Question 1

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) D) and E)

Question 2

Use a carefully drawn and labeled diagram of the titration curve to illustrate the titration of a weak diprotic acid, in which Ka1 and Ka2 are substantially different, with a strong base (base is the titrant). Label as many features of the diagram as possible.

Accepted Answer

Question 3

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. a for HClO? A)  1.1 × 10-7 B)  3.5 × 10-8 C)  1.2 × 10-8 D)  4.9 × 10-11 E)  none of the above" class="answers-bank-image d-inline" rel="preload" >
What is the Ka for HClO?

Accepted Answer

A)   1.1 × 10-7
B)   3.5 × 10-8
C)   1.2 × 10-8
D)   4.9 × 10-11
E)   none of the aboveF) A) and D)
G) D) and E)

Question 4

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) D) and E)
G) C) and D)

Question 5

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: 3.0-4.5
B)   bromcresol green, pH range: 3.8-5.4
C)   alizarin, pH range: 5.7-7.2
D)   phenol red, pH range: 6.9-8.2
E)   phenolphthalein, pH range: 8.0-10.1F) A) and B)
G) A) and C)

Question 6

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Accepted Answer

A)   It is a buffer, pH > pKa of propanoic acid.
B)   It is a buffer, pH a of propanoic acid.
C)   It is a buffer, pH = pKa of propanoic acid.
D)   It is a buffer, pH = pKb of sodium propanoate.
E)   Since sodium hydroxide is a strong base, this is not a buffer.F) C) and D)
G) A) and B)

Question 7

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For AgCl, Ksp = 1.8 × 10- 10.

Accepted Answer

A)   1.8 × 10-10 mol Ag+
B)   9.0 × 10-10 mol Ag+
C)   9.0 × 10-9 mol Ag+
D)   6.7 × 10-8 mol Ag+
E)   1.3 × 10-5 mol Ag+F) B) and C)
G) B) and D)

Question 8

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA) and 0.250 mol of sodium propenoate (NaA)? (Ka for propenoic acid is 5.52 × 10-5.)

Accepted Answer

Question 9

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) C) and D)
G) B) and C)

Question 10

What is the pKa for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

Accepted Answer

A)   
B)   4.63
C)   4.87
D)   5.02
E)   > 5.50F) A) and E)
G) C) and D)

Question 11

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. Which of the answers gives the concentration of chloride ions will precipitate the most YCl2 without precipitating any XCl2? Given Ksp values: XCl2, 2 × 10-5 YCl2, 1 × 10-10

Accepted Answer

A)   1 M Cl-
B)   0.1 M Cl-
C)   0.01 M Cl-
D)   0.001 M Cl-
E)   0.0001 M Cl-F) None of the above
G) B) and E)

Question 12

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO3) 2. Ksp = 6.5 × 10-6 for Ca(OH) 2) . Which of the following statements is correct?

Accepted Answer

A)   Calcium hydroxide precipitates until the solution is saturated.
B)   The solution is unsaturated and no precipitate forms.
C)   The concentration of calcium ions is reduced by the addition of the hydroxide ions.
D)   One must know Ksp for calcium nitrate to make meaningful predictions on this system.
E)   The presence of KOH will raise the solubility of Ca(NO3) 2.F) C) and E)
G) B) and D)

Question 13

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 the aboveF) B) and D)
G) C) and D)

Question 14

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10-4

Accepted Answer

A)   1.1 × 10-4 M
B)   2.6 × 10-4 M
C)   4.3 × 10-4 M
D)   6.7 × 10-5 M
E)   none of the aboveF) A) and C)
G) A) and B)

Question 15

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) A) and E)
G) None of the above

Question 16

A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka = 1.77 × 10-4

Accepted Answer

A)   4.00
B)   3.88
C)   3.63
D)   3.51
E)   3.47F) All of the above
G) A) and E)

Question 17

A 20.0-mL sample of 0.25 M HNO3 is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Accepted Answer

A)   2.00
B)   1.60
C)   1.05
D)   1.00
E)   none of the aboveF) B) and D)
G) All of the above

Question 18

Which of the following aqueous mixtures would be a buffer system?

Accepted Answer

A)   HCl, NaCl
B)   HNO3, NaNO3
C)   H3PO4, H2PO4-
D)   H2SO4, CH3COOH
E)   NH3, NaOHF) C) and E)
G) B) and D)

Question 19

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) B) and E)
G) C) and D)

Question 20

Consider the dissolution of MnS in water
a of H2S is needed before a reliable prediction can be made." class="answers-bank-image d-inline" rel="preload" >
How is the solubility of manganese(II)  sulfide affected by the addition of aqueous potassium hydroxide to the system?

Accepted Answer

A)   The solubility will be unchanged.
B)   The solubility will decrease.
C)   The solubility will increase.
D)   The amount of KOH added must be known before its effect can be predicted.
E)   The pKa of H2S is needed before a reliable prediction can be made.F) D) and E)
G) A) and B)

Exam 19: Ionic Equilibria in Aqueous Systems

What is the pK_a for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

Correct Answer
verified

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃) ₂. K_sp = 6.5 × 10^-6 for Ca(OH) ₂) . Which of the following statements is correct?

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

Correct Answer
verified

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
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A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? K_a = 1.77 × 10^-4

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

Correct Answer
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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) ₄^2-

Correct Answer
verified

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA) and 0.250 mol of sodium propenoate (NaA)? (K_a for propenoic acid is 5.52 × 10^-5.)

Correct Answer
verified

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. What is the K_a for HClO?

Correct Answer
verified

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Correct Answer
verified

Use a carefully drawn and labeled diagram of the titration curve to illustrate the titration of a weak diprotic acid, in which K_a1 and K_a2 are substantially different, with a strong base (base is the titrant). Label as many features of the diagram as possible.

Correct Answer
verified

A 20.0-mL sample of 0.25 M HNO₃is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Correct Answer
verified

Consider the dissolution of MnS in water How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct Answer
verified

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

Correct Answer
verified

Which of the following aqueous mixtures would be a buffer system?

Correct Answer
verified

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. For AgCl, K_sp = 1.8 × 10^{- 10}.

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10^-4

Correct Answer
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Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃and 2.5 NH₄Cl? K_b = 1.8 × 10^-5

Correct Answer
verified

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

What is the pKa for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

Correct AnswerverifiedShow Answer

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO3) 2. Ksp = 6.5 × 10-6 for Ca(OH) 2) . Which of the following statements is correct?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka = 1.77 × 10-4

Correct AnswerverifiedShow Answer

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

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

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA) and 0.250 mol of sodium propenoate (NaA)? (Ka for propenoic acid is 5.52 × 10-5.)

Correct AnswerverifiedShow Answer

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. What is the Ka for HClO?

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Correct AnswerverifiedShow Answer

Use a carefully drawn and labeled diagram of the titration curve to illustrate the titration of a weak diprotic acid, in which Ka1 and Ka2 are substantially different, with a strong base (base is the titrant). Label as many features of the diagram as possible.

Correct AnswerverifiedShow Answer

A 20.0-mL sample of 0.25 M HNO3 is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

Consider the dissolution of MnS in water How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which of the following aqueous mixtures would be a buffer system?

Correct AnswerverifiedShow Answer

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For AgCl, Ksp = 1.8 × 10- 10.

Correct AnswerverifiedShow Answer

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10-4

Correct AnswerverifiedShow Answer

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

What is the pK_a for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

Correct Answer
verified

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃) ₂. K_sp = 6.5 × 10^-6 for Ca(OH) ₂) . Which of the following statements is correct?

Correct Answer
verified

Correct Answer
verified

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

A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? K_a = 1.77 × 10^-4

Correct Answer
verified

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) ₄^2-

Correct Answer
verified

What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA) and 0.250 mol of sodium propenoate (NaA)? (K_a for propenoic acid is 5.52 × 10^-5.)

Correct Answer
verified

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH. The following data were collected during the titration. What is the K_a for HClO?

Correct Answer
verified

Correct Answer
verified

Use a carefully drawn and labeled diagram of the titration curve to illustrate the titration of a weak diprotic acid, in which K_a1 and K_a2 are substantially different, with a strong base (base is the titrant). Label as many features of the diagram as possible.

Correct Answer
verified

A 20.0-mL sample of 0.25 M HNO₃is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. For AgCl, K_sp = 1.8 × 10^{- 10}.

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10^-4

Correct Answer
verified

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃and 2.5 NH₄Cl? K_b = 1.8 × 10^-5

Correct Answer
verified

Correct Answer
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