Question 1

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

Accepted Answer

A)   dissolving a small amount of solid sodium acetate
B)   adding a small amount of dilute hydrochloric acid
C)   adding a small amount of dilute sodium hydroxide
D)   dissolving a small amount of solid sodium chloride
E)   diluting the buffer solution with waterF) A) and B)
G) A) and E)

Question 2

Barium sulfate (BaSO4)  is a slightly soluble salt, with Ksp = 1.1 × 10-10. What mass of Ba2+ ions will be present in 1.0 L of a saturated solution of barium sulfate?

Accepted Answer

A)   -7 g
B)   1.0 × 10-5 g
C)   0.0014 g
D)   0.0024 g
E)   > 0.05 gF) All of the above
G) B) and E)

Question 3

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

Accepted Answer

A)   The pH will be greater than the pKa of hypochlorous acid.
B)   The pH will be less than the pKa of hypochlorous acid.
C)   The pH will be equal to the pKa of hypochlorous acid.
D)   The pH will equal the pKb of sodium hypochlorite.
E)   The pH will be none of the above.F) A) and E)
G) D) and E) B

Question 4

What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?

Accepted Answer

A)   4.00 mL
B)   8.00 mL
C)   12.5 mL
D)   16.0 mL
E)   32.0 mLF) A) and E)
G) All of the above B

Question 5

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 the above reagents will accomplish the precipitation.F) A) and B)
G) A) and C)

Question 6

Write the ion product expression for silver sulfide, Ag2S.

Accepted Answer

A)   2S. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2S. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2S. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2S. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2S. 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and E)
G) A) and B)

Question 7

When a strong acid is titrated with a strong 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, but is not 3.5.
D)   is equal to the pKa of the acid.
E)   is equal to 3.5.F) C) and D)
G) A) and D)

Question 8

When a weak acid is titrated with a strong 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 14.0 - pKb , where pKb is that of the base.F) B) and C)
G) A) and C)

Question 9

Lead(II) iodide, PbI2, is an ionic compound with a solubility product constant
Ksp of 7.9 × 10-9.Calculate the solubility of this compound in
a. pure water.
b. 0.50 mol L-1 KI solution.

Accepted Answer

a. 1.3 × 1...

Question 10

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)   H2TeF) A) and B)
G) D) and E)

Question 11

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

Accepted Answer

A)   CH3COOH, NaH2PO4
B)   H2CO3, HCO3-
C)   H2PO4-, HCO3-
D)   HSO4-, HSO3-
E)   None of the above will be a buffer solution.F) B) and E)
G) A) and C)

Question 12

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) A) and E)
G) B) and D) D

Question 13

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4) 2?

Accepted Answer

A)   6.5 × 10-12
B)   6.0 × 10-14
C)   5.2 × 10-24
D)   4.8 × 10-26
E)   1.0 × 10-26F) A) and D)
G) D) and E)

Question 14

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 E)
G) C) and D)

Question 15

A phosphate buffer (H2PO4-/HPO42-)  has a pH of 8.3. Which of the following changes will cause the pH to increase?

Accepted Answer

A)   dissolving a small amount of Na2HPO4
B)   dissolving a small amount of NaH2PO4
C)   adding a small amount of dilute hydrochloric acid
D)   adding a small amount of dilute phosphoric acid
E)   making the buffer more concentrated by removing some waterF) All of the above
G) B) and E)

Question 16

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H2PO4-] = [HPO42-] = 0.35 M?

Accepted Answer

A)   The pH will increase slightly.
B)   The pH will increase significantly.
C)   The pH will decrease slightly.
D)   The pH will decrease significantly.
E)   Since it is a buffer solution, the pH will not be affected.F) A) and D)
G) C) and E)

Question 17

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

Accepted Answer

A) True 
 B)False

Question 18

A 20.0-mL sample of 0.30 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Accepted Answer

A)   2.95
B)   3.13
C)   10.87
D)   11.05
E)   13.14F) A) and D)
G) A) and E)

Question 19

Fe(NO3)3 (0.00100 mol) and KSCN (0.200 mol) are added to water to make exactly 1 liter of solution. The red complex ion FeSCN2+ is produced. Calculate the concentrations of Fe3+(aq) and FeSCN2+(aq) at equilibrium, if Kf  of the FeSCN2+ is
8.9 × 102.

Accepted Answer

[Fe³⁺] = 5.6...

Question 20

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Accepted Answer

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

Exam 19: Ionic Equilibria in Aqueous Systems

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

Correct Answer
verified

Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 × 10^-10. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

Correct Answer
verified

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

Correct Answer
verified
B

What volume of 0.500 M H₂SO₄is needed to react completely with 20.0 mL of 0.400 M LiOH?

Correct Answer
verified
B

Correct Answer
verified

Write the ion product expression for silver sulfide, Ag₂S.

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

Lead(II) iodide, PbI₂, is an ionic compound with a solubility product constant K_sp of 7.9 × 10^-9.Calculate the solubility of this compound in a. pure water. b. 0.50 mol L^-1 KI solution.

Correct Answer
verified
a. 1.3 × 1...
View 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 Answer
verified

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

Correct Answer
verified

Which of the following has the highest buffer capacity?

Correct Answer
verified
D

The solubility of magnesium phosphate is 2.27 × 10^-3g/1.0 L of solution. What is the K_sp for Mg₃(PO₄) ₂?

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

A phosphate buffer (H₂PO₄^-/HPO₄^2-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

Correct Answer
verified

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H₂PO₄^-] = [HPO₄^2-] = 0.35 M?

Correct Answer
verified

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

Correct Answer
verified

A 20.0-mL sample of 0.30 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Correct Answer
verified

Fe(NO₃)₃ (0.00100 mol) and KSCN (0.200 mol) are added to water to make exactly 1 liter of solution. The red complex ion FeSCN²⁺ is produced. Calculate the concentrations of Fe³⁺(aq) and FeSCN²⁺(aq) at equilibrium, if K_f of the FeSCN²⁺ is 8.9 × 10².

Correct Answer
verified
[Fe³⁺] = 5.6...
View Answer

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

Correct AnswerverifiedShow Answer

Barium sulfate (BaSO4) is a slightly soluble salt, with Ksp = 1.1 × 10-10. What mass of Ba2+ ions will be present in 1.0 L of a saturated solution of barium sulfate?

Correct AnswerverifiedShow Answer

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

Correct AnswerverifiedB

What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?

Correct AnswerverifiedB

Correct AnswerverifiedShow Answer

Write the ion product expression for silver sulfide, Ag2S.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Lead(II) iodide, PbI2, is an ionic compound with a solubility product constant Ksp of 7.9 × 10-9.Calculate the solubility of this compound in a. pure water. b. 0.50 mol L-1 KI solution.

Correct Answerverifieda. 1.3 × 1...View AnswerShow 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

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

Correct AnswerverifiedShow Answer

Which of the following has the highest buffer capacity?

Correct AnswerverifiedD

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4) 2?

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

A phosphate buffer (H2PO4-/HPO42-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

Correct AnswerverifiedShow Answer

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H2PO4-] = [HPO42-] = 0.35 M?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A 20.0-mL sample of 0.30 M HBr is titrated with 0.15 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

Fe(NO3)3 (0.00100 mol) and KSCN (0.200 mol) are added to water to make exactly 1 liter of solution. The red complex ion FeSCN2+ is produced. Calculate the concentrations of Fe3+(aq) and FeSCN2+(aq) at equilibrium, if Kf of the FeSCN2+ is 8.9 × 102.

Correct Answerverified[Fe3+] = 5.6...View AnswerShow Answer

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 × 10^-10. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

Correct Answer
verified

Correct Answer
verified
B

What volume of 0.500 M H₂SO₄is needed to react completely with 20.0 mL of 0.400 M LiOH?

Correct Answer
verified
B

Correct Answer
verified

Write the ion product expression for silver sulfide, Ag₂S.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Lead(II) iodide, PbI₂, is an ionic compound with a solubility product constant K_sp of 7.9 × 10^-9.Calculate the solubility of this compound in a. pure water. b. 0.50 mol L^-1 KI solution.

Correct Answer
verified
a. 1.3 × 1...
View Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
D

The solubility of magnesium phosphate is 2.27 × 10^-3g/1.0 L of solution. What is the K_sp for Mg₃(PO₄) ₂?

Correct Answer
verified

Correct Answer
verified

A phosphate buffer (H₂PO₄^-/HPO₄^2-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

Correct Answer
verified

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H₂PO₄^-] = [HPO₄^2-] = 0.35 M?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Fe(NO₃)₃ (0.00100 mol) and KSCN (0.200 mol) are added to water to make exactly 1 liter of solution. The red complex ion FeSCN²⁺ is produced. Calculate the concentrations of Fe³⁺(aq) and FeSCN²⁺(aq) at equilibrium, if K_f of the FeSCN²⁺ is 8.9 × 10².

Correct Answer
verified
[Fe³⁺] = 5.6...
View Answer

Correct Answer
verified