Question 1

Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid?

Accepted Answer

A)   Less than zero
B)   Between 0 and 7
C)   Close to 7.0
D)   Between 7 and 14
E)   Greater than 14F) B) and D)
G) A) and B)

Question 2

A 50.0-mL sample of a 0.100 M solution of a weak acid HA has an equilibrium pH of 4.00. After 1.0 × 10-3mol of a substance X is added to the solution, it is observed that the pH of the solution increases. What might be true about substance X? I. X might be a strong base that partially neutralized some weak acid.
II)  X might be a strong acid that made the solution more acidic.
III)  X might be a soluble ionic compound containing the anion A-.

Accepted Answer

A)   I only
B)   II only
C)   III only
D)   I or III
E)   II or IIIF) D) and E)
G) A) and B)

Question 3

Which compound has the highest solubility in pure water?

Accepted Answer

A)   Ag2C2O4, Ksp = 1.0 × 10-11
B)   PbCl2, Ksp = 1.7 × 10-5
C)   CaSO4, Ksp = 2.4 × 10-5
D)   Ca3(PO4) 2, Ksp = 1.2 × 10-26
E)   MgF2, Ksp = 6.9 × 10-9F) A) and E)
G) D) and E)

Question 4

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [Ka(HCOOH)  = 1.7 × 10-4]

Accepted Answer

A)   2.87
B)   3.72
C)   3.82
D)   3.95
E)   4.66F) A) and D)
G) None of the above

Question 5

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L. What is Ksp for this compound?

Accepted Answer

A)   1.8 × 10-4
B)   3.6 × 10-4
C)   1.3 × 10-7
D)   3.2 × 10-8
E)   2.8 × 10-14F) C) and E)
G) B) and E)

Question 6

A ________ helps maintain a constant pH even after the addition of acid or base.

Accepted Answer

The answer of A ________ helps maintain a constant pH...

Question 7

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid?
CH3COOH(aq)  H+(aq) + CH3COO-(aq)

Accepted Answer

The equilibrium shif...

Question 8

Which pair of substances is capable of forming a buffer in aqueous solution?

Accepted Answer

A)   H3PO4, Na3PO3
B)   HNO3, NaNO3
C)   HCl, NaCl
D)   H2CO3, NaNO2
E)   CH3COOH, CH3COONaF) A) and E)
G) A) and B)

Question 9

Which is the best choice for preparing a buffer with a pH of 3.5?

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

Question 10

Which compound has the lowest solubility in pure water?

Accepted Answer

A)   Ag2C2O4, Ksp = 1.0 × 10-11
B)   PbCl2, Ksp = 1.7 × 10-5
C)   FePO4, Ksp = 1.3 × 10-22
D)   Ca3(PO4) 2, Ksp = 1.2 × 10-26
E)   MgF2, Ksp = 6.9 × 10-9F) None of the above
G) A) and B)

Question 11

A(n) ________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

Accepted Answer

formation constant o...

Question 12

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

Question 13

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Accepted Answer

A)   0.025 mol HCl
B)   0.063 mol HCl
C)   0.082 mol HCl
D)   0.50 mol HCl
E)   1.0 mol HClF) B) and C)
G) B) and D)

Question 14

When a weak 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 determined by the magnitudes of Ka and Kb.
E)   depends on the pKa of the indicator.F) A) and D)
G) B) and D)

Question 15

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

Accepted Answer

A)   14.0
B)   7.0
C)   3.5
D)   1.0
E)   0.0F) B) and D)
G) None of the above

Question 16

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)   7.46 × 10-11
B)   2.68 × 10-9
C)   5.19 × 10-24
D)   4.80 × 10-26
E)   1.20 × 10-26F) D) and E)
G) A) and B)

Question 17

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

Question 18

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 E)
G) A) and C)

Question 19

The solubility of lead(II)  iodide is 0.064 g/100 mL at 20°C. What is the solubility product for lead(II)  iodide?

Accepted Answer

A)   1.1 × 10-8
B)   2.7 × 10-9
C)   1.1 × 10-11
D)   2.7 × 10-12
E)   1.1 × 10-3F) B) and E)
G) All of the above

Question 20

After the equivalence point, the titration curve of a weak acid is identical to that of a ________ ________.

Accepted Answer

The answer of After the equivalence point, the titration curve...

Exam 17: Acid-Base Equilibria and Solubility Equilibria

After the equivalence point, the titration curve of a weak acid is identical to that of a .

Correct Answer
verified

Which compound has the lowest solubility in pure water?

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

Correct Answer
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A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [K_a(HCOOH) = 1.7 × 10^-4]

Correct Answer
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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
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A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

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

Correct Answer
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Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid?

Correct Answer
verified

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

Correct Answer
verified

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C. What is the solubility product for lead(II) iodide?

Correct Answer
verified

A(n) ________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

Correct Answer
verified
formation constant o...
View 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? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

Correct Answer
verified

Which is the best choice for preparing a buffer with a pH of 3.5?

Correct Answer
verified

A ________ helps maintain a constant pH even after the addition of acid or base.

Correct Answer
verified

Which compound has the highest solubility in pure water?

Correct Answer
verified

Which pair of substances is capable of forming a buffer in aqueous solution?

Correct Answer
verified

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺(aq) + CH₃COO^-(aq)

Correct Answer
verified
The equilibrium shif...
View Answer

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L. What is K_sp for this compound?

Correct Answer
verified

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

Correct Answer
verified

Exam 17: Acid-Base Equilibria and Solubility Equilibria

After the equivalence point, the titration curve of a weak acid is identical to that of a ________ ________.

Correct AnswerverifiedShow Answer

Which compound has the lowest solubility in pure water?

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 buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [Ka(HCOOH) = 1.7 × 10-4]

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

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid?

Correct AnswerverifiedShow Answer

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

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C. What is the solubility product for lead(II) iodide?

Correct AnswerverifiedShow Answer

A(n) ________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

Correct Answerverifiedformation constant o...View AnswerShow 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

Correct AnswerverifiedShow Answer

Which is the best choice for preparing a buffer with a pH of 3.5?

Correct AnswerverifiedShow Answer

A ________ helps maintain a constant pH even after the addition of acid or base.

Correct AnswerverifiedShow Answer

Which compound has the highest solubility in pure water?

Correct AnswerverifiedShow Answer

Which pair of substances is capable of forming a buffer in aqueous solution?

Correct AnswerverifiedShow Answer

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH3COOH(aq) H+(aq) + CH3COO-(aq)

Correct AnswerverifiedThe equilibrium shif...View AnswerShow Answer

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L. What is Ksp for this compound?

Correct AnswerverifiedShow Answer

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

Correct AnswerverifiedShow Answer

After the equivalence point, the titration curve of a weak acid is identical to that of a .

Correct Answer
verified

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 buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [K_a(HCOOH) = 1.7 × 10^-4]

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

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
formation constant o...
View 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? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
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Correct Answer
verified

Correct Answer
verified

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺(aq) + CH₃COO^-(aq)

Correct Answer
verified
The equilibrium shif...
View Answer

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L. What is K_sp for this compound?

Correct Answer
verified

Correct Answer
verified