Question 1

Which of the following pairs of species is not a conjugate acid-base pair?

Accepted Answer

A)  HOCl and OCl- 
B)  HNO2 and NO2+ 
C)  O2- and OH- 
D)  HSO4- and SO42- 
E)  H2CO3 and HCO3- 
A)  HOCl and OCl- 
B)  HNO2 and NO2+ 
C)  O2- and OH- 
D)  HSO4- and SO42- 
E)  H2CO3 and HCO3- B

Question 2

Which of the following substances is never a Brønsted-Lowry acid in an aqueous solution?

Accepted Answer

A)  sodium dihydrogen phosphate,NaH2PO4(s) 
B)  sodium acetate,NaCH3CO2(s) 
C)  ammonium nitrate,NH4NO3(s) 
D)  hydrogen bromide,HCl(g) 
E)  sodium bicarbonate,NaHCO3(s) 
A)  sodium dihydrogen phosphate,NaH2PO4(s) 
B)  sodium acetate,NaCH3CO2(s) 
C)  ammonium nitrate,NH4NO3(s) 
D)  hydrogen bromide,HCl(g) 
E)  sodium bicarbonate,NaHCO3(s) B

Question 3

Calculate the pH of a 0.09 M solution of ascorbic acid (Ka1 = 7.9 × 10-5; Ka2 is 1.6 × 10-12).

Accepted Answer

A)  11.4 
B)  2.6 
C)  5.1 
D)  8.9 
E)  11.8 
A)  11.4 
B)  2.6 
C)  5.1 
D)  8.9 
E)  11.8 B

Question 4

Which is the stronger Brønsted-Lowry acid,Fe(H2O)62+ or Fe(H2O)63+? Explain.

Accepted Answer

Fe(H₂O)₆³⁺.When a proton dissociates from th

Question 5

Which of the following species is amphiprotic in aqueous solution?

Accepted Answer

A)  CHNH3+ 
B)  H3O+ 
C)  HF 
D)  OCl− 
E)  H2PO4- 
A)  CHNH3+ 
B)  H3O+ 
C)  HF 
D)  OCl− 
E)  H2PO4-

Question 6

Which equation depicts the hydrogen phosphate ion behaving as a Brønsted-Lowry base in water?

Accepted Answer

A)  HPO42-(aq)+ H2O(   )   H2PO4-(aq)+ OH-(aq) 
B)  HPO42-(aq)+ OH-(aq)   PO43-(aq)+ H2O(   ) 
C)  HPO42-(aq)+ H2O(   )   PO43-(aq)+ H3O+(aq) 
D)  2 HPO42-(aq)+ O2-(aq)   PO43-(aq)+ H2O(   ) 
E)  2 HPO42-(aq)+ H2O(   )   2 H2O(   )+ P2O7(s) 
A)  HPO42-(aq)+ H2O(   )   H2PO4-(aq)+ OH-(aq) 
B)  HPO42-(aq)+ OH-(aq)   PO43-(aq)+ H2O(   ) 
C)  HPO42-(aq)+ H2O(   )   PO43-(aq)+ H3O+(aq) 
D)  2 HPO42-(aq)+ O2-(aq)   PO43-(aq)+ H2O(   ) 
E)  2 HPO42-(aq)+ H2O(   )   2 H2O(   )+ P2O7(s)

Question 7

What is the pOH of 0.074 M HI(aq)at 25 °C? (Kw = 1.01 × 10-14)?

Accepted Answer

A)  2.60 
B)  12.87 
C)  11.40 
D)  15.13 
E)  1.13 
A)  2.60 
B)  12.87 
C)  11.40 
D)  15.13 
E)  1.13

Question 8

What is the pH of a solution prepared by dissolving 0.459 L of HCl(g),measured at STP,in enough water such that the total volume of the solution is 5.50 L? (R = 0.0821 L · atm/K·mol)

Accepted Answer

A)  2.429 
B)  11.571 
C)  1.689 
D)  7.000 
E)  12.311 
A)  2.429 
B)  11.571 
C)  1.689 
D)  7.000 
E)  12.311

Question 9

What is the conjugate base of HPO43- in aqueous solution?

Accepted Answer

A)  not possible 
B)  PO43- 
C)  HPO42− 
D)  H2PO4− 
E)  H3PO4 
A)  not possible 
B)  PO43- 
C)  HPO42− 
D)  H2PO4− 
E)  H3PO4

Question 10

What is the equilibrium constant for the following reaction, HCO2H(aq)+ CN-(aq)   HCO2-(aq)+ HCN(aq)
And does the reaction favor the formation of reactants or products? The acid dissociation constant,Ka,for HCO2H is 1.8 × 10-4 and the acid dissociation constant for HCN is 4.0 × 10-10.

Accepted Answer

A)  K = 1.00.The reaction favors neither the formation of reactants nor products. 
B)  K = 2.2 × 10-6.The reaction favors the formation of products. 
C)  K = 2.2 × 10-6.The reaction favors the formation of reactants. 
D)  K = 4.5 × 105.The reaction favors the formation of products. 
E)  K = 4.5 × 105.The reaction favors the formation of reactants. 
A)  K = 1.00.The reaction favors neither the formation of reactants nor products. 
B)  K = 2.2 × 10-6.The reaction favors the formation of products. 
C)  K = 2.2 × 10-6.The reaction favors the formation of reactants. 
D)  K = 4.5 × 105.The reaction favors the formation of products. 
E)  K = 4.5 × 105.The reaction favors the formation of reactants.

Question 11

Which of the following ionic compounds forms a neutral aqueous solution at 25 °C?

Accepted Answer

A)  NaHSO3 
B)  LiClO3 
C)  KOCl 
D)  NH4F 
E)  Li2S 
A)  NaHSO3 
B)  LiClO3 
C)  KOCl 
D)  NH4F 
E)  Li2S

Question 12

Which of the following is the strongest acid in aqueous solution?

Accepted Answer

A)  H3AsO4 
B)  H3PO4 
C)  H3PO3 
D)  H3SbO4 
E)  H3AsO3 
A)  H3AsO4 
B)  H3PO4 
C)  H3PO3 
D)  H3SbO4 
E)  H3AsO3

Question 13

Which of the following statements is INCORRECT?

Accepted Answer

A)  H3PO4 is a stronger acid than H2PO4−. 
B)  HClO3 is a stronger acid than HClO2. 
C)  HNO3 is a stronger acid than HNO2. 
D)  [Fe(H2O)6]2+ is a stronger acid than [Fe(H2O)6]3+. 
E)  HOCl is stronger acid than HOBr. 
A)  H3PO4 is a stronger acid than H2PO4−. 
B)  HClO3 is a stronger acid than HClO2. 
C)  HNO3 is a stronger acid than HNO2. 
D)  [Fe(H2O)6]2+ is a stronger acid than [Fe(H2O)6]3+. 
E)  HOCl is stronger acid than HOBr.

Question 14

Which acid-base reaction results in acidic solution?

Accepted Answer

A)  HBr(aq)+ KOH(aq)→ H2O(   )+ KBr(aq) 
B)  HNO3(aq)+ LiOH(aq)→ H2O(   )+ LiNO3(aq) 
C)  HCl(aq)+ KOH(aq)→ H2O(   )+ KCl(aq) 
D)  H2SO4(aq)+ CsOH(aq)   H2O(   )+ CsHSO4(aq) 
E)  HF(aq)+ RbOH(aq)   H2O(   )+ RbF(aq) 
A)  HBr(aq)+ KOH(aq)→ H2O(   )+ KBr(aq) 
B)  HNO3(aq)+ LiOH(aq)→ H2O(   )+ LiNO3(aq) 
C)  HCl(aq)+ KOH(aq)→ H2O(   )+ KCl(aq) 
D)  H2SO4(aq)+ CsOH(aq)   H2O(   )+ CsHSO4(aq) 
E)  HF(aq)+ RbOH(aq)   H2O(   )+ RbF(aq)

Question 15

What is the equilibrium pH of a 0.700 M solution of H3PO4(aq)? (Ka1 = 7.5 × 10-3,Ka2 = 6.2 × 10-8,Ka3 = 4.8 × 10-13)

Accepted Answer

A)  1.16 
B)  3.68 
C)  12.32 
D)  6.24 
E)  7.21 
A)  1.16 
B)  3.68 
C)  12.32 
D)  6.24 
E)  7.21

Question 16

Calculate the pH of the following aqueous solution: 0.17 M H2S (pKa1 = 7.00; pKa2 = 12.89)

Accepted Answer

A)  10.12 
B)  6.23 
C)  3.88 
D)  7.77 
E)  7.00 
A)  10.12 
B)  6.23 
C)  3.88 
D)  7.77 
E)  7.00

Question 17

The H3O+ concentration of a solution is 5.9 × 10-6 M.What is the pH of the solution?

Accepted Answer

A)  6.44 
B)  3.40 
C)  2.00 
D)  5.23 
E)  9.74 
A)  6.44 
B)  3.40 
C)  2.00 
D)  5.23 
E)  9.74

Question 18

Which equation depicts aqueous hydrogen sulfide behaving as a Brønsted-Lowry base in water?

Accepted Answer

A)  H2S(aq)+ 2 OH-(aq)   SO2(aq)+ 2 H2(g) 
B)  H2S(aq)+ H3O+(aq)   H3S+(aq)+ H2O(   ) 
C)  H2S(aq)+ H2O(   )   HS-(aq)+ H3O+(aq) 
D)  HS-(aq)+ H3O+(aq)   H2S(aq)+ H2O(   ) 
E)  H2S(aq)+ H2O(   )   H3S++(aq)+ OH-(aq) 
A)  H2S(aq)+ 2 OH-(aq)   SO2(aq)+ 2 H2(g) 
B)  H2S(aq)+ H3O+(aq)   H3S+(aq)+ H2O(   ) 
C)  H2S(aq)+ H2O(   )   HS-(aq)+ H3O+(aq) 
D)  HS-(aq)+ H3O+(aq)   H2S(aq)+ H2O(   ) 
E)  H2S(aq)+ H2O(   )   H3S++(aq)+ OH-(aq)

Question 19

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO3 in order to change the pH to 4.0?

Accepted Answer

A)  14.4 mL 
B)  143 mL 
C)  1.43 × 103 mL 
D)  36 mL 
E)  86 mL 
A)  14.4 mL 
B)  143 mL 
C)  1.43 × 103 mL 
D)  36 mL 
E)  86 mL

Question 20

Which of the following equations shows that isoquinoline,C9H7N,behaves as a Brønsted-Lowry base in water?

Accepted Answer

A)  C9H7N(aq)+ H2O(l)   C9H7NH+(aq)+ OH−(aq) 
B)  C9H7N(aq)+ H2O(l)   C9H6N-(aq)+ H3O+(aq) 
C)  C9H7N(aq)+ OH−(aq)   C9H6N−(aq)+ H2O(l) 
D)  C9H7N(aq)+ H3O+(aq)   C9H7NH+(aq)+ H2O(l) 
E)  C9H7NH+(aq)+ H2O(l)   C9H7N(aq)+ H3O+(aq) 
A)  C9H7N(aq)+ H2O(l)   C9H7NH+(aq)+ OH−(aq) 
B)  C9H7N(aq)+ H2O(l)   C9H6N-(aq)+ H3O+(aq) 
C)  C9H7N(aq)+ OH−(aq)   C9H6N−(aq)+ H2O(l) 
D)  C9H7N(aq)+ H3O+(aq)   C9H7NH+(aq)+ H2O(l) 
E)  C9H7NH+(aq)+ H2O(l)   C9H7N(aq)+ H3O+(aq)

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Which of the following pairs of species is not a conjugate acid-base pair?

Which of the following substances is never a Brønsted-Lowry acid in an aqueous solution?

Calculate the pH of a 0.09 M solution of ascorbic acid (Ka1 = 7.9 × 10-5; Ka2 is 1.6 × 10-12).

Which is the stronger Brønsted-Lowry acid,Fe(H2O)62+ or Fe(H2O)63+? Explain.

Which of the following species is amphiprotic in aqueous solution?

Which equation depicts the hydrogen phosphate ion behaving as a Brønsted-Lowry base in water?

What is the pOH of 0.074 M HI(aq)at 25 °C? (Kw = 1.01 × 10-14)?

What is the pH of a solution prepared by dissolving 0.459 L of HCl(g),measured at STP,in enough water such that the total volume of the solution is 5.50 L? (R = 0.0821 L · atm/K·mol)

What is the conjugate base of HPO43- in aqueous solution?

What is the equilibrium constant for the following reaction, HCO2H(aq)+ CN-(aq) HCO2-(aq)+ HCN(aq) And does the reaction favor the formation of reactants or products? The acid dissociation constant,Ka,for HCO2H is 1.8 × 10-4 and the acid dissociation constant for HCN is 4.0 × 10-10.

Which of the following ionic compounds forms a neutral aqueous solution at 25 °C?

Which of the following is the strongest acid in aqueous solution?

Which of the following statements is INCORRECT?

Which acid-base reaction results in acidic solution?

What is the equilibrium pH of a 0.700 M solution of H3PO4(aq)? (Ka1 = 7.5 × 10-3,Ka2 = 6.2 × 10-8,Ka3 = 4.8 × 10-13)

Calculate the pH of the following aqueous solution: 0.17 M H2S (pKa1 = 7.00; pKa2 = 12.89)

The H3O+ concentration of a solution is 5.9 × 10-6 M.What is the pH of the solution?

Which equation depicts aqueous hydrogen sulfide behaving as a Brønsted-Lowry base in water?

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO3 in order to change the pH to 4.0?

Which of the following equations shows that isoquinoline,C9H7N,behaves as a Brønsted-Lowry base in water?

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Calculate the pH of a 0.09 M solution of ascorbic acid (K_a1= 7.9 × 10^-5; K_a2 is 1.6 × 10^-12).

Which is the stronger Brønsted-Lowry acid,Fe(H₂O)₆²⁺ or Fe(H₂O)₆³⁺? Explain.

What is the pOH of 0.074 M HI(aq)at 25 °C? (K_w = 1.01 × 10^-14)?

What is the conjugate base of HPO₄^3- in aqueous solution?

What is the equilibrium constant for the following reaction, HCO₂H(aq)+ CN^-(aq) HCO₂^-(aq)+ HCN(aq) And does the reaction favor the formation of reactants or products? The acid dissociation constant,K_a,for HCO₂H is 1.8 × 10^-4 and the acid dissociation constant for HCN is 4.0 × 10^-10.

What is the equilibrium pH of a 0.700 M solution of H₃PO₄(aq)? (K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,K_a3 = 4.8 × 10^-13)

Calculate the pH of the following aqueous solution: 0.17 M H₂S (pK_a1 = 7.00; pK_a2 = 12.89)

The H₃O⁺ concentration of a solution is 5.9 × 10^-6 M.What is the pH of the solution?

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO₃ in order to change the pH to 4.0?

Which of the following equations shows that isoquinoline,C₉H₇N,behaves as a Brønsted-Lowry base in water?