Question 1

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

Accepted Answer

A) True 
 B)False

Question 2

For the 1:1 ratio combination of a monoprotic strong acid and a monoprotic strong base, the ________ is where equal molar amounts of the strong acid and strong base have been combined.

Accepted Answer

The answer of For the 1:1 ratio combination of a...

Question 3

What is the effect on equilibrium when sodium acetate is added to a solution of acetic acid? CH3COOH(aq)  3COOH(aq)    H+(aq)  + CH3COO-(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)  + CH3COO-(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) A) and B)
G) A) and C)

Question 4

A CH3COOH/CH3COO- buffer can be produced by adding a strong acid to a solution of CH3COO- ions.

Accepted Answer

A) True 
 B)False

Question 5

The indicator propyl red has Ka = 3.3 × 10-6. What would be the approximate pH range over which it would change color?

Accepted Answer

A)   3.5 - 5.5
B)   4.5 - 6.5
C)   5.5 - 7.5
D)   6.5 - 8.5
E)   7.5 - 9.5F) All of the above
G) A) and E)

Question 6

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH)  and 0.30 M sodium acetate (CH3COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka(CH3COOH)  = 1.8 × 10-5]

Accepted Answer

A)   4.41
B)   4.74
C)   4.56
D)   4.92
E)   5.07F) C) and D)
G) None of the above

Question 7

Suppose 50.0 mL of a 0.100 M solution of the weak acid HA is titrated with a 0.100 M solution of NaOH. Which diagram best represents the equilibrium composition of the solution once 25.0 mL of titrant have been added? (Solvent water molecules are omitted for clarity.)

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) A) and B)
G) A) and C)

Question 8

What is the Henderson-Hasselbach equation?

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) All of the above
G) A) and E)

Question 9

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO)  and 1.0 mole of cyanic acid (HCNO)  in enough water to make 1.0 liter of solution. [Ka(HCNO)  = 2.0 × 10-4]

Accepted Answer

A)   0.00
B)   3.00
C)   3.70
D)   4.40
E)   5.00F) A) and D)
G) A) and E)

Question 10

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M)  with a strong base of the same concentration?

Accepted Answer

A)   2A (0.10 M)  with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2A (0.10 M)  with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2A (0.10 M)  with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2A (0.10 M)  with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2A (0.10 M)  with a strong base of the same concentration? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) B) and E)
G) A) and B)

Question 11

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. [Ksp(MgF2)  = 6.9 × 10-9]

Accepted Answer

A)   1.4 × 107 M
B)   6.9 × 10-9 M
C)   6.9 × 10-8 M
D)   1.7 × 10-7 M
E)   6.9 × 10-7 MF) A) and D)
G) B) and C)

Question 12

Consider the dissolution of MnS in water. [Ksp(MnS)  =3.0 × 10-14] MnS(s)  + H2O(l)  sp(MnS)  =3.0 × 10-14] MnS(s)  + H2O(l)    Mn2+(aq)  + HS-(aq)  + OH-(aq)  How is the solubility of manganese(II)  sulfide affected by the addition of aqueous potassium hydroxide to the system? 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." class="answers-bank-image d-inline" rel="preload" > Mn2+(aq)  + HS-(aq)  + OH-(aq) 
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) A) and B)
G) A) and C)

Question 13

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Accepted Answer

A)   1.0
B)   6.0
C)   7.0
D)   8.0
E)   13.0F) A) and D)
G) B) and E)

Question 14

The ________ is the solution that is added from the buret during a titration.

Accepted Answer

The answer of The ________ is the solution that is...

Question 15

A 50.00-mL solution of 0.10 M HNO2 is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, what is the pH in the titration flask? [Ka(HNO2)  = 4.5 × 10-4]

Accepted Answer

A)   2.17
B)   3.35
C)   2.41
D)   1.48
E)   7.00F) C) and D)
G) All of the above

Question 16

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution. (Each circle represents 1.0 ×10-3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are omitted for clarity.)  -3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are omitted for clarity.)    What is Ksp for MX? A)  1.5 ×10-5 B)  6.0 ×10-6 C)  3.6 ×10-1 D)  1.8 ×10-3 E)  9.0 ×10-6" class="answers-bank-image d-inline" rel="preload" > What is Ksp for MX?

Accepted Answer

A)   1.5 ×10-5
B)   6.0 ×10-6
C)   3.6 ×10-1
D)   1.8 ×10-3
E)   9.0 ×10-6F) B) and C)
G) C) and D)

Question 17

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 the pKb of the conjugate base.F) A) and B)
G) B) and D)

Question 18

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 M 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)   5.6 × 10-10 M
E)   9.3 × 10-10 MF) A) and B)
G) A) and C)

Question 19

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO3) 2. Which statement is correct? [Ksp(Ca(OH) 2)  = 6.5 × 10-6]

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)   Potassium nitrate precipitates until the solution is saturated.
E)   The presence of KOH will raise the solubility of Ca(NO3) 2.F) B) and D)
G) A) and B)

Question 20

What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid)  and 0.75 M NaHC6H6O6 (sodium ascorbate) ? [Ka(H2C6H6O6)  = 6.8 × 10-5]

Accepted Answer

A)   3.76
B)   3.99
C)   4.34
D)   4.57
E)   5.66F) D) and E)
G) B) and C)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M) with a strong base of the same concentration?

Correct AnswerverifiedShow Answer

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. [Ksp(MgF2) = 6.9 × 10-9]

Correct AnswerverifiedShow Answer

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution. (Each circle represents 1.0 ×10-3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are omitted for clarity.) What is Ksp for MX?

Correct AnswerverifiedShow Answer

A CH3COOH/CH3COO- buffer can be produced by adding a strong acid to a solution of CH3COO- ions.

Correct AnswerverifiedShow Answer

The ________ is the solution that is added from the buret during a titration.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid) and 0.75 M NaHC6H6O6 (sodium ascorbate) ? [Ka(H2C6H6O6) = 6.8 × 10-5]

Correct AnswerverifiedShow Answer

A 50.00-mL solution of 0.10 M HNO2 is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, what is the pH in the titration flask? [Ka(HNO2) = 4.5 × 10-4]

Correct AnswerverifiedShow Answer

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO3) 2. Which statement is correct? [Ksp(Ca(OH) 2) = 6.5 × 10-6]

Correct AnswerverifiedShow Answer

What is the [H3O+] in a solution that consists of 1.5 M NH3 and 2.5 M NH4Cl? Kb = 1.8 × 10-5

Correct AnswerverifiedShow Answer

Suppose 50.0 mL of a 0.100 M solution of the weak acid HA is titrated with a 0.100 M solution of NaOH. Which diagram best represents the equilibrium composition of the solution once 25.0 mL of titrant have been added? (Solvent water molecules are omitted for clarity.)

Correct AnswerverifiedShow Answer

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 × 10-4]

Correct AnswerverifiedShow Answer

For the 1:1 ratio combination of a monoprotic strong acid and a monoprotic strong base, the ________ is where equal molar amounts of the strong acid and strong base have been combined.

Correct AnswerverifiedShow Answer

The indicator propyl red has Ka = 3.3 × 10-6. What would be the approximate pH range over which it would change color?

Correct AnswerverifiedShow Answer

What is the Henderson-Hasselbach equation?

Correct AnswerverifiedShow Answer

Consider the dissolution of MnS in water. [Ksp(MnS) =3.0 × 10-14] MnS(s) + H2O(l) Mn2+(aq) + HS-(aq) + OH-(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct AnswerverifiedShow Answer

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H₂A (0.10 M) with a strong base of the same concentration?

Correct Answer
verified

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. [K_sp(MgF₂) = 6.9 × 10^-9]

Correct Answer
verified

Below is a representation of the sparingly soluble salt MX at equilibrium in aqueous solution. (Each circle represents 1.0 ×10^-3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are omitted for clarity.) What is K_sp for MX?

Correct Answer
verified

A CH₃COOH/CH₃COO^- buffer can be produced by adding a strong acid to a solution of CH₃COO^- ions.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH₃COOH) and 0.30 M sodium acetate (CH₃COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

What is the pH of a solution that consists of 0.50 M H₂C₆H₆O₆ (ascorbic acid) and 0.75 M NaHC₆H₆O₆ (sodium ascorbate) ? [K_a(H₂C₆H₆O₆) = 6.8 × 10^-5]

Correct Answer
verified

A 50.00-mL solution of 0.10 M HNO₂ is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, what is the pH in the titration flask? [K_a(HNO₂) = 4.5 × 10^-4]

Correct Answer
verified

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO₃) ₂. Which statement is correct? [K_sp(Ca(OH) ₂) = 6.5 × 10^-6]

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.5 M NH₃ and 2.5 M NH₄Cl? K_b = 1.8 × 10^-5

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [K_a(HCNO) = 2.0 × 10^-4]

Correct Answer
verified

Correct Answer
verified

The indicator propyl red has K_a = 3.3 × 10^-6. What would be the approximate pH range over which it would change color?

Correct Answer
verified

Correct Answer
verified

Consider the dissolution of MnS in water. [K_sp(MnS) =3.0 × 10^-14] MnS(s) + H₂O(l) Mn²⁺(aq) + HS^-(aq) + OH^-(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct Answer
verified