Question 1

Which of the following statements is true concerning the titration of a weak monoprotic acid with a strong base?

Accepted Answer

A) At the equivalence point,the solution has excess moles of strong base. 
B) At the equivalence point,the solution is acidic. 
C) At the equivalence point,the solution has excess moles of weak acid. 
D) At the equivalence point,the solution is composed of the conjugate base of the weak acid. 
E) At the equivalence point,the pH is 7. 
A) At the equivalence point,the solution has excess moles of strong base. 
B) At the equivalence point,the solution is acidic. 
C) At the equivalence point,the solution has excess moles of weak acid. 
D) At the equivalence point,the solution is composed of the conjugate base of the weak acid. 
E) At the equivalence point,the pH is 7.

Question 2

What is the hydroxide-ion concentration at equilibrium in a 0.66 M solution of ethylamine (C2H5NH2,Kb = 4.7 × 10-4)at 25oC?

Accepted Answer

A) 1.7 × 10-2 M 
B) 2.7 × 10-2 M 
C) 1.5 × 10-14 M 
D) 5.8 × 10-13 M 
E) 6.6 × 10-1 M 
A) 1.7 × 10-2 M 
B) 2.7 × 10-2 M 
C) 1.5 × 10-14 M 
D) 5.8 × 10-13 M 
E) 6.6 × 10-1 M

Question 3

For a 0.05 M H2SO3 solution,which of the following relationships is true?

Accepted Answer

A) [SO32-] > [H2SO3] 
B) [SO32-] > [HSO3-] 
C) [HSO3-] > [H2SO3] 
D) [H2SO3] > [H+] 
E) [H+] > [H2SO3] 
A) [SO32-] > [H2SO3] 
B) [SO32-] > [HSO3-] 
C) [HSO3-] > [H2SO3] 
D) [H2SO3] > [H+] 
E) [H+] > [H2SO3]

Question 4

What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid valeric acid,HC5H9O2,at 25°C (Ka =   )?

Accepted Answer

A) 0.67% 
B) 1.30% 
C) 0.0014% 
D) 0.1% 
E) 2.00% 
A) 0.67% 
B) 1.30% 
C) 0.0014% 
D) 0.1% 
E) 2.00%

Question 5

What mass of sodium hydroxide must be added to 60.0 mL of 0.978 M acetic acid in order to create a buffer with a pH of 4.59? Ka for acetic acid is 1.8 × 10-5.

Accepted Answer

A) 28 g 
B) 0.96 g 
C) 1 g 
D) 0 g 
E) 2.3 g 
A) 28 g 
B) 0.96 g 
C) 1 g 
D) 0 g 
E) 2.3 g

Question 6

Given the following,what will be the approximate equilibrium pH of an aqueous solution of ammonium acetate,NH4CH3CO2?
NH4+
Ka = 5.69 x10-10
CH3CO2-
Kb = 5.71 x10-10

Accepted Answer

A) very basic 
B) very acidic 
C) nearly neutral 
A) very basic 
B) very acidic 
C) nearly neutral

Question 7

What is the equilibrium expression for the equilibrium A-(aq)+ H3O+(aq)   HA(aq)+ H2O(l)?

Accepted Answer

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

Question 8

Rank acetic acid (HC2H3O2),hydrocyanic acid (HOCN),and hydrofluoric acid (HF)in order of increasing strength.
Acid
Ka
HC2H3O2
1)8 × 10-5
HOCN
3)5 × 10-4
HF
6)8 × 10-4

Accepted Answer

A) HC2H3O2 2H3O2 2H3O2 
D) HF 2H3O2 
E) HF 2H3O2 < HOCN 
A) HC2H3O2 2H3O2 2H3O2 
D) HF 2H3O2 
E) HF 2H3O2 < HOCN

Which of the following statements is true concerning the titration of a weak monoprotic acid with a strong base?

What is the hydroxide-ion concentration at equilibrium in a 0.66 M solution of ethylamine (C₂H₅NH₂,K_b = 4.7 × 10^-4)at 25^oC?

For a 0.05 M H₂SO₃ solution,which of the following relationships is true?

What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid valeric acid,HC₅H₉O₂,at 25°C (K_a = )?

What mass of sodium hydroxide must be added to 60.0 mL of 0.978 M acetic acid in order to create a buffer with a pH of 4.59? K_a for acetic acid is 1.8 × 10^-5.

Given the following,what will be the approximate equilibrium pH of an aqueous solution of ammonium acetate,NH₄CH₃CO₂? NH₄⁺ K_a = 5.69 x10^-10 CH₃CO₂^- K_b = 5.71 x10^-10

What is the equilibrium expression for the equilibrium A^-(aq)+ H₃O⁺(aq) HA(aq)+ H₂O(l)?

Rank acetic acid (HC₂H₃O₂),hydrocyanic acid (HOCN),and hydrofluoric acid (HF)in order of increasing strength. Acid K_a HC₂H₃O₂ 1)8 × 10^-5 HOCN 3)5 × 10^-4 HF 6)8 × 10^-4

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Exam 16: Acid-Base Equilibria

Which of the following statements is true concerning the titration of a weak monoprotic acid with a strong base?

What is the hydroxide-ion concentration at equilibrium in a 0.66 M solution of ethylamine (C2H5NH2,Kb = 4.7 × 10-4)at 25oC?

For a 0.05 M H2SO3 solution,which of the following relationships is true?

What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid valeric acid,HC5H9O2,at 25°C (Ka = )?

What mass of sodium hydroxide must be added to 60.0 mL of 0.978 M acetic acid in order to create a buffer with a pH of 4.59? Ka for acetic acid is 1.8 × 10-5.

Given the following,what will be the approximate equilibrium pH of an aqueous solution of ammonium acetate,NH4CH3CO2? NH4+ Ka = 5.69 x10-10 CH3CO2- Kb = 5.71 x10-10

What is the equilibrium expression for the equilibrium A-(aq)+ H3O+(aq) HA(aq)+ H2O(l)?

Rank acetic acid (HC2H3O2),hydrocyanic acid (HOCN),and hydrofluoric acid (HF)in order of increasing strength. Acid Ka HC2H3O2 1)8 × 10-5 HOCN 3)5 × 10-4 HF 6)8 × 10-4

Chemistry and Measurement

Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

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Thermochemistry

Quantum Theory of the Atom

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Molecular Geometry and Chemical Bonding Theory

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Solutions

Rates of Reaction

Chemical Equilibrium

Acids and Bases

Solubility and Complex-Ion Equilibria

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Polymer Materials: Synthetic and Biological

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What is the hydroxide-ion concentration at equilibrium in a 0.66 M solution of ethylamine (C₂H₅NH₂,K_b = 4.7 × 10^-4)at 25^oC?

For a 0.05 M H₂SO₃ solution,which of the following relationships is true?

What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid valeric acid,HC₅H₉O₂,at 25°C (K_a = )?

What mass of sodium hydroxide must be added to 60.0 mL of 0.978 M acetic acid in order to create a buffer with a pH of 4.59? K_a for acetic acid is 1.8 × 10^-5.

Given the following,what will be the approximate equilibrium pH of an aqueous solution of ammonium acetate,NH₄CH₃CO₂? NH₄⁺ K_a = 5.69 x10^-10 CH₃CO₂^- K_b = 5.71 x10^-10

What is the equilibrium expression for the equilibrium A^-(aq)+ H₃O⁺(aq) HA(aq)+ H₂O(l)?

Rank acetic acid (HC₂H₃O₂),hydrocyanic acid (HOCN),and hydrofluoric acid (HF)in order of increasing strength. Acid K_a HC₂H₃O₂ 1)8 × 10^-5 HOCN 3)5 × 10^-4 HF 6)8 × 10^-4