Question 1

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 M hydronium ion.

Accepted Answer

A) 4)65 × 10-12 
B) 2)15 × 10-3 
C) 2)67 
D) 11.33 
A) 4)65 × 10-12 
B) 2)15 × 10-3 
C) 2)67 
D) 11.33

Question 2

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-4 M?

Accepted Answer

A) 6)67 × 10-10 M,4.82 
B) 6)67 × 10-10 M,9.18 
C) 6)67 × 10-11 M,3.82 
D) 6)67 × 10-11 M,10.18 
A) 6)67 × 10-10 M,4.82 
B) 6)67 × 10-10 M,9.18 
C) 6)67 × 10-11 M,3.82 
D) 6)67 × 10-11 M,10.18

Question 3

The concentration of H3O+ in human sweat can be as low as 2.5 × 10-6.The concentration of OH- in the sweat is ________,and this solution is ________ (acidic,basic,neutral).

Accepted Answer

Question 4

Identify the Lewis acid that acts as a reactant in the following reaction.
Fe(H2O)63+(aq)+ 6 CN-(aq)→ Fe(CN)63-(aq)+ 6 H2O(l)

Accepted Answer

A) Fe3+ 
B) H2O 
C) CN- 
D) Fe(H2O)63+ 
A) Fe3+ 
B) H2O 
C) CN- 
D) Fe(H2O)63+

Question 5

What are the Br∅nsted-Lowry acids in the following chemical reaction?
HBr(sol)+ CH3COOH(sol)⇌ CH3C(OH)2+(sol)+ Br-(sol)

Accepted Answer

A) HBr,CH3COOH 
B) HBr,CH3C(OH)2+ 
C) CH3COOH,CH3C(OH)2+ 
D) CH3COOH,Br- 
A) HBr,CH3COOH 
B) HBr,CH3C(OH)2+ 
C) CH3COOH,CH3C(OH)2+ 
D) CH3COOH,Br-

Question 6

The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity.  
-Arrange the acids in order of increasing pH.

Accepted Answer

A) HZ < HY < HX 
B) HY < HZ < HX 
C) HZ < HX < HY 
D) HX < HZ < HY 
A) HZ < HY < HX 
B) HY < HZ < HX 
C) HZ < HX < HY 
D) HX < HZ < HY

Question 7

The acid strength of an oxoacid having the general formula HnYOm increases as the electronegativity of Y ________ and as the oxidation number of Y ________.

Accepted Answer

Question 8

What is the pH of a 0.020 M HClO4 solution?

Accepted Answer

A) 0)020 
B) 0)040 
C) 1)70 
D) 12.30 
A) 0)020 
B) 0)040 
C) 1)70 
D) 12.30

Question 9

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity.  
-Arrange the three acids in order of increasing acid strength.

Accepted Answer

A) HZ < HY < HX 
B) HY < HZ < HX 
C) HZ < HX < HY 
D) HX < HZ < HY 
A) HZ < HY < HX 
B) HY < HZ < HX 
C) HZ < HX < HY 
D) HX < HZ < HY

Question 10

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.0 10 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 6)6 × 10- 5 M 
B) 4)3 × 10-7 M 
C) 4)3 × 10- 9 M 
D) 5)6 × 10-11 M 
A) 6)6 × 10- 5 M 
B) 4)3 × 10-7 M 
C) 4)3 × 10- 9 M 
D) 5)6 × 10-11 M

Question 11

What is the pH of a solution prepared by diluting 100.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?

Accepted Answer

A) 1)80 
B) 2)10 
C) 11.90 
D) 12.20 
A) 1)80 
B) 2)10 
C) 11.90 
D) 12.20

Question 12

What is the equilibrium constant expression (Ka)for the acid dissociation of hydrocyanic acid HCN? The equation of interest is
HCN(aq)+ H2O(l)⇌ H3O+(aq)+ CN-(aq).

Accepted Answer

A) Ka = ([H3O+][CN-])/([HCN][H2O]) 
B) Ka = ([H3O+][CN-])/([HCN]) 
C) Ka = ([HCN][H2O])/([H3O+][CN-]) 
D) Ka = ([HCN])/([H3O+][CN-]) 
A) Ka = ([H3O+][CN-])/([HCN][H2O]) 
B) Ka = ([H3O+][CN-])/([HCN]) 
C) Ka = ([HCN][H2O])/([H3O+][CN-]) 
D) Ka = ([HCN])/([H3O+][CN-])

Question 13

What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the lowest pH?

Accepted Answer

A) Li+ 
B) Na+ 
C) Mg2+ 
D) Al3+ 
A) Li+ 
B) Na+ 
C) Mg2+ 
D) Al3+

Question 14

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Accepted Answer

A) 2)55 
B) 4)25 
C) 9)75 
D) 11.45 
A) 2)55 
B) 4)25 
C) 9)75 
D) 11.45

Question 15

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH3 (Kb = 1.8 × 10-5)is
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq).

Accepted Answer

A) 3)0 M 
B) 0)056 M 
C) 1)8 × 10- 2 M 
D) 1)0 × 10-3 M 
A) 3)0 M 
B) 0)056 M 
C) 1)8 × 10- 2 M 
D) 1)0 × 10-3 M

Question 16

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.15?

Accepted Answer

A) 1)41 × 10-11 M 
B) 7)08 × 10-4 M 
C) 3)15 M 
D) 10.85 M 
A) 1)41 × 10-11 M 
B) 7)08 × 10-4 M 
C) 3)15 M 
D) 10.85 M

Question 17

When dissolved in water,which of the following compounds is an Arrhenius base?

Accepted Answer

A) CH3OH 
B) HOCl 
C) KOH 
D) KCl 
A) CH3OH 
B) HOCl 
C) KOH 
D) KCl

Question 18

The pH of 0.150 M CH3CO2H,acetic acid,is 2.78.What is the value of Ka for acetic acid?

Accepted Answer

A) 2)8 × 10-6 
B) 1)9 × 10-5 
C) 1)7 × 10-3 
D) 1)1 × 10-2 
A) 2)8 × 10-6 
B) 1)9 × 10-5 
C) 1)7 × 10-3 
D) 1)1 × 10-2

Question 19

The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity.  
-Arrange the conjugate bases (A- = X-,Y-,or Z-)in order of increasing value of Kb.

Accepted Answer

A) Kb(Z-)b(Y-)b(X-) 
B) Kb(Y-)b(Z-)b(X-) 
C) Kb(Z-)b(X-)b(Y-) 
D) Kb(X-)b(Z-)b(Y-) 
A) Kb(Z-)b(Y-)b(X-) 
B) Kb(Y-)b(Z-)b(X-) 
C) Kb(Z-)b(X-)b(Y-) 
D) Kb(X-)b(Z-)b(Y-)

Question 20

Calculate the pH of a 0.20 M H2SO3 solution that has the stepwise dissociation constants
Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.

Accepted Answer

A) 1)26 
B) 1)32 
C) 1)82 
D) 2)52 
A) 1)26 
B) 1)32 
C) 1)82 
D) 2)52

Exam 14: Aqueous Equilibria: Acids and Bases

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 M hydronium ion.

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-4 M?

The concentration of H3O+ in human sweat can be as low as 2.5 × 10-6.The concentration of OH- in the sweat is ________,and this solution is ________ (acidic,basic,neutral).

Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H2O)63+(aq)+ 6 CN-(aq)→ Fe(CN)63-(aq)+ 6 H2O(l)

What are the Br∅nsted-Lowry acids in the following chemical reaction? HBr(sol)+ CH3COOH(sol)⇌ CH3C(OH)2+(sol)+ Br-(sol)

The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. -Arrange the acids in order of increasing pH.

The acid strength of an oxoacid having the general formula HnYOm increases as the electronegativity of Y ________ and as the oxidation number of Y ________.

What is the pH of a 0.020 M HClO4 solution?

The following pictures represent aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. -Arrange the three acids in order of increasing acid strength.

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.0 10 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

What is the pH of a solution prepared by diluting 100.00 mL of 0.020 M Ba(OH)2 with enough water to produce a total volume of 250.00 mL?

What is the equilibrium constant expression (Ka)for the acid dissociation of hydrocyanic acid HCN? The equation of interest is HCN(aq)+ H2O(l)⇌ H3O+(aq)+ CN-(aq).

What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the lowest pH?

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH3 (Kb = 1.8 × 10-5)is NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq).

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.15?

When dissolved in water,which of the following compounds is an Arrhenius base?

The pH of 0.150 M CH3CO2H,acetic acid,is 2.78.What is the value of Ka for acetic acid?

The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. -Arrange the conjugate bases (A- = X-,Y-,or Z-)in order of increasing value of Kb.

Calculate the pH of a 0.20 M H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Solutions and Their Properties

Chemical Kinetics

Chemical Equilibrium

Applications of Aqueous Equilibria

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

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Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10^-3 M hydronium ion.

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10^-4 M?

The concentration of H₃O⁺ in human sweat can be as low as 2.5 × 10^-6.The concentration of OH^- in the sweat is ,and this solution is (acidic,basic,neutral).

Identify the Lewis acid that acts as a reactant in the following reaction. Fe(H₂O)₆³⁺(aq)+ 6 CN^-(aq)→ Fe(CN)₆^3-(aq)+ 6 H₂O(l)

What are the Br∅nsted-Lowry acids in the following chemical reaction? HBr(sol)+ CH₃COOH(sol)⇌ CH₃C(OH)₂⁺(sol)+ Br^-(sol)

The acid strength of an oxoacid having the general formula H_nYO_m increases as the electronegativity of Y and as the oxidation number of Y .

What is the pH of a 0.020 M HClO₄ solution?

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.0 10 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the pH of a solution prepared by diluting 100.00 mL of 0.020 M Ba(OH)₂ with enough water to produce a total volume of 250.00 mL?

What is the equilibrium constant expression (K_a)for the acid dissociation of hydrocyanic acid HCN? The equation of interest is HCN(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CN^-(aq).

What is the identity of M in the hydrate M(H₂O)₆ⁿ⁺ that has the 0.10 M solution with the lowest pH?

Calculate the pH of a 1.60 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-9.

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH₃ (K_b= 1.8 × 10^-5)is NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq).

The pH of 0.150 M CH₃CO₂H,acetic acid,is 2.78.What is the value of K_a for acetic acid?

The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X,Y,or Z);water molecules have been omitted for clarity. -Arrange the conjugate bases (A^- = X^-,Y^-,or Z^-)in order of increasing value of K_b.

Calculate the pH of a 0.20 M H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and K_a2 = 6.3 × 10^-8.