Question 1

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

Question 2

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Accepted Answer

A)   1.26
B)   1.67
C)   12.33
D)   12.74
E)   13.03F) A) and B)
G) All of the above

Question 3

At the equivalence point in an acid-base titration

Accepted Answer

A)   the [H3O+] equals the Ka of the acid.
B)   the [H3O+] equals the Ka of the indicator.
C)   the amounts of acid and base which have been combined are in their stoichiometric ratio.
D)   the pH is 7.0.
E)   the pH has reached a maximum.F) B) and D)
G) B) and C)

Question 4

Which of the following has the highest buffer capacity?

Accepted Answer

A)   0.10 M H2PO4¯/0.10 M HPO42¯
B)   0.50 M H2PO4¯/0.10 M HPO42¯
C)   0.10 M H2PO4¯/0.50 M HPO42¯
D)   0.50 M H2PO4¯/0.50 M HPO42¯
E)   They all have the same buffer capacity.F) C) and E)
G) D) and E)

Question 5

A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? Kb = 1.8 * 10¯5

Accepted Answer

A)   10.26
B)   9.30
C)   9.21
D)   8.30
E)   8.21F) C) and E)
G) B) and C)

Question 6

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 *10¯18

Accepted Answer

A)   4.0 * 10¯5 M
B)   1.8 * 10¯5 M
C)   4.0 *10¯6 M
D)   1.5 * 10¯6 M
E)   6 MF) A) and B)
G) None of the above

Question 7

Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 * 10¯12

Accepted Answer

A)   1.4 * 10¯4 M
B)   3.4 * 10¯5 M
C)   1.1 * 10¯5 M
D)   1.6 * 10¯6 M
E)   6 MF) None of the above
G) B) and C)

Question 8

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Accepted Answer

A)   3(PO4) 2. 
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B)   3(PO4) 2. 
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C)   3(PO4) 2. 
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D)   3(PO4) 2. 
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E)   None of these choices is correct.F) B) and C)
G) B) and E)

Question 9

When a strong acid is titrated with a weak base, the pH at the equivalence point

Accepted Answer

A)   is greater than 7.0.
B)   is equal to 7.0.
C)   is less than 7.0.
D)   is equal to the pKa of the acid.
E)   is equal to the pKb of the base.F) C) and D)
G) B) and C)

Question 10

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO3) 2. What is the equilibrium concentration of cobalt ions? Kf = 5.0 *109 for Co(OH) 42¯

Accepted Answer

A)   1.1 * 10¯2 M
B)   1.4 * 10¯5 M
C)   3.2 *10¯9 M
D)   2.0* 10¯10 M
E)   4.9* 10¯13 MF) B) and C)
G) A) and E)

Question 11

If the pH of a buffer solution is greater than the pKa value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

Accepted Answer

A) True 
 B)False

Question 12

If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, Ka = 6.8 *10¯4

Accepted Answer

A)   7.13
B)   2.54
C)   1.57
D)   3.17
E)   4.86F) A) and D)
G) A) and C)

Question 13

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 * 10¯4

Accepted Answer

A)   1.3 g
B)   0.69 g
C)   6.9 g
D)   23 g
E)   1.5 gF) D) and E)
G) C) and D)

Question 14

A popular buffer solution consists of carbonate (CO32¯)  and hydrogen carbonate (HCO3¯)  conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

Accepted Answer

A)   0.9 M CO32¯ and 0.1 M HCO3¯
B)   0.1 M CO32¯ and 0.9 M HCO3¯
C)   0.5 M CO32¯ and 0.5 M HCO3¯
D)   0.1 M CO32¯ and 0.1 M HCO3¯
E)   They all have the same buffer capacity.F) A) and D)
G) B) and E)

Question 15

Use the following information to calculate the solubility product constant, Ksp, for PbCl2. A saturated solution of PbCl2 in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid PbCl2 residue recovered in the beaker amounted to 0.0162 moles.

Accepted Answer

A)   Ksp = 6.9 *10¯8
B)   Ksp = 4.3 * 10¯6
C)   Ksp = 1.7 * 10¯5
D)   Ksp = 2.6 *10¯4
E)   Ksp = 3.2 *10¯2F) B) and D)
G) B) and C)

Question 16

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8 (ethylene diamine)  and 0.35 C2N2H9Cl? Kb = 4.7 * 10¯4

Accepted Answer

A)   2.0 * 10¯3 M
B)   1.1 * 10¯3 M
C)   6.3 * 10¯9 M
D)   2.1 * 10¯10 M
E)   5.0 * 10¯11 MF) B) and E)
G) A) and E)

Question 17

The solubility of silver chloride _______________ when dilute nitric is added to it.

Accepted Answer

A)   increases
B)   decreases
C)   does not change
D)   first increases, then decreases
E)   first decreases, then increasesF) B) and C)
G) All of the above

Question 18

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

Accepted Answer

A) True 
 B)False

Question 19

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? Ka = 1.8 * 10¯5

Accepted Answer

A)   4.57
B)   4.52
C)   4.87
D)   4.92
E)   4.97F) B) and D)
G) A) and B)

Question 20

Which of the following substances has the greatest solubility in water?

Accepted Answer

A)   MgCO3, Ksp = 3.5*10¯8
B)   NiCO3, Ksp = 1.3 * 10¯7
C)   AgIO3, Ksp = 3.1 * 10¯8
D)   CuBr, Ksp = 5.0 * 10¯9
E)   AgCN, Ksp = 2.2 *10¯16F) B) and C)
G) A) and E)

Exam 19: Ionic Equilibria in Aqueous Systems

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈ (ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 * 10¯⁴

Correct Answer
verified

If the pH of a buffer solution is greater than the pK_a value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

Correct Answer
verified

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃) ₂. What is the equilibrium concentration of cobalt ions? K_f = 5.0 *10⁹ for Co(OH) ₄²¯

Correct Answer
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A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? K_b = 1.8 * 10¯⁵

Correct Answer
verified

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

Correct Answer
verified

Correct Answer
verified

A popular buffer solution consists of carbonate (CO₃²¯) and hydrogen carbonate (HCO₃¯) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

Correct Answer
verified

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH. What is the pH of this buffer? K_a = 1.8 * 10¯⁵

Correct Answer
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When a strong acid is titrated with a weak base, the pH at the equivalence point

Correct Answer
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If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, K_a = 6.8 *10¯⁴

Correct Answer
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What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, K_a = 7.2 * 10¯⁴

Correct Answer
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Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
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Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 *10¯¹⁸

Correct Answer
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Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 * 10¯¹²

Correct Answer
verified

Which of the following has the highest buffer capacity?

Correct Answer
verified

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Correct Answer
verified

The solubility of silver chloride _______________ when dilute nitric is added to it.

Correct Answer
verified

At the equivalence point in an acid-base titration

Correct Answer
verified

Correct Answer
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Which of the following substances has the greatest solubility in water?

Correct Answer
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Exam 19: Ionic Equilibria in Aqueous Systems

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8 (ethylene diamine) and 0.35 C2N2H9Cl? Kb = 4.7 * 10¯4

Correct AnswerverifiedShow Answer

If the pH of a buffer solution is greater than the pKa value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

Correct AnswerverifiedShow Answer

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO3) 2. What is the equilibrium concentration of cobalt ions? Kf = 5.0 *109 for Co(OH) 42¯

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? Kb = 1.8 * 10¯5

Correct AnswerverifiedShow Answer

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A popular buffer solution consists of carbonate (CO32¯) and hydrogen carbonate (HCO3¯) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? Ka = 1.8 * 10¯5

Correct AnswerverifiedShow Answer

When a strong acid is titrated with a weak base, the pH at the equivalence point

Correct AnswerverifiedShow Answer

If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, Ka = 6.8 *10¯4

Correct AnswerverifiedShow Answer

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 * 10¯4

Correct AnswerverifiedShow Answer

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

Correct AnswerverifiedShow Answer

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 *10¯18

Correct AnswerverifiedShow Answer

Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 * 10¯12

Correct AnswerverifiedShow Answer

Which of the following has the highest buffer capacity?

Correct AnswerverifiedShow Answer

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Correct AnswerverifiedShow Answer

The solubility of silver chloride _______________ when dilute nitric is added to it.

Correct AnswerverifiedShow Answer

At the equivalence point in an acid-base titration

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following substances has the greatest solubility in water?

Correct AnswerverifiedShow Answer

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈ (ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 * 10¯⁴

Correct Answer
verified

If the pH of a buffer solution is greater than the pK_a value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

Correct Answer
verified

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃) ₂. What is the equilibrium concentration of cobalt ions? K_f = 5.0 *10⁹ for Co(OH) ₄²¯

Correct Answer
verified

A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? K_b = 1.8 * 10¯⁵

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A popular buffer solution consists of carbonate (CO₃²¯) and hydrogen carbonate (HCO₃¯) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

Correct Answer
verified

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH. What is the pH of this buffer? K_a = 1.8 * 10¯⁵

Correct Answer
verified

Correct Answer
verified

If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, K_a = 6.8 *10¯⁴

Correct Answer
verified

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, K_a = 7.2 * 10¯⁴

Correct Answer
verified

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

Correct Answer
verified

Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 *10¯¹⁸

Correct Answer
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Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 * 10¯¹²

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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