0 g

Question 66

You have three ammonium chloride solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M ammonium chloride. Solution 1 contains 124.6 mL of the 3.00 M solution.
Solution 2 contains 52.9 mL of the 3.00 M solution.
Solution 3 contains 21.3 mL of the 3.00 M solution.
How many moles of ions does Solution 3 contain?

A) 0.128 mol
B) 0.192 mol
C) 0.320 mol
D) 0.0639 mol
E) 0.0320 mol

Question 67

You have a 16.0-oz. (473-mL) glass of lemonade with a concentration of 2.89 M. The lemonade sits out on your counter for a couple of days, and 150. mL of water evaporates from the glass. What is the new concentration of the lemonade?

A) 9.11 M
B) 6.11 M
C) 4.23 M
D) 0.164 M
E) 19.3 M

Question 68

Which of the following solutions contains the smallest number of ions?

A) 539.8 mL of 1.0 M lithium nitrate
B) 305.6 mL of 2.0 M potassium hydroxide
C) 189.6 mL of 2.0 M iron(III) chloride
D) 246.8 mL of 1.0 M sodium sulfate
E) At least two of the above contain the smallest number of ions.

Question 69

How many moles of chloride ions are in 56.7 mL of a 2.00 M aluminum chloride solution?

A) 0.113 mol
B) 0.0284 mol
C) 0.0378 mol
D) 0.680 mol
E) 0.340 mol

Question 70

You have three sodium carbonate solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M sodium carbonate. Solution 1 contains 100.0 mL of the 3.00 M solution.
Solution 2 contains 50.0 mL of the 3.00 M solution.
Solution 3 contains 10.0 mL of the 3.00 M solution.
What volume of water (in mL) must evaporate from Solution 1 in order to have a concentration of 4.48 M?

A) 67.0 mL
B) 49.3 mL
C) 33.0 mL
D) 14.9 mL
E) 85.1 mL