Question 1

A buffer solution

Accepted Answer

A)  contains more than the expected amount of solute for a particular temperature and is therefore unstable 
B)  contains the maximum amount of solute possible for a particular temperature 
C)  changes color upon addition of strong base 
D)  contains an equal number of hydronium and hydroxide ions 
E)  resists changes in pH upon addition of acid or base 
A)  contains more than the expected amount of solute for a particular temperature and is therefore unstable 
B)  contains the maximum amount of solute possible for a particular temperature 
C)  changes color upon addition of strong base 
D)  contains an equal number of hydronium and hydroxide ions 
E)  resists changes in pH upon addition of acid or base E

Question 2

A mixture of two metal ions in solution is to be separated by selective precipitation. As the concentration of the precipitating ion is increased, which metal ion precipitates first?

Accepted Answer

A)  The one with the lower value of Ksp for its precipitate 
B)  The one with the higher value of Ksp for its precipitate 
C)  The one present at higher concentration 
D)  The one present at lower concentration 
E)  Cannot answer the question without more information 
A)  The one with the lower value of Ksp for its precipitate 
B)  The one with the higher value of Ksp for its precipitate 
C)  The one present at higher concentration 
D)  The one present at lower concentration 
E)  Cannot answer the question without more information E

Question 3

In order to make up a buffer solution with a neutral pH, it would be best to make use of

Accepted Answer

A)  a weak acid with a Ka at or near 1.00 × 107 and its conjugate base 
B)  a weak acid with a pKa near 7.00 or a Ka near 1.00 × 10-7 and its conjugate base 
C)  an equimolar mixture of a strong acid and a strong base 
D)  an equimolar mixture of an extremely weak acid and an extremely strong base 
E)  an equimolar mixture of NaCl and HCl 
A)  a weak acid with a Ka at or near 1.00 × 107 and its conjugate base 
B)  a weak acid with a pKa near 7.00 or a Ka near 1.00 × 10-7 and its conjugate base 
C)  an equimolar mixture of a strong acid and a strong base 
D)  an equimolar mixture of an extremely weak acid and an extremely strong base 
E)  an equimolar mixture of NaCl and HCl B

Question 4

Which formula represents the Henderson-Hasselbalch equation for the generic acid HA?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 5

When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact volume of 0.55 M NaOH required to convert the acid to its conjugate base, at the endpoint the solution will have a

Accepted Answer

A)  pH  7.00 
C)  pH = 7.00 
D)  pH a 
E)  pH = pKa 
A)  pH  7.00 
C)  pH = 7.00 
D)  pH a 
E)  pH = pKa

Question 6

What is the minimum volume of 0.55 M NaOH required to completely convert 1.00 L of 0.45 M acetic acid (pKa = 4.74) to its conjugate base?

Accepted Answer

A)  0.82 L 
B)  1.0 L 
C)  1.2 L 
D)  1.8 L 
E)  2.2 L 
A)  0.82 L 
B)  1.0 L 
C)  1.2 L 
D)  1.8 L 
E)  2.2 L

Question 7

If solid sodium chloride is added to a saturated aqueous solution of sodium chloride

Accepted Answer

A)  the total dissolved solids concentration in the solution will increase 
B)  the anion concentration in the solution will increase 
C)  the cation concentration in the solution will increase 
D)  both the anion and anion concentrations in the solution will decrease 
E)  there will be no change in the anion or cation concentrations in the solution 
A)  the total dissolved solids concentration in the solution will increase 
B)  the anion concentration in the solution will increase 
C)  the cation concentration in the solution will increase 
D)  both the anion and anion concentrations in the solution will decrease 
E)  there will be no change in the anion or cation concentrations in the solution

Question 8

A buffer solution is 0.500 M in acetic acid and 0.500 M in sodium acetate. Its pH is 4.74. What is its pH after dilution by a factor of 2?

Accepted Answer

A)  4.44 
B)  4.49 
C)  4.74 
D)  4.99 
E)  5.04 
A)  4.44 
B)  4.49 
C)  4.74 
D)  4.99 
E)  5.04

Question 9

Isotonic saline solution is 0.154 M NaCl(aq). What is the solubility of AgCl (Ksp = 1.8 × 10-10) in such a solution?

Accepted Answer

A)  2.8 × 10-11 M 
B)  1.2 × 10-9 M 
C)  5.3 × 10-6 M 
D)  3.4 × 10-5 M 
E)  0.077 M 
A)  2.8 × 10-11 M 
B)  1.2 × 10-9 M 
C)  5.3 × 10-6 M 
D)  3.4 × 10-5 M 
E)  0.077 M

Question 10

Will a precipitate form when 10.0 mL of 0.500 M NaCl is added to 10.0 mL of 0.0500 M AgNO3? The Ksp for AgCl is 1.8 × 10-10.

Accepted Answer

A)  Yes, because Q sp 
B)  Yes, because Q = Ksp 
C)  Yes, because Q > Ksp 
D)  No, because Q sp 
E)  No, because Q > Ksp 
A)  Yes, because Q sp 
B)  Yes, because Q = Ksp 
C)  Yes, because Q > Ksp 
D)  No, because Q sp 
E)  No, because Q > Ksp

Question 11

Answer the following questions:
a.	Explain why the solubility of carbonates and phosphates is increased by lowering the pH, but the solubility of chlorides is unaffected by lowering the pH.
b.	The solubility of copper(II) carbonate is dramatically increased by the addition of NH3, but the solubility of copper(II) phosphate is not. Referring to the data below, explain why.

Ksp for copper(II) carbonate = 2.5 ´ 10-10
Ksp for copper(II) phosphate = 1.4 ´ 10-37
Cu2+(aq) + 4 NH3(aq) 
(Kf = 1.1 ´ 1013)
 
(aq)

Accepted Answer

a. The carbonate and phosphate ions are

Question 12

A 50.00 mL sample of 0.0950 M acetic acid (Ka = 1.8 × 10-5) is being titrated with 0.0848 M NaOH. What is the pH after 28.00 mL of NaOH has been added?

Accepted Answer

A)  5.04 
B)  4.74 
C)  4.44 
D)  3.18 
E)  3.06 
A)  5.04 
B)  4.74 
C)  4.44 
D)  3.18 
E)  3.06

Question 13

A solution contains 0.100 M Pb(NO3)2 and 1.00 × 10-5 M AgNO3. It is intended to separate out the silver by selective precipitation of AgI. What is the maximum percentage of the total silver that can be recovered free of contamination by PbI2?

Accepted Answer

For PbI₂, K_sp = [Pb²⁺][I^-]² Þ [I^-] = Ö(K_sp/[Pb²⁺]).

Question 14

To make a buffer using acetic acid one could add

Accepted Answer

A)  carbonic acid 
B)  sodium acetate 
C)  sodium chloride 
D)  ammonium chloride 
E)  ammonium phosphate 
A)  carbonic acid 
B)  sodium acetate 
C)  sodium chloride 
D)  ammonium chloride 
E)  ammonium phosphate

Question 15

What is the largest mass of solid NaCl that can be dissolved in 1.000 L of 5.00 × 10-3 M AgNO3 without a precipitate of AgCl forming? Ksp for AgCl is 1.8 × 10-10.

Accepted Answer

A)  0.78 mg 
B)  86 mg 
C)  13 mg 
D)  2.1 mg 
E)  36 ng 
A)  0.78 mg 
B)  86 mg 
C)  13 mg 
D)  2.1 mg 
E)  36 ng

Question 16

In how many different pairs can these substances be mixed to produce buffer solutions?

Accepted Answer

A)  2 
B)  3 
C)  4 
D)  5 
E)  6 
A)  2 
B)  3 
C)  4 
D)  5 
E)  6

Question 17

The solubility of silver chloride in water is increased by the addition of NH3. Why?

Accepted Answer

A)  The solubility of many salts is affected by the pH of the solution. 
B)  The formation of complex ions displaces the solubility equilibrium to the right. 
C)  The solubility of most salts increases as temperature increases. 
D)  Some insoluble compounds are amphoteric. 
E)  A common ion displaces the solubility equilibrium toward the undissolved solute. 
A)  The solubility of many salts is affected by the pH of the solution. 
B)  The formation of complex ions displaces the solubility equilibrium to the right. 
C)  The solubility of most salts increases as temperature increases. 
D)  Some insoluble compounds are amphoteric. 
E)  A common ion displaces the solubility equilibrium toward the undissolved solute.

Question 18

In which aqueous solution would the smallest amount of barium sulfate dissolve?

Accepted Answer

A)  0.1 M Mg(OH)2 
B)  0.1 M Na2SO4 
C)  0.1 M Al2(SO4)3 
D)  0.1 M Ba(NO3)2 
E)  0.1 M HCl 
A)  0.1 M Mg(OH)2 
B)  0.1 M Na2SO4 
C)  0.1 M Al2(SO4)3 
D)  0.1 M Ba(NO3)2 
E)  0.1 M HCl

Question 19

What volume of 0.1060 M NaOH is needed to neutralize a 50.00 mL sample of 0.09500 M HNO3?

Accepted Answer

A)  55.79 mL 
B)  55.19 mL 
C)  50.00 mL 
D)  44.81 mL 
E)  5.19 mL 
A)  55.79 mL 
B)  55.19 mL 
C)  50.00 mL 
D)  44.81 mL 
E)  5.19 mL

Question 20

Exhibit 16-1 The following question(s) refer to the same titration: a 50.00 mL sample of 0.0950 M acetic acid (Ka = 1.8 × 10-5) is being titrated with 0.106 M NaOH.
Refer to Exhibit 16-1. What is the pH at the midpoint of the titration?

Accepted Answer

A)  3.06 
B)  3.18 
C)  4.44 
D)  4.74 
E)  5.04 
A)  3.06 
B)  3.18 
C)  4.44 
D)  4.74 
E)  5.04

A buffer solution

A mixture of two metal ions in solution is to be separated by selective precipitation. As the concentration of the precipitating ion is increased, which metal ion precipitates first?

In order to make up a buffer solution with a neutral pH, it would be best to make use of

Which formula represents the Henderson-Hasselbalch equation for the generic acid HA?

When 1.00 L of 0.45 M acetic acid (pK_a = 4.74) is mixed with the exact volume of 0.55 M NaOH required to convert the acid to its conjugate base, at the endpoint the solution will have a

What is the minimum volume of 0.55 M NaOH required to completely convert 1.00 L of 0.45 M acetic acid (pK_a = 4.74) to its conjugate base?

If solid sodium chloride is added to a saturated aqueous solution of sodium chloride

A buffer solution is 0.500 M in acetic acid and 0.500 M in sodium acetate. Its pH is 4.74. What is its pH after dilution by a factor of 2?

Isotonic saline solution is 0.154 M NaCl(aq). What is the solubility of AgCl (K_sp = 1.8 × 10^-10) in such a solution?

Will a precipitate form when 10.0 mL of 0.500 M NaCl is added to 10.0 mL of 0.0500 M AgNO₃? The K_sp for AgCl is 1.8 × 10^-10.

A 50.00 mL sample of 0.0950 M acetic acid (K_a = 1.8 × 10^-5) is being titrated with 0.0848 M NaOH. What is the pH after 28.00 mL of NaOH has been added?

A solution contains 0.100 M Pb(NO₃)₂ and 1.00 × 10^-5 M AgNO₃. It is intended to separate out the silver by selective precipitation of AgI. What is the maximum percentage of the total silver that can be recovered free of contamination by PbI₂?

To make a buffer using acetic acid one could add

What is the largest mass of solid NaCl that can be dissolved in 1.000 L of 5.00 × 10^-3 M AgNO₃ without a precipitate of AgCl forming? K_sp for AgCl is 1.8 × 10^-10.

In how many different pairs can these substances be mixed to produce buffer solutions?

The solubility of silver chloride in water is increased by the addition of NH₃. Why?

In which aqueous solution would the smallest amount of barium sulfate dissolve?

What volume of 0.1060 M NaOH is needed to neutralize a 50.00 mL sample of 0.09500 M HNO₃?

Exhibit 16-1 The following question(s) refer to the same titration: a 50.00 mL sample of 0.0950 M acetic acid (K_a = 1.8 × 10^-5) is being titrated with 0.106 M NaOH. Refer to Exhibit 16-1. What is the pH at the midpoint of the titration?

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Exam 16: Additional Aqueous Equilibria

A buffer solution

A mixture of two metal ions in solution is to be separated by selective precipitation. As the concentration of the precipitating ion is increased, which metal ion precipitates first?

In order to make up a buffer solution with a neutral pH, it would be best to make use of

Which formula represents the Henderson-Hasselbalch equation for the generic acid HA?

When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact volume of 0.55 M NaOH required to convert the acid to its conjugate base, at the endpoint the solution will have a

What is the minimum volume of 0.55 M NaOH required to completely convert 1.00 L of 0.45 M acetic acid (pKa = 4.74) to its conjugate base?

If solid sodium chloride is added to a saturated aqueous solution of sodium chloride

A buffer solution is 0.500 M in acetic acid and 0.500 M in sodium acetate. Its pH is 4.74. What is its pH after dilution by a factor of 2?

Isotonic saline solution is 0.154 M NaCl(aq). What is the solubility of AgCl (Ksp = 1.8 × 10-10) in such a solution?

Will a precipitate form when 10.0 mL of 0.500 M NaCl is added to 10.0 mL of 0.0500 M AgNO3? The Ksp for AgCl is 1.8 × 10-10.

A 50.00 mL sample of 0.0950 M acetic acid (Ka = 1.8 × 10-5) is being titrated with 0.0848 M NaOH. What is the pH after 28.00 mL of NaOH has been added?

A solution contains 0.100 M Pb(NO3)2 and 1.00 × 10-5 M AgNO3. It is intended to separate out the silver by selective precipitation of AgI. What is the maximum percentage of the total silver that can be recovered free of contamination by PbI2?

To make a buffer using acetic acid one could add

What is the largest mass of solid NaCl that can be dissolved in 1.000 L of 5.00 × 10-3 M AgNO3 without a precipitate of AgCl forming? Ksp for AgCl is 1.8 × 10-10.

In how many different pairs can these substances be mixed to produce buffer solutions?

The solubility of silver chloride in water is increased by the addition of NH3. Why?

In which aqueous solution would the smallest amount of barium sulfate dissolve?

What volume of 0.1060 M NaOH is needed to neutralize a 50.00 mL sample of 0.09500 M HNO3?

Exhibit 16-1 The following question(s) refer to the same titration: a 50.00 mL sample of 0.0950 M acetic acid (Ka = 1.8 × 10-5) is being titrated with 0.106 M NaOH. Refer to Exhibit 16-1. What is the pH at the midpoint of the titration?

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Thermodynamics: Directionality of Chemical Reactions

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Nuclear Chemistry

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When 1.00 L of 0.45 M acetic acid (pK_a = 4.74) is mixed with the exact volume of 0.55 M NaOH required to convert the acid to its conjugate base, at the endpoint the solution will have a

What is the minimum volume of 0.55 M NaOH required to completely convert 1.00 L of 0.45 M acetic acid (pK_a = 4.74) to its conjugate base?

Isotonic saline solution is 0.154 M NaCl(aq). What is the solubility of AgCl (K_sp = 1.8 × 10^-10) in such a solution?

Will a precipitate form when 10.0 mL of 0.500 M NaCl is added to 10.0 mL of 0.0500 M AgNO₃? The K_sp for AgCl is 1.8 × 10^-10.

A 50.00 mL sample of 0.0950 M acetic acid (K_a = 1.8 × 10^-5) is being titrated with 0.0848 M NaOH. What is the pH after 28.00 mL of NaOH has been added?

A solution contains 0.100 M Pb(NO₃)₂ and 1.00 × 10^-5 M AgNO₃. It is intended to separate out the silver by selective precipitation of AgI. What is the maximum percentage of the total silver that can be recovered free of contamination by PbI₂?

What is the largest mass of solid NaCl that can be dissolved in 1.000 L of 5.00 × 10^-3 M AgNO₃ without a precipitate of AgCl forming? K_sp for AgCl is 1.8 × 10^-10.

The solubility of silver chloride in water is increased by the addition of NH₃. Why?

What volume of 0.1060 M NaOH is needed to neutralize a 50.00 mL sample of 0.09500 M HNO₃?

Exhibit 16-1 The following question(s) refer to the same titration: a 50.00 mL sample of 0.0950 M acetic acid (K_a = 1.8 × 10^-5) is being titrated with 0.106 M NaOH. Refer to Exhibit 16-1. What is the pH at the midpoint of the titration?