Question 1

Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA with a 0.100 M solution of NaOH. a of HA? A) 4 B) 6 C) 8 D) 9 E) 12" class="answers-bank-image d-inline" rel="preload" > What is the approximate pKa of HA?

Accepted Answer

A)  4
B)  6
C)  8
D)  9
E)  12F) A) and C)
G) C) and D)

Question 2

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

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

Question 3

Bromothymol blue is a common acid-base indicator.It has a Ka equal to 1.6 × 10-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

Accepted Answer

Question 4

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 E)
G) B) and E)

Question 5

An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74.What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Accepted Answer

A)  4.77
B)  4.71
C)  4.68
D)  4.62
E)  1.70.F) B) and E)
G) A) and D)

Question 6

What is the pH of a buffer that consists of 0.20 M Na H2PO4 and 0.40 M Na2HPO4? [Ka(Na H2PO4) = 6.2 × 10-8]

Accepted Answer

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

Question 7

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

Accepted Answer

A) True 
 B)False

Question 8

Which is more soluble in a basic solution than in pure water?

Accepted Answer

A)  Mg(OH) 2
B)  CaHPO4
C)  NaCl
D)  CaCO3
E)  AgIF) C) and D)
G) A) and C)

Question 9

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa) .(Ka = 6.5 × 10-5 for benzoic acid)

Accepted Answer

A)  3.97
B)  4.83
C)  4.19
D)  3.40
E)  4.41F) A) and D)
G) B) and E)

Question 10

When the concentration of the conjugate base of a weak acid is less than the concentration of the weak acid in a buffer solution,the pH of the solution is

Accepted Answer

A)  less than the pKa.
B)  greater than the pKa.
C)  always acidic.
D)  always basic.
E)  equal to the pKa.F) D) and E)
G) B) and E)

Question 11

Calculate the NaOH concentration necessary to precipitate Ca(OH) 2 from a solution in which [Ca2+] = 1.0.Ksp of Ca(OH) 2 = 8 x 10-6.

Accepted Answer

A)  6.7 x 10-8 M
B)  2.8 x 10-3 M
C)  1.5 x 10-7 M
D)  0.10 ME) B) and C)
F) A) and D)

Question 12

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH.What is the pH of this buffer? [Ka(CH3COOH) = 1.8 × 10-5]

Accepted Answer

A)  4.57
B)  4.52
C)  4.87
D)  4.92
E)  4.97F) D) and E)
G) A) and E)

Question 13

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

Question 14

_______________ is the way to identify the types of ions in a solution using selective precipitation.

Accepted Answer

Qualitativ...

Question 15

The ___________________ is the point in a titration where neutralization is complete.

Accepted Answer

The answer of The ___________________ is the point in a...

Question 16

A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NaOH.What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Accepted Answer

A)  1.00
B)  3.13
C)  10.87
D)  11.05
E)  13.14F) None of the above
G) C) and D)

Question 17

Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10-3 M MgCl2 are added to 500.0 mL of 1.2 × 10-3 M NaF?
[Ksp (MgF2) = 6.9 × 10-9]

Accepted Answer

A)  Yes,because Q > Ksp.
B)  No,because Q sp.
C)  No,because Q = Ksp.
D)  Yes,because Q sp.
E)  No,because Q > Ksp.F) B) and E)
G) C) and D)

Question 18

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 19

Which of the following compounds is appreciably more soluble in 1 M HNO3 than in pure water?

Accepted Answer

A)  FeCO3
B)  AgBr
C)  BaSO4
D)  NaNO3
E)  NaClF) A) and C)
G) All of the above

Question 20

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH.The following data were collected during the titration.Determine to Ka for HClO. mL NaOH added
5) 00
10) 00
15) 00
20) 00
PH
6) 98
7) 46
7) 93
10) 31

Accepted Answer

A)  1.1 × 10-7
B)  3.5 × 10-8
C)  1.2 × 10-8
D)  4.9 × 10-11
E)  None of the answers is correct.F) A) and B)
G) A) and C)

Exam 17: Acid-Base Equilibria and Solubility Equilibria

What is the pH of a buffer that consists of 0.20 M Na H2PO4 and 0.40 M Na2HPO4? [Ka(Na H2PO4) = 6.2 × 10-8]

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

The ___________________ is the point in a titration where neutralization is complete.

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Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10-3 M MgCl2 are added to 500.0 mL of 1.2 × 10-3 M NaF? [Ksp (MgF2) = 6.9 × 10-9]

Correct AnswerverifiedShow Answer

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH.The following data were collected during the titration.Determine to Ka for HClO. mL NaOH added 5) 00 10) 00 15) 00 20) 00 PH 6) 98 7) 46 7) 93 10) 31

Correct AnswerverifiedShow Answer

Bromothymol blue is a common acid-base indicator.It has a Ka equal to 1.6 × 10-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

Correct AnswerverifiedShow Answer

Which of the following compounds is appreciably more soluble in 1 M HNO3 than in pure water?

Correct AnswerverifiedShow Answer

A 20.00-mL sample of 0.3000 M HBr is titrated with 0.15 M NaOH.What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

When the concentration of the conjugate base of a weak acid is less than the concentration of the weak acid in a buffer solution,the pH of the solution is

Correct AnswerverifiedShow Answer

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa) .(Ka = 6.5 × 10-5 for benzoic acid)

Correct AnswerverifiedShow Answer

Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA with a 0.100 M solution of NaOH. What is the approximate pKa of HA?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

_______________ is the way to identify the types of ions in a solution using selective precipitation.

Correct AnswerverifiedQualitativ...View AnswerShow 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

Calculate the NaOH concentration necessary to precipitate Ca(OH) 2 from a solution in which [Ca2+] = 1.0.Ksp of Ca(OH) 2 = 8 x 10-6.

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH.What is the pH of this buffer? [Ka(CH3COOH) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74.What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which is more soluble in a basic solution than in pure water?

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.20 M Na H₂PO₄ and 0.40 M Na₂HPO₄? [K_a(Na H₂PO₄) = 6.2 × 10^-8]

Correct Answer
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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
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Correct Answer
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Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10^-3 M MgCl₂ are added to 500.0 mL of 1.2 × 10^-3 M NaF? [K_sp (MgF₂) = 6.9 × 10^-9]

Correct Answer
verified

A 20.0-mL sample of 0.30 M HClO was titrated with 0.30 M NaOH.The following data were collected during the titration.Determine to K_a for HClO. mL NaOH added 5) 00 10) 00 15) 00 20) 00 PH 6) 98 7) 46 7) 93 10) 31

Correct Answer
verified

Bromothymol blue is a common acid-base indicator.It has a K_a equal to 1.6 × 10^-7.Its un-ionized form is yellow and its conjugate base is blue.What color would a solution have at pH = 5.8?

Correct Answer
verified

Which of the following compounds is appreciably more soluble in 1 M HNO₃ than in pure water?

Correct Answer
verified

Correct Answer
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Correct Answer
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Correct Answer
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Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C₆H₅CO₂H) and 0.15 M sodium benzoate (C₆H₅COONa) .(K_a = 6.5 × 10^-5 for benzoic acid)

Correct Answer
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Below is a titration curve for the titration of 50.0 mL of a 0.100 M solution of the weak acid HA with a 0.100 M solution of NaOH. What is the approximate pK_a of HA?

Correct Answer
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Correct Answer
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Correct Answer
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Qualitativ...
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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
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Calculate the NaOH concentration necessary to precipitate Ca(OH) ₂ from a solution in which [Ca²⁺] = 1.0.K_sp of Ca(OH) ₂ = 8 x 10^-6.

Correct Answer
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A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH.What is the pH of this buffer? [K_a(CH₃COOH) = 1.8 × 10^-5]

Correct Answer
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An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74.What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct Answer
verified

Correct Answer
verified

Correct Answer
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