Question 1

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.)

Accepted Answer

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

Question 2

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?

Accepted Answer

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

Question 3

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?

Accepted Answer

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

Question 4

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?

Accepted Answer

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

Question 5

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

Accepted Answer

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

Question 6

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 3(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" class="answers-bank-image d-inline" rel="preload" > ions in solution C.

Accepted Answer

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

Question 7

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

Accepted Answer

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

Question 8

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?

Accepted Answer

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

Question 9

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

Accepted Answer

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

Question 10

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.

Accepted Answer

A) True 
 B)False

Question 11

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?

Accepted Answer

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 12

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.

Accepted Answer

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

Question 13

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.

Accepted Answer

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

Question 14

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

Accepted Answer

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 15

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

Accepted Answer

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

Question 16

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.

Accepted Answer

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

Question 17

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.

Accepted Answer

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

Question 18

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

Accepted Answer

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 19

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

Accepted Answer

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

Question 20

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.

Accepted Answer

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

Exam 15: Solutions

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

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

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

Correct Answer
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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?

Correct Answer
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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

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

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

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

Correct Answer
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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?

Correct Answer
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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?

Correct Answer
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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.

Correct Answer
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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.

Correct Answer
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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.

Correct Answer
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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.)

Correct Answer
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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.

Correct Answer
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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.

Correct Answer
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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?

Correct Answer
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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.

Correct Answer
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Correct Answer
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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.

Correct Answer
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Exam 15: Solutions

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

Correct AnswerverifiedShow Answer

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

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

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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?

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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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

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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?

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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.

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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.

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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.

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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.)

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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.

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

Correct Answer
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Correct Answer
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Correct Answer
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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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
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Correct Answer
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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?

Correct Answer
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Correct Answer
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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.

Correct Answer
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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.

Correct Answer
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Correct Answer
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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.

Correct Answer
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Correct Answer
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Correct Answer
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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.

Correct Answer
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Correct Answer
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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.

Correct Answer
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