Question 1

CO2 acts as an acid in the reaction CaO(s)+ CO2 ⇌ CaCO3(s)because it ________.

Accepted Answer

A) turns blue litmus red 
B) reacts with a metal 
C) is a proton donor 
D) is an electron-pair acceptor 
E) is a gas containing a non-metal 
A) turns blue litmus red 
B) reacts with a metal 
C) is a proton donor 
D) is an electron-pair acceptor 
E) is a gas containing a non-metal

Question 2

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

Accepted Answer

A) 1.0 × 10-5 
B) 9.00 
C) 1.0 × 10-9 
D) 5.0 ×   
E) 9.0 × 10-14 
A) 1.0 × 10-5 
B) 9.00 
C) 1.0 × 10-9 
D) 5.0 ×   
E) 9.0 × 10-14

Question 3

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 mol L-1 aqueous 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 mol L-1 
B) 4.3 × 10-7 mol L-1 
C) 4.3 × 10-9 mol L-1 
D) 5.6 × 10-11 mol L-1 
A) 6.6 × 10-5 mol L-1 
B) 4.3 × 10-7 mol L-1 
C) 4.3 × 10-9 mol L-1 
D) 5.6 × 10-11 mol L-1

Question 4

Calculate the pH for an aqueous solution of acetic acid that contains 5.15 × 10-3 mol L-1 hydronium
Ion.

Accepted Answer

A) 1.94 × 10-12  
B) 5.15 × 10-3  
C) 2.288 
D) 11.712 
A) 1.94 × 10-12  
B) 5.15 × 10-3  
C) 2.288 
D) 11.712

Question 5

A 0.214 M aqueous solution of a monoprotic base has a pH of 11.48.What is the ionization constant of this base?

Accepted Answer

A) 1.4 × 10-2 
B) 4.3 × 10-5 
C) 1.5 × 10-11 
D) 5.1 × 10-23 
E) 2.0 × 10-6 
A) 1.4 × 10-2 
B) 4.3 × 10-5 
C) 1.5 × 10-11 
D) 5.1 × 10-23 
E) 2.0 × 10-6

Question 6

A 0.632 M aqueous solution of a monoprotic base has a pH of 11.53.What is the ionization constant of this base?

Accepted Answer

A) 1.8 × 10-5 
B) 2.1 × 10-3 
C) 1.6 × 10-23 
D) 5.0 × 10-12 
E) 5.3 × 10-3 
A) 1.8 × 10-5 
B) 2.1 × 10-3 
C) 1.6 × 10-23 
D) 5.0 × 10-12 
E) 5.3 × 10-3

Question 7

Choose the strongest acid.

Accepted Answer

A) HF 
B) H2CO3  
C) HCN 
D) HC2H3O2  
E) HClO4  
A) HF 
B) H2CO3  
C) HCN 
D) HC2H3O2  
E) HClO4

Question 8

What is the selenide ion concentration [Se2-] for a 0.100 mol L-1 aqueous H2Se solution that has the stepwise dissociation constants of   And

Accepted Answer

A) 3.6 × 10-3 mol L-1 
B) 1.3 × 10-4 mol L-1 
C) 1.3 × 10-5 mol L-1 
D) 1.0 × 10-11 mol L-1 
A) 3.6 × 10-3 mol L-1 
B) 1.3 × 10-4 mol L-1 
C) 1.3 × 10-5 mol L-1 
D) 1.0 × 10-11 mol L-1

Question 9

What is the pH for a solution labeled "0.10 M arsenic acid (H3AsO4)"?
[Ka1 = 6 × 10-3,Ka2 = 1 × 10-7,Ka3 = 3 × 10-12]

Accepted Answer

A) 1.6 
B) 4.0 
C) 6.3 
D) 1.0 
E) 3.2 
A) 1.6 
B) 4.0 
C) 6.3 
D) 1.0 
E) 3.2

Question 10

A solution with a hydrogen ion concentration of 3.25 × 10-6 mol L-1 is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A) acidic,3.08 × 10-8 mol L-1 
B) acidic,3.08 × 10-9 mol L-1 
C) basic,3.08 × 10-8 mol L-1 
D) basic,3.08 × 10-9 mol L-1 
A) acidic,3.08 × 10-8 mol L-1 
B) acidic,3.08 × 10-9 mol L-1 
C) basic,3.08 × 10-8 mol L-1 
D) basic,3.08 × 10-9 mol L-1

Question 11

Which one of the following salts,when dissolved in water,produces the solution with a pH closest to 7.00?

Accepted Answer

A) CsCl 
B) CaO 
C) KH CO3 
D) NH4l  
A) CsCl 
B) CaO 
C) KH CO3 
D) NH4l

Question 12

Proton acceptor is an abbreviated definition of:

Accepted Answer

A) Br∅nsted-Lowry base 
B) Br∅nsted-Lowry acid 
C) Lewis base 
D) Lewis acid 
E) Arrhenius acid 
A) Br∅nsted-Lowry base 
B) Br∅nsted-Lowry acid 
C) Lewis base 
D) Lewis acid 
E) Arrhenius acid

Question 13

What is the pH of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

Accepted Answer

A) 2.000 
B) 6.000 
C) 10.000 
D) 12.000 
E) 14.000 
A) 2.000 
B) 6.000 
C) 10.000 
D) 12.000 
E) 14.000

Question 14

What is the pH of a 0.253 M aqueous solution of ammonium chloride? 
Kb (NH3)= 1.2 × 10-5

Accepted Answer

A) 2.7 
B) 4.8 
C) 9.2 
D) 11.3 
E) 9.9 
A) 2.7 
B) 4.8 
C) 9.2 
D) 11.3 
E) 9.9

Question 15

Which of the following are Br∅nsted-Lowry acids?
I.CH3COOH
II.[Cu(H2O)4]2+

III.H2O
IV.CH3NH2

V.H3O+

Accepted Answer

A) I,IIand III 
B) II,III,and IV 
C) I,II,IIIand IV 
D) I,II,III,and V 
E) II,IIIand V 
A) I,IIand III 
B) II,III,and IV 
C) I,II,IIIand IV 
D) I,II,III,and V 
E) II,IIIand V

Question 16

If an equal number of moles of the weak acid HCN and the strong base KOH are added to water,is the resulting solution acidic,basic,or neutral?

Accepted Answer

A) acidic 
B) basic 
C) neutral 
D) Depends on the solution volume 
A) acidic 
B) basic 
C) neutral 
D) Depends on the solution volume

Question 17

What is the [K+] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

Accepted Answer

A) 10-5 M 
B) 10-8 M 
C) 10-12 M 
D) 10-4 M 
E) 10-2 M 
A) 10-5 M 
B) 10-8 M 
C) 10-12 M 
D) 10-4 M 
E) 10-2 M

Question 18

0.272 g of a monoprotic acid (MW = 189 g/mol)is dissolved in water to produce 25.0 mL of a solution with pH = 4.93.Determine the ionization constant of the acid.

Accepted Answer

A) 4.1 × 10-8  
B) 1.4 × 10-10  
C) 2.1 × 10-4  
D) 2.8 × 10-7  
E) 2.4 × 10-9  
A) 4.1 × 10-8  
B) 1.4 × 10-10  
C) 2.1 × 10-4  
D) 2.8 × 10-7  
E) 2.4 × 10-9

Question 19

What is the pH of a 0.40 mol L-1 aqueous H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and

Accepted Answer

A) 2.14 
B) 3.89 
C) 4.28 
D) 5.57 
A) 2.14 
B) 3.89 
C) 4.28 
D) 5.57

Question 20

What is the pH of a 0.020 mol L-1 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

Exam 16: Acids and Bases

CO2 acts as an acid in the reaction CaO(s)+ CO2 ⇌ CaCO3(s)because it ________.

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 mol L-1 aqueous H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Calculate the pH for an aqueous solution of acetic acid that contains 5.15 × 10-3 mol L-1 hydronium Ion.

A 0.214 M aqueous solution of a monoprotic base has a pH of 11.48.What is the ionization constant of this base?

A 0.632 M aqueous solution of a monoprotic base has a pH of 11.53.What is the ionization constant of this base?

Choose the strongest acid.

What is the selenide ion concentration [Se2-] for a 0.100 mol L-1 aqueous H2Se solution that has the stepwise dissociation constants of And

What is the pH for a solution labeled "0.10 M arsenic acid (H3AsO4)"? [Ka1 = 6 × 10-3,Ka2 = 1 × 10-7,Ka3 = 3 × 10-12]

A solution with a hydrogen ion concentration of 3.25 × 10-6 mol L-1 is ________ and has a hydroxide ion concentration of ________.

Which one of the following salts,when dissolved in water,produces the solution with a pH closest to 7.00?

Proton acceptor is an abbreviated definition of:

What is the pH of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

What is the pH of a 0.253 M aqueous solution of ammonium chloride? Kb (NH3)= 1.2 × 10-5

Which of the following are Br∅nsted-Lowry acids? I.CH3COOH II.[Cu(H2O)4]2+ III.H2O IV.CH3NH2 V.H3O+

If an equal number of moles of the weak acid HCN and the strong base KOH are added to water,is the resulting solution acidic,basic,or neutral?

What is the [K+] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

0.272 g of a monoprotic acid (MW = 189 g/mol)is dissolved in water to produce 25.0 mL of a solution with pH = 4.93.Determine the ionization constant of the acid.

What is the pH of a 0.40 mol L-1 aqueous H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and

What is the pH of a 0.020 mol L-1 HClO4 solution?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

CO₂ acts as an acid in the reaction CaO(s)+ CO₂ ⇌ CaCO₃(s)because it ________.

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.010 mol L^-1aqueous H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Calculate the pH for an aqueous solution of acetic acid that contains 5.15 × 10^-3 mol L^-1hydronium Ion.

What is the selenide ion concentration [Se^2-] for a 0.100 mol L^-1 aqueous H₂Se solution that has the stepwise dissociation constants of And

What is the pH for a solution labeled "0.10 M arsenic acid (H₃AsO₄)"? [K_a1 = 6 × 10^-3,K_a2 = 1 × 10^-7,K_a3 = 3 × 10^-12]

A solution with a hydrogen ion concentration of 3.25 × 10^-⁶ mol L^-1 is and has a hydroxide ion concentration of .

What is the pH of a 0.253 M aqueous solution of ammonium chloride? K_b (NH₃)= 1.2 × 10^-5

Which of the following are Br∅nsted-Lowry acids? I.CH₃COOH II.[Cu(H₂O)₄]²⁺ ^III.H₂O IV.CH₃NH₂ _V.H₃O⁺

If an equal number of moles of the weak acid HCNand the strong base KOH are added to water,is the resulting solution acidic,basic,or neutral?

What is the [K⁺] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution?

What is the pH of a 0.40 mol L^-1 aqueous H₂Se solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and

What is the pH of a 0.020 mol L^-1 HClO₄ solution?