Question 1

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of
4.77.Ka = 1.7 × 10-4

Accepted Answer

Prepare a solution h...

Question 2

A ___________ helps maintain a constant pH even after the addition of acid or base.

Accepted Answer

The answer of A ___________ helps maintain a constant pH...

Question 3

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

Question 4

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl.What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Accepted Answer

A)  1.26
B)  1.67
C)  12.33
D)  12.74
E)  13.03F) None of the above
G) A) and B)

Question 5

What happens to the solution if sodium acetate is added to a solution of acetic acid? CH3COOH(aq)  3COOH(aq)    H+ (aq) + CH3COO- (aq)  A) The equilibrium shifts to the right. B) There is an increase in percent ionization of acetic acid. C) Less of hydrogen ion is consumed. D) There is an increased concentration of acetate ions. E) Less of the acetate ion is consumed." class="answers-bank-image d-inline" rel="preload" > H+ (aq) + CH3COO- (aq)

Accepted Answer

A)  The equilibrium shifts to the right.
B)  There is an increase in percent ionization of acetic acid.
C)  Less of hydrogen ion is consumed.
D)  There is an increased concentration of acetate ions.
E)  Less of the acetate ion is consumed.F) A) and B)
G) A) and E)

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 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 C)
G) A) and B)

Question 7

A(n)________________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

Accepted Answer

formation constant o...

Question 8

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L.What is Ksp for this compound?

Accepted Answer

A)  1.8 × 10-4
B)  3.6 × 10-4
C)  1.3 × 10-7
D)  3.2 × 10-8
E)  2.8 × 10-14F) All of the above
G) A) and E)

Question 9

What is the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl? [Ka(HOCl) = 3.2 × 10-8]

Accepted Answer

A)  0.39
B)  3.94
C)  6.58
D)  7.49
E)  8.40F) C) and D)
G) A) and B)

Question 10

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution.What is the Ksp for Mg3(P O4) 2?

Accepted Answer

A)  7.46 × 10-11
B)  2.68 × 10-9
C)  5.19 × 10-24
D)  4.80 × 10-26
E)  1.20 × 10-26F) A) and E)
G) A) and D)

Question 11

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO.What is the pH of this buffer? [Ka (HCOOH) = 1.7 × 10-4]

Accepted Answer

A)  2.87
B)  3.72
C)  3.82
D)  3.95
E)  4.66F) A) and E)
G) B) and D)

Question 12

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Accepted Answer

A) True 
 B)False

Question 13

When a strong 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 equal to the pKa of the conjugate acid.
E)  is equal to the pKb of the base.F) A) and B)
G) None of the above

Question 14

Which compound has the lowest solubility in pure water?

Accepted Answer

A)  Ag2C2O4,Ksp = 1.0 × 10-11
B)  PbCl2,Ksp = 1.7 × 10-5
C)  FePO4,Ksp = 1.3 × 10-22
D)  Ca3(PO4) 2,Ksp = 1.2 × 10-26
E)  MgF2,Ksp = 6.9 × 10-9F) B) and E)
G) A) and E)

Question 15

The endpoint is used to estimate the equivalence point.

Accepted Answer

A) True 
 B)False

Question 16

What is the ion product expression for magnesium fluoride,MgF2?

Accepted Answer

A)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and C)
G) A) and B)

Question 17

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10-3 M Ba(NO3) 2 are added to 80.0 mL of 8.4 ×10-4M Na2CO3?

Accepted Answer

A)  Yes,the ppt is Ba(NO3) 2.
B)  Yes,the ppt is NaNO3.
C)  Yes,the ppt is BaCO3.
D)  Yes,the ppt is Na2CO3.
E)  No,a precipitate will not form.F) A) and B)
G) A) and E)

Question 18

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid?
CH3COOH(aq)

Accepted Answer

H⁺(aq)+ CH₃COO^-(aq)The equilibriu...

Question 19

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) B) and C)
G) A) and B)

Question 20

Explain why it is important that the amount of added strong acid not exceed the original amount of conjugate base present in the buffer.

Accepted Answer

All the added strong acid must...

Exam 17: Acid-Base Equilibria and Solubility Equilibria

The endpoint is used to estimate the equivalence point.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.Ka = 1.7 × 10-4

Correct AnswerverifiedPrepare a solution h...View AnswerShow 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

What happens to the solution if sodium acetate is added to a solution of acetic acid? CH3COOH(aq) H+ (aq) + CH3COO- (aq)

Correct AnswerverifiedShow Answer

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L.What is Ksp for this compound?

Correct AnswerverifiedShow Answer

Which compound has the lowest solubility in pure water?

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Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH3COOH(aq)

Correct AnswerverifiedH+(aq)+ CH3COO-(aq)The equilibriu...View AnswerShow Answer

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Correct AnswerverifiedShow Answer

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl.What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Correct AnswerverifiedShow Answer

Explain why it is important that the amount of added strong acid not exceed the original amount of conjugate base present in the buffer.

Correct AnswerverifiedAll the added strong acid must...View AnswerShow Answer

What is the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl? [Ka(HOCl) = 3.2 × 10-8]

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10-3 M Ba(NO3) 2 are added to 80.0 mL of 8.4 ×10-4M Na2CO3?

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

A ___________ helps maintain a constant pH even after the addition of acid or base.

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO.What is the pH of this buffer? [Ka (HCOOH) = 1.7 × 10-4]

Correct AnswerverifiedShow Answer

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution.What is the Ksp for Mg3(P O4) 2?

Correct AnswerverifiedShow Answer

A(n)________________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

Correct Answerverifiedformation constant o...View AnswerShow Answer

What is the ion product expression for magnesium fluoride,MgF2?

Correct AnswerverifiedShow Answer

Correct Answer
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Correct Answer
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Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.K_a = 1.7 × 10^-4

Correct Answer
verified
Prepare a solution h...
View Answer

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
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What happens to the solution if sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺ (aq) + CH₃COO^- (aq)

Correct Answer
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The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L.What is K_sp for this compound?

Correct Answer
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Correct Answer
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Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH₃COOH(aq)

Correct Answer
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H⁺(aq)+ CH₃COO^-(aq)The equilibriu...
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The pH of a solution that is 0.20 M CH₃COOH and 0.20 M CH₃COONa should be higher than the pH of a 0.20 M CH₃COOH solution.

Correct Answer
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Correct Answer
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Correct Answer
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All the added strong acid must...
View Answer

What is the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl? [K_a(HOCl) = 3.2 × 10^-8]

Correct Answer
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Correct Answer
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Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10^-3 M Ba(NO₃) ₂ are added to 80.0 mL of 8.4 ×10^-4M Na₂CO₃?

Correct Answer
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Correct Answer
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Correct Answer
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A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO.What is the pH of this buffer? [K_a (HCOOH) = 1.7 × 10^-4]

Correct Answer
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The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution.What is the K_sp for Mg₃(P O₄) ₂?

Correct Answer
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Correct Answer
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formation constant o...
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What is the ion product expression for magnesium fluoride,MgF₂?

Correct Answer
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