Question 1

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 2

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq)  +(aq) + HCOO-(aq)  A) There is no change in the equilibrium. B) The equilibrium shifts to the right. C) More information is needed to answer the question. D) The equilibrium shifts to the left. E) The pH decreases." class="answers-bank-image d-inline" rel="preload" > H+(aq) + HCOO-(aq)

Accepted Answer

A)  There is no change in the equilibrium.
B)  The equilibrium shifts to the right.
C)  More information is needed to answer the question.
D)  The equilibrium shifts to the left.
E)  The pH decreases.F) D) and E)
G) C) and D)

Question 3

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

Accepted Answer

A) True 
 B)False

Question 4

Which of the following acids is the best acid to prepare a buffer with the highest pH?

Accepted Answer

A)  C5H5O5COOH,Ka = 4.0 × 10-6
B)  HOC6H4OCOOH,Ka = 1.0 × 10-3
C)  HBrO,Ka = 2.3 × 10-9
D)  C6H4(COOH) 2,Ka = 2.9 × 10-4
E)  CH3COOH,Ka = 1.8 × 10-5F) B) and D)
G) B) and C)

Question 5

A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH.What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [Ka(CH3CH2COOH) = 1.3 × 10-5]

Accepted Answer

A)  5.75
B)  4.94
C)  4.83
D)  4.02
E)  3.95F) A) and B)
G) A) and D)

Question 6

Which will precipitate first when AgNO3 is added to a solution containing equal concentrations of Br-,Cl-, and I- ions?

Accepted Answer

A)  AgBr
B)  AgCl
C)  AgI
D)  AgNO3
E)  No precipitate will formF) C) and D)
G) B) and E)

Question 7

The ____________________ is the point in a titration where the color of the indicator changes.

Accepted Answer

The answer of The ____________________ is the point in a...

Question 8

Calculate the solubility of zinc hydroxide,Zn(OH) 2,in 1.00 M NaOH.Ksp = 3.0 × 10-16 for Zn(OH) 2,Kf = 3.0 × 1015 for Zn(OH) 42-

Accepted Answer

A)  0.60 M
B)  0.52 M
C)  0.37 M
D)  0.32 M
E)  0.24 MF) A) and B)
G) A) and E)

Question 9

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH.What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Accepted Answer

A)  0.85
B)  2.96
C)  2.85
D)  1.49
E)  3.81F) A) and B)
G) A) and C)

Question 10

Which of the following is correct for the equivalence point in an acid-base titration?

Accepted Answer

A)  The pH is at its highest value for any reaction.
B)  The amounts of acid and base combined are in a stoichiometric ratio at the equivalence point in an acid-base titration.
C)  The pH is 7.0.
D)  The pH is equal to the pKa of the weak acid.
E)  The pH is equal to the pKb of the weak base.F) A) and D)
G) All of the above

Question 11

Indicators are weak acids that are one color in acidic solution and another color in basic solution.

Accepted Answer

A) True 
 B)False

Question 12

Calculate the solubility of silver oxalate,Ag2C2 O4,in pure water. [Ksp(Ag2C2O4) = 1.0 × 10-11]

Accepted Answer

A)  1.4 × 10-4 M
B)  8.2 × 10-5 M
C)  5.4 × 10-5 M
D)  3.2 × 10-6 M
E)  2.5 × 10-12 MF) B) and C)
G) A) and B)

Question 13

What molar ratio of CH3COOH to CH3COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [Ka(CH3COOH) = 1.8 × 10-5]

Accepted Answer

A)  0.18
B)  0.84
C)  1.2
D)  5.6
E)  0.10F) A) and D)
G) A) and B)

Question 14

What is the pH of a solution prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl?
[Ka(HOCl) = 3.2 × 10-8]

Accepted Answer

A)  4.10
B)  7.00
C)  7.19
D)  7.49
E)  7.80F) B) and D)
G) A) and B)

Question 15

When an acid,HA,is titrated with 0.1 M NaOH,the pH at the half equivalence point of the titration is 4.5.What is the Ka of the acid?

Accepted Answer

A)  3.2 x 10-5
B)  3.2 x 10-10
C)  1.8 x 10-3
D)  7.0 x 10-7
E)  HA is a strong acidF) C) and D)
G) B) and E)

Question 16

The molar solubility of tin(II) iodide is 1.28 × 10-2 mol/L.What is Ksp for this compound?

Accepted Answer

A)  8.39 × 10-6
B)  1.28 × 10-2
C)  4.20 × 10-6
D)  1.64 × 10-4
E)  2.10 × 10-6F) All of the above
G) D) and E)

Question 17

Methyl red is a common acid-base indicator.It has a Ka equal to 6.3 × 10-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Accepted Answer

A)  green
B)  red
C)  blue
D)  yellow
E)  violetF) B) and C)
G) A) and E)

Question 18

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.[Ksp(CrF3) = 6.6 × 10-11]

Accepted Answer

A)  0.023 M
B)  0.032 M
C)  7.7 × 10-8 M
D)  2.9 × 10-9 M
E)  6.9 × 10-10 MF) B) and C)
G) A) and B)

Question 19

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 between 3.5 and 7.0.
D)  is equal to the p Ka of the acid.
E)  is equal to 3.5.F) None of the above
G) A) and C)

Question 20

Which is the best acid to prepare a buffer with the lowest pH?

Accepted Answer

A)  C5H5O5COOH,Ka = 4.0 × 10-6
B)  HOC6H4OCOOH,Ka = 1.0 × 10-3
C)  HBrO,Ka = 2.3 × 10-9
D)  C6H4(COOH) 2,Ka = 2.9 × 10-4
E)  CH3COOH,Ka = 1.8 × 10-5F) A) and D)
G) A) and C)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Which is the best acid to prepare a buffer with the lowest pH?

Correct AnswerverifiedShow Answer

What molar ratio of CH3COOH to CH3COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [Ka(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

The molar solubility of tin(II) iodide is 1.28 × 10-2 mol/L.What is Ksp for this compound?

Correct AnswerverifiedShow Answer

When an acid,HA,is titrated with 0.1 M NaOH,the pH at the half equivalence point of the titration is 4.5.What is the Ka of the acid?

Correct AnswerverifiedShow Answer

Indicators are weak acids that are one color in acidic solution and another color in basic solution.

Correct AnswerverifiedShow Answer

Which of the following acids is the best acid to prepare a buffer with the highest pH?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.[Ksp(CrF3) = 6.6 × 10-11]

Correct AnswerverifiedShow Answer

What is the pH of a solution prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl? [Ka(HOCl) = 3.2 × 10-8]

Correct AnswerverifiedShow Answer

Which will precipitate first when AgNO3 is added to a solution containing equal concentrations of Br-,Cl-, and I- ions?

Correct AnswerverifiedShow Answer

A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH.What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [Ka(CH3CH2COOH) = 1.3 × 10-5]

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

Which of the following is correct for the equivalence point in an acid-base titration?

Correct AnswerverifiedShow Answer

The ____________________ is the point in a titration where the color of the indicator changes.

Correct AnswerverifiedShow Answer

Calculate the solubility of silver oxalate,Ag2C2 O4,in pure water. [Ksp(Ag2C2O4) = 1.0 × 10-11]

Correct AnswerverifiedShow Answer

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq) H+(aq) + HCOO-(aq)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Methyl red is a common acid-base indicator.It has a Ka equal to 6.3 × 10-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Correct AnswerverifiedShow Answer

Calculate the solubility of zinc hydroxide,Zn(OH) 2,in 1.00 M NaOH.Ksp = 3.0 × 10-16 for Zn(OH) 2,Kf = 3.0 × 1015 for Zn(OH) 42-

Correct AnswerverifiedShow Answer

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH.What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

Correct Answer
verified

What molar ratio of CH₃COOH to CH₃COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

The molar solubility of tin(II) iodide is 1.28 × 10^-2 mol/L.What is K_sp for this compound?

Correct Answer
verified

When an acid,HA,is titrated with 0.1 M NaOH,the pH at the half equivalence point of the titration is 4.5.What is the K_a of the acid?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.[K_sp(CrF₃) = 6.6 × 10^-11]

Correct Answer
verified

What is the pH of a solution prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl? [K_a(HOCl) = 3.2 × 10^-8]

Correct Answer
verified

Which will precipitate first when AgNO₃ is added to a solution containing equal concentrations of Br^-,Cl^-, and I^- ions?

Correct Answer
verified

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH.What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? [K_a(CH₃CH₂COOH) = 1.3 × 10^-5]

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

Correct Answer
verified

Correct Answer
verified

Calculate the solubility of silver oxalate,Ag₂C₂ O₄,in pure water. [K_sp(Ag₂C₂O₄) = 1.0 × 10^-11]

Correct Answer
verified

What is the effect on the equilibrium when sodium formate is added to a solution of formic acid? HCOOH(aq) H⁺(aq) + HCOO^-(aq)

Correct Answer
verified

Correct Answer
verified

Methyl red is a common acid-base indicator.It has a K_a equal to 6.3 × 10^-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Correct Answer
verified

Calculate the solubility of zinc hydroxide,Zn(OH) ₂,in 1.00 M NaOH.K_sp = 3.0 × 10^-16 for Zn(OH) ₂,K_f = 3.0 × 10¹⁵ for Zn(OH) ₄^2-

Correct Answer
verified

Correct Answer
verified