Question 1

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

Question 2

At the equivalence point in an acid-base titration

Accepted Answer

A)  the [H3O+] equals the Ka of the acid.
B)  the [H3O+] equals the Ka of the indicator.
C)  the amounts of acid and base which have been combined are in their stoichiometric ratio.
D)  the pH is 7.0.
E)  the pH has reached a maximum.F) B) and C)
G) A) and B)

Question 3

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Accepted Answer

A)  3.67
B)  3.78
C)  3.81
D)  3.85
E)  3.95F) C) and E)
G) C) and D)

Question 4

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

Question 5

Which of the following substances has the greatest solubility in water?

Accepted Answer

A)  Ba(IO3) 2,Ksp = 1.5  ×	imes×  10-9
B)  PbF2,Ksp = 3.6  ×	imes×  10-8
C)  SrSO4,Ksp = 3.2  ×	imes×  10-7
D)  CuCl,Ksp = 1.9  ×	imes×  10-7
E)  CdS,Ksp = 1.0  ×	imes×  10-24 F) A) and E)
G) A) and D)

Question 6

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

Accepted Answer

A)  HCl,NaCl
B)  HNO3,NaNO3
C)  H3PO4,H2PO4-
D)  H2SO4,CH3COOH
E)  NH3,NaOHF) B) and C)
G) B) and E)

Question 7

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8(ethylene diamine) and 0.35 C2N2H9Cl?
Kb = 4.7  ×	imes×  10-4

Accepted Answer

A)  2.0  ×	imes×  l0-3 M
B)  1.1  ×	imes×  10-3 M
C)  6.3  ×	imes×  10-9 M
D)  2.1  ×	imes×  10-10 M
E)  5.0  ×	imes×  10-11 M F) None of the above
G) A) and B)

Question 8

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4?
Ka = 6.2  ×	imes×  10-8

Accepted Answer

A)  6.51
B)  6.91
C)  7.51
D)  7.90
E)  8.13 F) B) and D)
G) A) and C)

Question 9

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

Question 10

The end point in a titration is defined as the point when the indicator changes color.

Accepted Answer

A) True 
 B)False

Question 11

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 B)
G) A) and C)

Question 12

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Accepted Answer

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

Question 13

Calculate the solubility of lead(II) iodide,PbI2,in 0.025 M KI.Ksp = 7.9  ×	imes×  10-9

Accepted Answer

A)  4.5  ×	imes×  10-2 M
B)  2.8  ×	imes×  10-2 M
C)  8.9  ×	imes×  10-5 M
D)  5.0  ×	imes×  10-5 M
E)  1.3  ×	imes×  10-5 M F) A) and B)
G) B) and D)

Question 14

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO3) 2.Which of the following statements is correct? Ksp = 6.44  ×	imes×  10-3 for CdF2

Accepted Answer

A)  Cadmium fluoride precipitates until the solution is saturated.
B)  The solution is unsaturated and no precipitate forms.
C)  The solubility of cadmium fluoride is increased by the presence of additional fluoride ions.
D)  One must know Ksp for cadmium nitrate to make meaningful predictions on this system.
E)  The presence of NaF will raise the solubility of Cd(NO3) 2. F) C) and D)
G) A) and E)

Question 15

Calculate the solubility of barium carbonate,BaCO3,in pure water.Ksp = 2.0  ×	imes×  10-9

Accepted Answer

A)  1.3  ×	imes×  10-3 M
B)  3.2  ×	imes×  10-5 M
C)  2.2  ×	imes×  10-5 M
D)  4.5  ×	imes×  10-5 M
E)  4.0  ×	imes×  10-18 M F) C) and D)
G) A) and B)

Question 16

Which of the following substances has the greatest solubility in water?

Accepted Answer

A)  PbI2,Ksp = 7.9  ×	imes×  10-9
B)  BaF2,Ksp = 1.5  ×	imes×  10-6
C)  Ca(OH) 2,Ksp = 6.5  ×	imes×  10-6
D)  Zn(IO3) 2,Ksp = 3.9  ×	imes×  10-6
E)  Ag2SO4,Ksp = 1.5  ×	imes×  10-5 F) A) and E)
G) A) and D)

Exam 19: Ionic Equilibria in Aqueous Systems

Which of the following substances has the greatest solubility in water?

Correct Answer
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A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO₃) ₂.Which of the following statements is correct? K_sp = 6.44 $\times$ 10^-3 for CdF₂

Correct Answer
verified

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

Correct Answer
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What is the pH of a buffer that consists of 0.20 M NaH₂PO₄ and 0.40 M Na₂HPO₄? K_a = 6.2 $\times$ 10^-8

Correct Answer
verified

Calculate the solubility of barium carbonate,BaCO₃,in pure water.K_sp = 2.0 $\times$ 10^-9

Correct Answer
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Which of the following has the highest buffer capacity?

Correct Answer
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Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Correct Answer
verified

The end point in a titration is defined as the point when the indicator changes color.

Correct Answer
verified

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct Answer
verified

Calculate the solubility of lead(II) iodide,PbI₂,in 0.025 M KI.K_sp = 7.9 $\times$ 10^-9

Correct Answer
verified

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

Correct Answer
verified

At the equivalence point in an acid-base titration

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

Which of the following substances has the greatest solubility in water?

Correct Answer
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Which of the following aqueous mixtures would be a buffer system?

Correct Answer
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What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈(ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 $\times$ 10^-4

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

Which of the following substances has the greatest solubility in water?

Correct AnswerverifiedShow Answer

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO3) 2.Which of the following statements is correct? Ksp = 6.44 ×\times× 10-3 for CdF2

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? Ka = 6.2 ×\times× 10-8

Correct AnswerverifiedShow Answer

Calculate the solubility of barium carbonate,BaCO3,in pure water.Ksp = 2.0 ×\times× 10-9

Correct AnswerverifiedShow Answer

Which of the following has the highest buffer capacity?

Correct AnswerverifiedShow Answer

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Correct AnswerverifiedShow Answer

The end point in a titration is defined as the point when the indicator changes color.

Correct AnswerverifiedShow Answer

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct AnswerverifiedShow Answer

Calculate the solubility of lead(II) iodide,PbI2,in 0.025 M KI.Ksp = 7.9 ×\times× 10-9

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

At the equivalence point in an acid-base titration

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

Which of the following substances has the greatest solubility in water?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8(ethylene diamine) and 0.35 C2N2H9Cl? Kb = 4.7 ×\times× 10-4

Correct AnswerverifiedShow Answer

Correct Answer
verified

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO₃) ₂.Which of the following statements is correct? K_sp = 6.44 $\times$ 10^-3 for CdF₂

Correct Answer
verified

Correct Answer
verified

What is the pH of a buffer that consists of 0.20 M NaH₂PO₄ and 0.40 M Na₂HPO₄? K_a = 6.2 $\times$ 10^-8

Correct Answer
verified

Calculate the solubility of barium carbonate,BaCO₃,in pure water.K_sp = 2.0 $\times$ 10^-9

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the solubility of lead(II) iodide,PbI₂,in 0.025 M KI.K_sp = 7.9 $\times$ 10^-9

Correct Answer
verified

Correct Answer
verified

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

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈(ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 $\times$ 10^-4

Correct Answer
verified