Question 1

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 E)
G) A) and D)

Question 2

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)  0.00F) C) and E)
G) A) and D)

Question 3

Which is more soluble in an acidic solution than in pure water?

Accepted Answer

A)  CH3CH2OH,ethanol
B)  Li2O
C)  C6H12O6,glucose
D)  CCl4
E)  ICl3F) A) and C)
G) A) and B)

Question 4

Suppose 3.0 ×10-3 mol of NaOH are added to 6.0 ×10-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)

Accepted Answer

A)   -3 mol of NaOH are added to 6.0 ×10-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)  
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B)     
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C)   -3 mol of NaOH are added to 6.0 ×10-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)  
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E)   -3 mol of NaOH are added to 6.0 ×10-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)  
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G) None of the above

Question 5

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10-5M AgNO3 are added to 200.0 mL of 2.5 × 10-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Accepted Answer

A)  Yes,the ppt is AgNO3(s) .
B)  Yes,the ppt is AgBr(s) .
C)  Yes,the ppt is NaBr(s) .
D)  Yes,the ppt is NaNO3(s) .
E)  No,a precipitate will not form.F) B) and C)
G) A) and B)

Question 6

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 at point X on the titration curve below? (Solvent water molecules are omitted for clarity.)

Accepted Answer

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

Question 7

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) A) and B)
G) All of the above

Question 8

Which of the following is correct?

Accepted Answer

A)  Solubility is the concentration of unsaturated ions in solution.
B)  Ksp is the same as the solubility.
C)  Ksp is an equilibrium constant and solubility is the concentration of a saturated solution.
D)  Ksp is the solubility product constant for a precipitate.
E)  Solubility = Kw × Ksp.F) All of the above
G) A) and C)

Question 9

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 10

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

Question 11

Which indicator would be the best to use if 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.050 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 - 8.5E) All of the above
F) B) and C)

Question 12

Which is included in the Ksp expression? I.Concentration of cation
II) Concentration of anion
III) Concentration of solid

Accepted Answer

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

Question 13

When sodium acetate is added to a solution of acetic acid,what happens to the pH of the solution?
Explain why this effect occurs?
CH3COOH(aq)  H+(aq)CH3COO-(aq)

Accepted Answer

The pH increases because the equilibrium...

Question 14

A mixture made of 100 mL of 0.5 M CH3COOH and 100 mL of 0.5 M CH3COONa is classified as a buffer solution.

Accepted Answer

A) True 
 B)False

Question 15

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

Question 16

The molar solubility of manganese(II) carbonate is 4.2 × 10-6 M.What is Ksp for this compound?

Accepted Answer

A)  4.2 × 10-6
B)  8.4 × 10-6
C)  3.0 × 10-16
D)  1.8 × 10-11
E)  2.0 × 10-3F) C) and D)
G) A) and C)

Question 17

If 50.0 mL of 1.2 × 10-3 M Pb(NO3) 2 are added to 50.0 mL of 2.0 × 10-4 M Na2S,what takes place?

Accepted Answer

A)  A precipitate of PbS forms.
B)  A precipitate of NaNO3 forms.
C)  A precipitate of Na2S forms.
D)  A precipitate of Pb(NO3) 2 forms.
E)  No precipitate forms.F) A) and B)
G) B) and E)

Question 18

Which pair of substances cannot form a buffered aqueous solution?

Accepted Answer

A)  HCN and KCN
B)  NH3 and (NH4) 2SO4
C)  HNO3 and NaNO3
D)  HF and NaF
E)  HNO2 and NaNO2F) B) and C)
G) None of the above

Question 19

After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid,the equilibrium pH is basic.What may be concluded about the identity of the acid?

Accepted Answer

A)  The acid can only be a strong monoprotic acid.
B)  The acid can only be a weak monoprotic acid.
C)  The acid must be a strong acid,but could be either monoprotic,diprotic,or polyprotic.
D)  The acid must be a weak acid,but could be either monoprotic,diprotic,or polyprotic.
E)  The acid could be either a strong or weak acid,and could be either a monoprotic,diprotic,orpolyprotic acid.F) B) and E)
G) C) and E)

Question 20

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? [Ka(CH3COOH) = 1.8 × 10-5]

Accepted Answer

A)  3.43
B)  4.64
C)  4.85
D)  4.74
E)  6.06F) B) and D)
G) A) and E)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Correct Answer
verified

Which is included in the K_sp expression? I.Concentration of cation II) Concentration of anion III) Concentration of solid

Correct Answer
verified

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 at point X on the titration curve below? (Solvent water molecules are omitted for clarity.)

Correct Answer
verified

The molar solubility of manganese(II) carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

Correct Answer
verified

Which indicator would be the best to use if 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.050 M NaOH?

Correct Answer
verified

Suppose 3.0 ×10^-3 mol of NaOH are added to 6.0 ×10^-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

Which is more soluble in an acidic solution than in pure water?

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

Which of the following is correct?

Correct Answer
verified

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10^-5M AgNO₃ are added to 200.0 mL of 2.5 × 10^-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Correct Answer
verified

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

Correct Answer
verified

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 Answer
verified

After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid,the equilibrium pH is basic.What may be concluded about the identity of the acid?

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

Which pair of substances cannot form a buffered aqueous solution?

Correct Answer
verified

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

Correct Answer
verified

When sodium acetate is added to a solution of acetic acid,what happens to the pH of the solution? Explain why this effect occurs? CH₃COOH(aq) H⁺(aq)CH₃COO^-(aq)

Correct Answer
verified
The pH increases because the equilibrium...
View Answer

If 50.0 mL of 1.2 × 10^-3 M Pb(NO₃) ₂ are added to 50.0 mL of 2.0 × 10^-4 M Na₂S,what takes place?

Correct Answer
verified

A mixture made of 100 mL of 0.5 M CH₃COOH and 100 mL of 0.5 M CH₃COONa is classified as a buffer solution.

Correct Answer
verified

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Correct AnswerverifiedShow Answer

Which is included in the Ksp expression? I.Concentration of cation II) Concentration of anion III) Concentration of solid

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 at point X on the titration curve below? (Solvent water molecules are omitted for clarity.)

Correct AnswerverifiedShow Answer

The molar solubility of manganese(II) carbonate is 4.2 × 10-6 M.What is Ksp for this compound?

Correct AnswerverifiedShow Answer

Which indicator would be the best to use if 0.050 M benzoic acid (Ka = 6.6 × 10-5) is titrated with 0.050 M NaOH?

Correct AnswerverifiedShow Answer

Suppose 3.0 ×10-3 mol of NaOH are added to 6.0 ×10-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? [Ka(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

Which is more soluble in an acidic solution than in pure water?

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

Which of the following is correct?

Correct AnswerverifiedShow Answer

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10-5M AgNO3 are added to 200.0 mL of 2.5 × 10-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Correct AnswerverifiedShow Answer

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

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

After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid,the equilibrium pH is basic.What may be concluded about the identity of the acid?

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

Which pair of substances cannot form a buffered aqueous solution?

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

When sodium acetate is added to a solution of acetic acid,what happens to the pH of the solution? Explain why this effect occurs? CH3COOH(aq) H+(aq)CH3COO-(aq)

Correct AnswerverifiedThe pH increases because the equilibrium...View AnswerShow Answer

If 50.0 mL of 1.2 × 10-3 M Pb(NO3) 2 are added to 50.0 mL of 2.0 × 10-4 M Na2S,what takes place?

Correct AnswerverifiedShow Answer

A mixture made of 100 mL of 0.5 M CH3COOH and 100 mL of 0.5 M CH3COONa is classified as a buffer solution.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Which is included in the K_sp expression? I.Concentration of cation II) Concentration of anion III) Concentration of solid

Correct Answer
verified

Correct Answer
verified

The molar solubility of manganese(II) carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

Correct Answer
verified

Which indicator would be the best to use if 0.050 M benzoic acid (K_a = 6.6 × 10^-5) is titrated with 0.050 M NaOH?

Correct Answer
verified

Suppose 3.0 ×10^-3 mol of NaOH are added to 6.0 ×10^-3 mol of the weak acid HA.Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of each box is 1.0 L.Solvent water molecules are omitted for clarity.)

Correct Answer
verified

What is the pH of a buffer that consists of 0.45 M CH₃COOH and 0.35 M CH₃COONa? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
verified

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

Correct Answer
verified

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10^-5M AgNO₃ are added to 200.0 mL of 2.5 × 10^-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Correct Answer
verified

Correct Answer
verified

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 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

Correct Answer
verified

Correct Answer
verified

When sodium acetate is added to a solution of acetic acid,what happens to the pH of the solution? Explain why this effect occurs? CH₃COOH(aq) H⁺(aq)CH₃COO^-(aq)

Correct Answer
verified
The pH increases because the equilibrium...
View Answer

If 50.0 mL of 1.2 × 10^-3 M Pb(NO₃) ₂ are added to 50.0 mL of 2.0 × 10^-4 M Na₂S,what takes place?

Correct Answer
verified

A mixture made of 100 mL of 0.5 M CH₃COOH and 100 mL of 0.5 M CH₃COONa is classified as a buffer solution.

Correct Answer
verified