Question 1

Which is the strongest acid?

Accepted Answer

A) HBrO4 
B) HBr 
C) HBrO2 
D) HBrO 
E) HBrO3 
A) HBrO4 
B) HBr 
C) HBrO2 
D) HBrO 
E) HBrO3 A

Question 2

Below is a representation of an aqueous solution of a weak acid HA at equilibrium.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are not shown for clarity.)   What is the pH of the solution?

Accepted Answer

A) 2.4 
B) 3.0 
C) 2.1 
D) 11.0 
E) 11.6 
A) 2.4 
B) 3.0 
C) 2.1 
D) 11.0 
E) 11.6 B

Question 3

What is the value of the equilibrium constant for the autoionization of water at 25°C?

Accepted Answer

A) 1.0 × 10-7 
B) 1.0 × 10-14 
C) 1.0 × 1014 
D) 1.0 × 107 
E) 14 
A) 1.0 × 10-7 
B) 1.0 × 10-14 
C) 1.0 × 1014 
D) 1.0 × 107 
E) 14 B

Question 4

After a substance acting as a strong acid reacts,what remains of the acid?

Accepted Answer

A) a weak conjugate base 
B) a strong conjugate base 
C) a strong conjugate acid 
D) a strong acid 
E) a weak conjugate acid 
A) a weak conjugate base 
B) a strong conjugate base 
C) a strong conjugate acid 
D) a strong acid 
E) a weak conjugate acid

Question 5

List the components in an oxoacid.

Accepted Answer

hydrogen,o

Question 6

What is the pH of a 0.056 M HNO3 solution?

Accepted Answer

A) 0.056 
B) 1.25 
C) 12.75 
D) 2.88 
E) 11.11 
A) 0.056 
B) 1.25 
C) 12.75 
D) 2.88 
E) 11.11

Question 7

The pH of a Ba(OH)2 solution is 10.00.What is the H+ ion concentration of this solution?

Accepted Answer

A) 4.0 × 10-11 M 
B) 1.6 × 10-10 M 
C) 1.3 × 10-5 M 
D) 1.0 × 10-10 M 
E) 10.00 M 
A) 4.0 × 10-11 M 
B) 1.6 × 10-10 M 
C) 1.3 × 10-5 M 
D) 1.0 × 10-10 M 
E) 10.00 M

Question 8

Which one of these salts will form an acidic solution upon dissolving in water?

Accepted Answer

A) LiBr 
B) NaF 
C) NH4Br 
D) KOH 
E) NaCN 
A) LiBr 
B) NaF 
C) NH4Br 
D) KOH 
E) NaCN

Question 9

A student adds 0.1 mol of oxalic acid and 0.1 mol of sodium dihydrogen phosphate to enough water to make 1.0 L of solution.The following equilibrium is established with the concentrations of the products greater than the concentrations of the reactants.Which of the statements about the equilibrium system is correct? H2C2O4(aq)+ H2PO4-(aq)   HC2O4-(aq)+ H3PO4(aq)

Accepted Answer

A) Oxalic acid is a weaker acid than phosphoric acid. 
B) The hydrogen oxalate anion,HC2O4-,is a stronger base than the dihydrogen phosphate anion,H2PO4-. 
C) Phosphoric acid is a weaker acid than oxalic acid. 
D) The dihydrogen phosphate anion,H2PO4-,is a stronger acid than oxalic acid. 
E) Water is a stronger acid than either oxalic or phosphoric acids. 
A) Oxalic acid is a weaker acid than phosphoric acid. 
B) The hydrogen oxalate anion,HC2O4-,is a stronger base than the dihydrogen phosphate anion,H2PO4-. 
C) Phosphoric acid is a weaker acid than oxalic acid. 
D) The dihydrogen phosphate anion,H2PO4-,is a stronger acid than oxalic acid. 
E) Water is a stronger acid than either oxalic or phosphoric acids.

Question 10

For H3PO4,Ka1 = 7.3 × 10-3,Ka2 = 6.2 × 10-6,and Ka3 = 4.8 × 10-13.A 0.10 M aqueous solution of NaH2PO4 therefore would be _____.

Accepted Answer

A) neutral 
B) weakly basic 
C) weakly acidic 
D) strongly acidic 
E) strongly basic 
A) neutral 
B) weakly basic 
C) weakly acidic 
D) strongly acidic 
E) strongly basic

Question 11

What is the conjugate acid of CO32- in the reaction below? CO32- + HSO4-
    HCO3- + SO42-

Accepted Answer

A) HCO3- 
B) HSO4- 
C) OH- 
D) H3O+ 
E) SO42- 
A) HCO3- 
B) HSO4- 
C) OH- 
D) H3O+ 
E) SO42-

Question 12

What is the value of Kb for the formate anion,HCOO- ? Ka (HCOOH)= 2.1 × 10-4

Accepted Answer

A) (-2.1 × 10-4) 
B) 2.1 × 10-4 
C) 6.9 × 10-6 
D) 4.8 × 10-11 
E) 2.1 × 10-18 
A) (-2.1 × 10-4) 
B) 2.1 × 10-4 
C) 6.9 × 10-6 
D) 4.8 × 10-11 
E) 2.1 × 10-18

Question 13

The most acidic oxides are formed from elements found in the _________________ region of the periodic table.

Accepted Answer

A) upper right 
B) upper left 
C) center 
D) lower right 
E) lower left 
A) upper right 
B) upper left 
C) center 
D) lower right 
E) lower left

Question 14

What is the name of a proton acceptor in an acid-base reaction?

Accepted Answer

A) Arrhenius acid 
B) Arrhenius base 
C) Brønsted acid 
D) Brønsted base 
E) Lewis base 
A) Arrhenius acid 
B) Arrhenius base 
C) Brønsted acid 
D) Brønsted base 
E) Lewis base

Question 15

A 1.25 M solution of the weak acid HA is 9.2% dissociated.What is the pH of the solution?

Accepted Answer

A) 0.64 
B) 0.94 
C) 1.13 
D) 2.16 
E) (-0.097) 
A) 0.64 
B) 0.94 
C) 1.13 
D) 2.16 
E) (-0.097)

Question 16

What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

Accepted Answer

A) 2.34 × 10-4 M 
B) 2.29 × 10-6 M 
C) 4.37 × 10-9 M 
D) 4.27 × 10-11 M 
E) 8.360 M 
A) 2.34 × 10-4 M 
B) 2.29 × 10-6 M 
C) 4.37 × 10-9 M 
D) 4.27 × 10-11 M 
E) 8.360 M

Question 17

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2-)= 1.5 × 10-10

Accepted Answer

A) 0.38 
B) 12.00 
C) 10.91 
D) 8.09 
E) 13.62 
A) 0.38 
B) 12.00 
C) 10.91 
D) 8.09 
E) 13.62

Question 18

NH3 is a typical Lewis base.

Accepted Answer

A) True 
 B)False

Question 19

What is the conjugate base of water?

Accepted Answer

A) H3O+ 
B) OH- 
C) H3O 
D) OH 
E) H2O2 
A) H3O+ 
B) OH- 
C) H3O 
D) OH 
E) H2O2

Question 20

What is the conjugate base of HSO4- in the reaction below? CO32- + HSO4-   HCO3- + SO42-

Accepted Answer

A) HSO4- 
B) CO32- 
C) OH- 
D) H3O+ 
E) SO42- 
A) HSO4- 
B) CO32- 
C) OH- 
D) H3O+ 
E) SO42-

Exam 16: Acids and Bases

Which is the strongest acid?

Below is a representation of an aqueous solution of a weak acid HA at equilibrium.(Each circle represents 1.0 ×10-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are not shown for clarity.) What is the pH of the solution?

What is the value of the equilibrium constant for the autoionization of water at 25°C?

After a substance acting as a strong acid reacts,what remains of the acid?

List the components in an oxoacid.

What is the pH of a 0.056 M HNO3 solution?

The pH of a Ba(OH)2 solution is 10.00.What is the H+ ion concentration of this solution?

Which one of these salts will form an acidic solution upon dissolving in water?

For H3PO4,Ka1 = 7.3 × 10-3,Ka2 = 6.2 × 10-6,and Ka3 = 4.8 × 10-13.A 0.10 M aqueous solution of NaH2PO4 therefore would be _____.

What is the conjugate acid of CO32- in the reaction below? CO32- + HSO4- HCO3- + SO42-

What is the value of Kb for the formate anion,HCOO- ? Ka (HCOOH)= 2.1 × 10-4

The most acidic oxides are formed from elements found in the _________________ region of the periodic table.

What is the name of a proton acceptor in an acid-base reaction?

A 1.25 M solution of the weak acid HA is 9.2% dissociated.What is the pH of the solution?

What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2-)= 1.5 × 10-10

NH3 is a typical Lewis base.

What is the conjugate base of water?

What is the conjugate base of HSO4- in the reaction below? CO32- + HSO4- HCO3- + SO42-

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

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Below is a representation of an aqueous solution of a weak acid HA at equilibrium.(Each circle represents 1.0 ×10^-3 mol of atoms,and the volume of the box is 1.0 L.Solvent water molecules are not shown for clarity.) What is the pH of the solution?

What is the pH of a 0.056 M HNO₃ solution?

The pH of a Ba(OH)₂ solution is 10.00.What is the H⁺ ion concentration of this solution?

For H₃PO₄,K_a₁ = 7.3 × 10^-³,K_a₂ = 6.2 × 10^-⁶,and Ka₃ = 4.8 × 10^-¹³.A 0.10 M aqueous solution of NaH₂PO₄ therefore would be _____.

What is the conjugate acid of CO₃^2- in the reaction below? CO₃^2- + HSO₄^- HCO₃^- + SO₄^2-

What is the value of K_b for the formate anion,HCOO^- ? K_a (HCOOH)= 2.1 × 10^-⁴

What is the [H₃O⁺] for a solution at 25°C that has pOH = 5.640?

What is the pH of a 0.0100 M sodium benzoate solution? K_b (C₇H₅O₂^-)= 1.5 × 10^-¹⁰

NH₃ is a typical Lewis base.

What is the conjugate base of HSO₄^- in the reaction below? CO₃^2- + HSO₄^- HCO₃^- + SO₄^2-