Question 1

Which of the following bases is the weakest? The base is followed by its Kb value.

Accepted Answer

A) HOCH2CH2NH2,3.2 × 10-5 
B) NH3,1.76 × 10-5 
C) C5H5N,1.7 × 10-9 
D) (CH3CH2)3N,5.2 × 10-4 
E) CH3CH2NH2,5.6 × 10-4 
A) HOCH2CH2NH2,3.2 × 10-5 
B) NH3,1.76 × 10-5 
C) C5H5N,1.7 × 10-9 
D) (CH3CH2)3N,5.2 × 10-4 
E) CH3CH2NH2,5.6 × 10-4

Question 2

What does the term amphoteric mean?

Accepted Answer

A substance is ampho

Question 3

Calculate the pH of a solution that contains 2.4 × 10-5 mol L-1 H3O+ at 25 °C.

Accepted Answer

A) 2.40 
B) 9.38 
C) 4.62 
D) 11.60 
E) 4.17 
A) 2.40 
B) 9.38 
C) 4.62 
D) 11.60 
E) 4.17

Question 4

Which of the following is a general property of a base?

Accepted Answer

A) Bases have sour taste. 
B) Bases turn blue litmus paper red. 
C) Bases leave red litmus paper unchanged. 
D) Bases turn red litmus paper blue. 
E) Bases easily dissolve many metallic elements. 
A) Bases have sour taste. 
B) Bases turn blue litmus paper red. 
C) Bases leave red litmus paper unchanged. 
D) Bases turn red litmus paper blue. 
E) Bases easily dissolve many metallic elements.

Question 5

Identify the monoprotic acid.

Accepted Answer

A) H2CO3 
B) NH3 
C) H3PO4 
D) H2SO4 
E) HBr 
A) H2CO3 
B) NH3 
C) H3PO4 
D) H2SO4 
E) HBr

Question 6

Order the following acids in order of increasing strength: 
$\quad$HBrO $\quad$HBrO3 $\quad$HBrO4$\quad$HBrO2

Accepted Answer

A) HBrO 3 HBrO4 2 
B) HBrO4 3 HBrO2 3 HBrO2 4 
D) HBrO 2 HBrO3 4 
E) HBrO2 4 HBrO 2 
A) HBrO 3 HBrO4 2 
B) HBrO4 3 HBrO2 3 HBrO2 4 
D) HBrO 2 HBrO3 4 
E) HBrO2 4 HBrO 2

Question 7

Determine the concentration of CO32- ions in a 0.18 mol L-1 H2CO3 solution.Carbonic acid is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 2.8 × 10-4 mol L-1 
B) 3.2 × 10-6 mol L-1 
C) 5.6 × 10-11 mol L-1 
D) 4.3 × 10-7 mol L-1 
E) 6.9 × 10-8 mol L-1 
A) 2.8 × 10-4 mol L-1 
B) 3.2 × 10-6 mol L-1 
C) 5.6 × 10-11 mol L-1 
D) 4.3 × 10-7 mol L-1 
E) 6.9 × 10-8 mol L-1

Question 8

An aqueous solution at 25.0 °C contains [ $ \mathrm{H}^{+} $ ] = 0.085 mol L-1.What is the pH of the solution?

Accepted Answer

A) 1.07 
B) -1.07 
C) 13.0 
D) 0.0850 
E) 1.20 × $ 10^{-13} $ 
A) 1.07 
B) -1.07 
C) 13.0 
D) 0.0850 
E) 1.20 × $ 10^{-13} $

Question 9

Determine the Ka of an acid whose 0.294 mol L-1 solution has a pH of 2.80.

Accepted Answer

A) 1.2 × 10-5 
B) 8.5 × 10-6 
C) 2.7 
D) 4.9 × 10-7 
E) 5.4 × 10-3 
A) 1.2 × 10-5 
B) 8.5 × 10-6 
C) 2.7 
D) 4.9 × 10-7 
E) 5.4 × 10-3

Question 10

Determine the pH of a 0.227 mol L-1 C5H5N solution at 25 °C.The Kb of C5H5N is 1.7 × 10-9.

Accepted Answer

A) 4.59 
B) 9.41 
C) 4.71 
D) 10.14 
E) 9.29 
A) 4.59 
B) 9.41 
C) 4.71 
D) 10.14 
E) 9.29

Question 11

Which one of the following will form an acidic solution in water?

Accepted Answer

A) NH4Cl 
B) NaF 
C) LiI 
D) KNO3 
E) NaCH3COO 
A) NH4Cl 
B) NaF 
C) LiI 
D) KNO3 
E) NaCH3COO

Question 12

A solution with a hydroxide ion concentration of 4.15 × 10-6 mol L-1 is ________ and has a hydrogen ion concentration of ________.

Accepted Answer

A) acidic,2.41 × 10-8 mol L-1 
B) acidic,2.41 × 10-9 mol L-1 
C) basic,2.41 × 10-8 mol L-1 
D) basic,2.41 × 10-9 mol L-1 
A) acidic,2.41 × 10-8 mol L-1 
B) acidic,2.41 × 10-9 mol L-1 
C) basic,2.41 × 10-8 mol L-1 
D) basic,2.41 × 10-9 mol L-1

Question 13

Which of the following acids will have the strongest conjugate base?

Accepted Answer

A) HCl 
B) HClO4 
C) HNO3 
D) HCN 
E) HI 
A) HCl 
B) HClO4 
C) HNO3 
D) HCN 
E) HI

Question 14

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

Accepted Answer

No.Polyprotic acids ionize in stages.A s

Question 15

Determine the pH of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Accepted Answer

A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56 
A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56

Question 16

Which of the following increases the strength of a binary acid,HY?

Accepted Answer

A) decreasing the electron affinity of Y and decreasing the H-Y bond strength 
B) increasing the electron affinity of Y and increasing the H-Y bond strength 
C) increasing the electron affinity of Y and decreasing the H-Y bond strength 
D) decreasing the electron affinity of Y and increasing the H-Y bond strength 
E) none of the above 
A) decreasing the electron affinity of Y and decreasing the H-Y bond strength 
B) increasing the electron affinity of Y and increasing the H-Y bond strength 
C) increasing the electron affinity of Y and decreasing the H-Y bond strength 
D) decreasing the electron affinity of Y and increasing the H-Y bond strength 
E) none of the above

Question 17

A 4.0 × 10-3 mol L-1 aqueous solution of $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ at 25.0 °C has a pH of ________.

Accepted Answer

A) 2.40 
B) 11.60 
C) 8.0 × 10-3 
D) 2.10 
E) 11.90 
A) 2.40 
B) 11.60 
C) 8.0 × 10-3 
D) 2.10 
E) 11.90

Question 18

Calculate the pOH of a solution that contains 3.9 × 10-4 mol L-1 H3O+ at 25 °C.

Accepted Answer

A) 4.59 
B) 3.31 
C) 10.59 
D) 9.14 
E) 0.59 
A) 4.59 
B) 3.31 
C) 10.59 
D) 9.14 
E) 0.59

Question 19

Which of the following is the correct definition of Lewis acids and bases?

Accepted Answer

A) A Lewis acid is an electron acceptor while a Lewis base is an electron donor. 
B) A Lewis acid is an electron pair donor while a Lewis base is an electron pair acceptor. 
C) A Lewis acid is an electron donor while a Lewis base is an electron acceptor. 
D) A Lewis acid is an electron pair acceptor while a Lewis base is a proton donor. 
E) A Lewis acid is an electron pair acceptor while a Lewis base is an electron pair donor. 
A) A Lewis acid is an electron acceptor while a Lewis base is an electron donor. 
B) A Lewis acid is an electron pair donor while a Lewis base is an electron pair acceptor. 
C) A Lewis acid is an electron donor while a Lewis base is an electron acceptor. 
D) A Lewis acid is an electron pair acceptor while a Lewis base is a proton donor. 
E) A Lewis acid is an electron pair acceptor while a Lewis base is an electron pair donor.

Question 20

Identify the strongest acid.

Accepted Answer

A) H2O 
B) H2S 
C) H2Se 
D) H2Te 
E) CaH2 
A) H2O 
B) H2S 
C) H2Se 
D) H2Te 
E) CaH2

Exam 15: Acids and Bases

Which of the following bases is the weakest? The base is followed by its Kb value.

What does the term amphoteric mean?

Calculate the pH of a solution that contains 2.4 × 10-5 mol L-1 H3O+ at 25 °C.

Which of the following is a general property of a base?

Identify the monoprotic acid.

Order the following acids in order of increasing strength: \quad HBrO \quad HBrO3 \quad HBrO4 \quad HBrO2

Determine the concentration of CO32- ions in a 0.18 mol L-1 H2CO3 solution.Carbonic acid is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

An aqueous solution at 25.0 °C contains [ H+ \mathrm{H}^{+} H+ ] = 0.085 mol L-1.What is the pH of the solution?

Determine the Ka of an acid whose 0.294 mol L-1 solution has a pH of 2.80.

Determine the pH of a 0.227 mol L-1 C5H5N solution at 25 °C.The Kb of C5H5N is 1.7 × 10-9.

Which one of the following will form an acidic solution in water?

A solution with a hydroxide ion concentration of 4.15 × 10-6 mol L-1 is ________ and has a hydrogen ion concentration of ________.

Which of the following acids will have the strongest conjugate base?

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

Determine the pH of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Which of the following increases the strength of a binary acid,HY?

A 4.0 × 10-3 mol L-1 aqueous solution of Ca(OH)2\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }Ca(OH)2​ at 25.0 °C has a pH of ________.

Calculate the pOH of a solution that contains 3.9 × 10-4 mol L-1 H3O+ at 25 °C.

Which of the following is the correct definition of Lewis acids and bases?

Identify the strongest acid.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Which of the following bases is the weakest? The base is followed by its K_b value.

Calculate the pH of a solution that contains 2.4 × 10^-5 mol L^-1 H₃O⁺ at 25 °C.

Order the following acids in order of increasing strength: $\quad$ HBrO $\quad$ HBrO₃ $\quad$ HBrO₄ $\quad$ HBrO₂

Determine the concentration of CO₃^2- ions in a 0.18 mol L^-1 H₂CO₃ solution.Carbonic acid is a diprotic acid with K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

An aqueous solution at 25.0 °C contains [ $\mathrm{H}^{+}$ ] = 0.085 mol L^-1.What is the pH of the solution?

Determine the K_a of an acid whose 0.294 mol L^-1 solution has a pH of 2.80.

Determine the pH of a 0.227 mol L^-1 C₅H₅N solution at 25 °C.The K_b of C₅H₅N is 1.7 × 10^-9.

A solution with a hydroxide ion concentration of 4.15 × 10^-⁶ mol L^-1 is and has a hydrogen ion concentration of .

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

Determine the pH of a 0.116 mol L^-1 Ba(OH)₂ solution at 25 °C.

A 4.0 × 10^-3 mol L^-1 aqueous solution of $\mathrm { Ca } ( \mathrm { OH } ) _ { 2 }$ at 25.0 °C has a pH of ________.

Calculate the pOH of a solution that contains 3.9 × 10^-4 mol L^-1 H₃O⁺ at 25 °C.