Question 1

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 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)  4.65
B)  4.71
C)  4.56
D)  4.84
E)  5.07F) A) and E)
G) A) and D)

Question 2

A(n)________________ is an ion containing a central metal cation bonded to one or more molecules or ions.

Accepted Answer

The answer of A(n)________________ is an ion containing a central...

Question 3

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 4

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

Question 5

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

Question 6

What is the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution? [Ka(HCNO) = 2.0 × 10-4]

Accepted Answer

A)  0.97
B)  3.10
C)  4.40
D)  3.70
E)  4.30F) C) and D)
G) A) and E) E

Question 7

Which cation would form an insoluble chloride when reacted with HCl?

Accepted Answer

A)  Na+
B)  Ag+
C)  B3+
D)  Ca2+
E)  Cs+F) A) and B)
G) A) and C) B

Question 8

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

Question 9

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

Accepted Answer

A)  CuI
B)  PbCl2
C)  Ca3(PO4) 2
D)  NaNO3
E)  NaBrF) A) and D)
G) A) and B)

Question 10

The amount of strong acid added to a buffer solution cannot exceed the original amount of conjugate base present in order for the buffer to still work.

Accepted Answer

A) True 
 B)False

Question 11

For a conjugate acid-base pair,Kw = Ka /Kb

Accepted Answer

A) True 
 B)False

Question 12

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 C)
G) A) and B)

Question 13

The solubility of lead(II) chloride is 0.45 g/100 mL of solution.What is the Ksp of PbCl2?

Accepted Answer

A)  4.9 × 10-2
B)  1.7 × 10-5
C)  8.5 × 10-6
D)  4.2 × 10-6
E)  2.6 × 10-4F) B) and C)
G) C) and D)

Question 14

Which pair of substances could form a buffered aqueous solution?

Accepted Answer

A)  HCl,NaCl
B)  HNO3,NaNO3
C)  H3PO4,Na H2PO4
D)  H SO4,CH3COOH
E)  NH3,NaOHF) A) and C)
G) None of the above

Question 15

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

Question 16

mL of 3.0 M NH3?
(Kf for Ag(NH3)2+ is 1.5 × 107; Ksp (AgCl)= 1.6 × 10-10)

Accepted Answer

Question 17

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

Question 18

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

Question 19

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3) 2 with 50.0 mL of 0.50 M Co(NO3) 2. Sodium hydroxide is slowly added to the mixture.Which precipitates first?
[Ksp(Cu(OH) 2) = 2.2 × 10-20,Ksp(Co(OH) 2) = 1.3 × 10-15]

Accepted Answer

A)  Co(OH) 2
B)  Co(NO3) 2
C)  Cu(NO3) 2
D)  Cu(OH) 2
E)  No precipitate is formed.F) B) and C)
G) All of the above

Question 20

What is the name of the principle of selective precipitation used to identify the types of ions present in a solution?

Accepted Answer

A)  Ionization
B)  Selective ion precipitation
C)  Selective ion typing
D)  Limited precipitation
E)  Qualitative analysisF) C) and D)
G) A) and B)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 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

A(n)________________ is an ion containing a central metal cation bonded to one or more molecules or ions.

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

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 AnswerverifiedB

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 pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution? [Ka(HCNO) = 2.0 × 10-4]

Correct AnswerverifiedE

Which cation would form an insoluble chloride when reacted with HCl?

Correct AnswerverifiedB

Which compound has the highest solubility in pure water?

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

Correct AnswerverifiedShow Answer

The amount of strong acid added to a buffer solution cannot exceed the original amount of conjugate base present in order for the buffer to still work.

Correct AnswerverifiedShow Answer

For a conjugate acid-base pair,Kw = Ka /Kb

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The solubility of lead(II) chloride is 0.45 g/100 mL of solution.What is the Ksp of PbCl2?

Correct AnswerverifiedShow Answer

Which pair of substances could form a buffered aqueous solution?

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

mL of 3.0 M NH3? (Kf for Ag(NH3)2+ is 1.5 × 107; Ksp (AgCl)= 1.6 × 10-10)

Correct AnswerverifiedShow Answer

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

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

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3) 2 with 50.0 mL of 0.50 M Co(NO3) 2. Sodium hydroxide is slowly added to the mixture.Which precipitates first? [Ksp(Cu(OH) 2) = 2.2 × 10-20,Ksp(Co(OH) 2) = 1.3 × 10-15]

Correct AnswerverifiedShow Answer

What is the name of the principle of selective precipitation used to identify the types of ions present in a solution?

Correct AnswerverifiedShow Answer

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH₃COOH) and 0.20 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
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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

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B

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What is the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution? [K_a(HCNO) = 2.0 × 10^-4]

Correct Answer
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E

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B

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For a conjugate acid-base pair,K_w = K_a /K_b

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The solubility of lead(II) chloride is 0.45 g/100 mL of solution.What is the K_sp of PbCl₂?

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?

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mL of 3.0 M NH₃? (Kf for Ag(NH₃)₂⁺ is 1.5 × 10⁷; K_sp (AgCl)= 1.6 × 10^-10)

Correct Answer
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Correct Answer
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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
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A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO₃) ₂ with 50.0 mL of 0.50 M Co(NO₃) ₂. Sodium hydroxide is slowly added to the mixture.Which precipitates first? [K_sp(Cu(OH) ₂) = 2.2 × 10^-20,K_sp(Co(OH) ₂) = 1.3 × 10^-15]

Correct Answer
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Correct Answer
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