Question 1

Write the ion product expression for magnesium fluoride, MgF2.

Accepted Answer

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Question 2

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH3COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

Accepted Answer

A)   3.0 M CH3COONa
B)   2.5 M CH3COONa
C)   2.0 M CH3COONa
D)   1.5 M CH3COONa
E)   0.30 M CH3COONa

Question 3

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH?

Accepted Answer

A)   [CH3COOH] = 0.25 M, [CH3COO¯] = 0.25 M
B)   [CH3COOH] = 0.75 M, [CH3COO¯] = 0.75 M
C)   [CH3COOH] = 0.75 M, [CH3COO¯] = 0.25 M
D)   [CH3COOH] = 0.25 M, [CH3COO¯] = 0.75 M
E)   [CH3COOH] = 1.00 M, [CH3COO¯] = 1.00 M

Question 4

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 NH4Cl? Kb = 1.8 * 10¯5

Accepted Answer

A)   1.1 * 10¯5 M
B)   3.0 * 10¯6 M
C)   3.3 * 10¯9 M
D)   9.3 * 10¯10 M
E)   None of these choices is correct.

Question 5

The equivalence point in a titration is defined as the point when the indicator changes color.

Accepted Answer

A) True 
 B)False

Question 6

You need to use KH2PO4 and K2HPO4 to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H3PO4) , Ka2 = 6.2 *10¯8

Accepted Answer

A)   [base]/[acid] = 1.75
B)   [base]/[acid] = 1.27
C)   [base]/[acid] = 1.24
D)   [base]/[acid] = 0.79
E)   [base]/[acid] = 0.57

Question 7

Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6*10¯5)  is titrated with 0.05 M NaOH?

Accepted Answer

A)   bromphenol blue, pH range: 3.0 to 4.5
B)   bromcresol green, pH range: 3.8 to 5.4
C)   alizarin, pH range: 5.7 to 7.2
D)   phenol red, pH range: 6.9 to 8.2
E)   phenolphthalein, pH range: 8.0 to 10.1

Question 8

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Accepted Answer

A)   3.67
B)   3.78
C)   3.81
D)   3.85
E)   3.95

Question 9

A solution is prepared by dissolving 20.0 g of K2HPO4 and 25.0 g of KH2PO4 in enough water to produce 1.0 L of solution. What is the pH of this buffer? For phosphoric acid (H3PO4) , Ka2 = 6.2 *10¯8

Accepted Answer

A)   7.70
B)   7.42
C)   7.21
D)   7.00
E)   6.72

Question 10

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Accepted Answer

A)   BaF2
B)   CuCl
C)   CuBr
D)   AgI
E)   None of the solubilities will be significantly affected.

Question 11

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 *10¯5

Accepted Answer

A)   4.49
B)   4.64
C)   4.85
D)   5.00
E)   5.52

Question 12

Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 * 10¯9

Accepted Answer

A)   1.4 * 10¯3 M
B)   3.4 * 10¯4 M
C)   8.7 * 10¯4 M
D)   5.l *10¯5 M
E)   5 M

Question 13

The salts X(NO3) 2 and Y(NO3) 2 (where X+ and Y+ are metal ions)  are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values: XCl2, 1 * 10¯5; YCl2, 1 * 10¯10; X(OH) 2, 1 *10¯10; Y(OH) 2, 1 * 10¯5

Accepted Answer

A)   1 M NaNO3
B)   1 M HCl
C)   1 M HNO3
D)   1 M NaCl
E)   None of these reagents will accomplish the precipitation.

Question 14

The solubility of calcium chromate is 1.56 *10¯3 g/100 mL of solution. What is the Ksp for CaCrO4?

Accepted Answer

A)   2.4 * 10¯4
B)   1.5 *10¯5
C)   7.6 * 10¯6
D)   1.0 * 10¯8
E)   8

Question 15

When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

Accepted Answer

A)   H2S
B)   H2C2O4
C)   H2C4H4O6
D)   H2Se
E)   H2Te

Exam 19: Ionic Equilibria in Aqueous Systems

Which of the following indicators would be the best to use when 0.050 M benzoic acid (K_a = 6.6*10¯⁵) is titrated with 0.05 M NaOH?

Correct Answer
verified

The solubility of calcium chromate is 1.56 *10¯³ g/100 mL of solution. What is the K_sp for CaCrO₄?

Correct Answer
verified

A solution is prepared by dissolving 20.0 g of K₂HPO₄ and 25.0 g of KH₂PO₄ in enough water to produce 1.0 L of solution. What is the pH of this buffer? For phosphoric acid (H₃PO₄) , K_a2 = 6.2 *10¯⁸

Correct Answer
verified

Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
verified

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct Answer
verified

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH₃COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

Correct Answer
verified

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Correct Answer
verified

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH?

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 NH₄Cl? K_b = 1.8 * 10¯⁵

Correct Answer
verified

Correct Answer
verified

When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

Correct Answer
verified

The equivalence point in a titration is defined as the point when the indicator changes color.

Correct Answer
verified

Calculate the solubility of strontium fluoride, SrF₂, in pure water. K_sp = 2.6 * 10¯⁹

Correct Answer
verified

You need to use KH₂PO₄ and K₂HPO₄ to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H₃PO₄) , K_a2 = 6.2 *10¯⁸

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? K_a = 1.8 *10¯⁵

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6*10¯5) is titrated with 0.05 M NaOH?

Correct AnswerverifiedShow Answer

The solubility of calcium chromate is 1.56 *10¯3 g/100 mL of solution. What is the Ksp for CaCrO4?

Correct AnswerverifiedShow Answer

A solution is prepared by dissolving 20.0 g of K2HPO4 and 25.0 g of KH2PO4 in enough water to produce 1.0 L of solution. What is the pH of this buffer? For phosphoric acid (H3PO4) , Ka2 = 6.2 *10¯8

Correct AnswerverifiedShow Answer

Write the ion product expression for magnesium fluoride, MgF2.

Correct AnswerverifiedShow Answer

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct AnswerverifiedShow Answer

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH3COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

Correct AnswerverifiedShow Answer

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Correct AnswerverifiedShow Answer

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH?

Correct AnswerverifiedShow Answer

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 NH4Cl? Kb = 1.8 * 10¯5

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

Correct AnswerverifiedShow Answer

The equivalence point in a titration is defined as the point when the indicator changes color.

Correct AnswerverifiedShow Answer

Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 * 10¯9

Correct AnswerverifiedShow Answer

You need to use KH2PO4 and K2HPO4 to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H3PO4) , Ka2 = 6.2 *10¯8

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 *10¯5

Correct AnswerverifiedShow Answer

Which of the following indicators would be the best to use when 0.050 M benzoic acid (K_a = 6.6*10¯⁵) is titrated with 0.05 M NaOH?

Correct Answer
verified

The solubility of calcium chromate is 1.56 *10¯³ g/100 mL of solution. What is the K_sp for CaCrO₄?

Correct Answer
verified

A solution is prepared by dissolving 20.0 g of K₂HPO₄ and 25.0 g of KH₂PO₄ in enough water to produce 1.0 L of solution. What is the pH of this buffer? For phosphoric acid (H₃PO₄) , K_a2 = 6.2 *10¯⁸

Correct Answer
verified

Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
verified

Correct Answer
verified

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH₃COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 NH₄Cl? K_b = 1.8 * 10¯⁵

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the solubility of strontium fluoride, SrF₂, in pure water. K_sp = 2.6 * 10¯⁹

Correct Answer
verified

You need to use KH₂PO₄ and K₂HPO₄ to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H₃PO₄) , K_a2 = 6.2 *10¯⁸

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? K_a = 1.8 *10¯⁵

Correct Answer
verified