Question 1

What is the pH of a 0.250 M aqueous solution of formic acid? 
Ka = 1.8 × 10-4

Accepted Answer

A) 11.8 
B) 2.2 
C) 0.60 
D) 5.4 
E) 8.6 
A) 11.8 
B) 2.2 
C) 0.60 
D) 5.4 
E) 8.6 B

Question 2

HNO3 is a strong acid.

Accepted Answer

A) True 
 B)False  True

Question 3

What is the hydronium ion concentration of a 0.500 mol L-1 aqueous acetic acid solution with Ka = 1.8 × 10-5? 
The equation for the dissociation of acetic acid is below:

Accepted Answer

A) 3.0 × 10-2 mol L-1 
B) 4.2 × 10-2 mol L-1 
C) 3.0 × 10-3 mol L-1 
D) 4.2 × 10-3 mol L-1 
A) 3.0 × 10-2 mol L-1 
B) 4.2 × 10-2 mol L-1 
C) 3.0 × 10-3 mol L-1 
D) 4.2 × 10-3 mol L-1 C

Question 4

For Na2CO3,predict whether the aqueous solution is acidic,basic or neutral and why.

Accepted Answer

A) acidic because Na2CO3 is a strong acid 
B) basic because Na2CO3 is a weak base 
C) neutral because there is no hydrolysis 
D) basic because Na2CO3 is the salt of a weak acid 
E) acidic because Na2CO3 is the salt of a weak base 
A) acidic because Na2CO3 is a strong acid 
B) basic because Na2CO3 is a weak base 
C) neutral because there is no hydrolysis 
D) basic because Na2CO3 is the salt of a weak acid 
E) acidic because Na2CO3 is the salt of a weak base

Question 5

A certain acid,HA,has a Ka given by:
HA + H2O ⇌ H3O+ + A- Ka = 6.80 × 10-6 
What is the pH of a 0.247 M aqueous solution of the acid's potassium salt,KA,which undergoes the hydrolysis reaction?
A- + H2O ⇌ OH- + HA

Accepted Answer

A) 4.72 
B) 9.28 
C) 4.11 
D) 9.89 
E) 9.44 
A) 4.72 
B) 9.28 
C) 4.11 
D) 9.89 
E) 9.44

Question 6

Complete the following equation.List the conjugate acid base pairs.Put the base first in each pair.
HCl + NH3 ⇌

Accepted Answer

A) Cl- + NH4+ (NH3,NH4+)(Cl-,HCl) 
B) Cl- + NH4+ (NH3,HCl)(Cl-,NH4+) 
C) H2 + Cl- + NH2- (NH3,NH2-)(Cl-,HCl) 
D) H2Cl+ + NH2- (NH3,NH2-)(HCl,H2Cl) 
E) Cl- + NH4+ (NH3,Cl-)(NH4+,HCl) 
A) Cl- + NH4+ (NH3,NH4+)(Cl-,HCl) 
B) Cl- + NH4+ (NH3,HCl)(Cl-,NH4+) 
C) H2 + Cl- + NH2- (NH3,NH2-)(Cl-,HCl) 
D) H2Cl+ + NH2- (NH3,NH2-)(HCl,H2Cl) 
E) Cl- + NH4+ (NH3,Cl-)(NH4+,HCl)

Question 7

Which one of the following salts,when dissolved in water,produces the solution with the lowest pH?

Accepted Answer

A) NaCl 
B) KCl 
C) MgCl2 
D) AlCl3 
A) NaCl 
B) KCl 
C) MgCl2 
D) AlCl3

Question 8

What is the pH of a 0.563 M aqueous solution of ethylammonium bromide? Kb (ethylammonia)= 4.3 × 10-4

Accepted Answer

A) 8.58 
B) 1.79 
C) 8.68 
D) 5.32 
E) 5.44 
A) 8.58 
B) 1.79 
C) 8.68 
D) 5.32 
E) 5.44

Question 9

Hypochlorous acid (HOCl)has an ionization constant of 3.2 × 10-8.What is its percent ionization in 1.0 M and 0.10 M solutions,respectively?

Accepted Answer

A) 0.018% and 0.057% 
B) 0.032% and 0.0032% 
C) 0.57% and 0.18% 
D) 0.57% in both 
E) 0.32% in both 
A) 0.018% and 0.057% 
B) 0.032% and 0.0032% 
C) 0.57% and 0.18% 
D) 0.57% in both 
E) 0.32% in both

Question 10

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 11

Calculate the pH of a 0.080 mol L-1 aqueous carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 1.10 
B) 3.73 
C) 6.37 
D) 10.25 
A) 1.10 
B) 3.73 
C) 6.37 
D) 10.25

Question 12

List the following acids in order of increasing strength:
H3PO4 H2SO4 HClO4

Accepted Answer

A) HClO4 3PO4 2SO4  
B) H2SO4 4 3PO4  
C) H2SO4 3PO4 4  
D) H3PO4 2SO4 4  
E) HClO4 2SO4 3PO4  
A) HClO4 3PO4 2SO4  
B) H2SO4 4 3PO4  
C) H2SO4 3PO4 4  
D) H3PO4 2SO4 4  
E) HClO4 2SO4 3PO4

Question 13

What is the pH of a 0.375 M aqueous solution of methylammonium chloride? 
Kb (CH3NH2)= 4.2 × 10-4

Accepted Answer

A) 12.1 
B) 1.9 
C) 5.5 
D) 8.5 
E) 11.0 
A) 12.1 
B) 1.9 
C) 5.5 
D) 8.5 
E) 11.0

Question 14

Choose the Br∅nsted-Lowry acids and bases in the following equation:
HCO3- + OH- ⇌ H2O + CO32-

Accepted Answer

A) acids HCO3-,H2O bases OH-,CO32-  
B) acids OH-,CO32- bases HCO3-,H2O 
C) acids H2O,OH- bases HCO3-,CO32-  
D) acids HCO3-,OH- bases CO32-,H2O 
E) acids H2O,CO32- bases HCO3-,OH-  
A) acids HCO3-,H2O bases OH-,CO32-  
B) acids OH-,CO32- bases HCO3-,H2O 
C) acids H2O,OH- bases HCO3-,CO32-  
D) acids HCO3-,OH- bases CO32-,H2O 
E) acids H2O,CO32- bases HCO3-,OH-

Question 15

What is the pH of a 0.175 M aqueous solution of potassium benzoate? 
Ka (benzoic acid)= 6.3 × 10-5

Accepted Answer

A) 9.10 
B) 3.44 
C) 10.56 
D) 5.28 
E) 8.72 
A) 9.10 
B) 3.44 
C) 10.56 
D) 5.28 
E) 8.72

Question 16

What is the pH of a 0.530 M aqueous solution of hypochlorus acid? 
Ka = 2.9 × 10-8

Accepted Answer

A) 10.6 
B) 3.4 
C) 10.1 
D) 3.9 
E) 0.28 
A) 10.6 
B) 3.4 
C) 10.1 
D) 3.9 
E) 0.28

Question 17

According to the Arrhenius theory,a neutralization reaction involves:

Accepted Answer

A) the combination of hydrogen ions and hydroxide ions to form water 
B) the dissociation of a strong acid to hydrogen ions and an anion 
C) the dissociation of a strong base into hydroxide ions and a cation 
D) the addition of water to ammonia to make ammonium hydroxide 
E) the combination of an acid with a base to make only water 
A) the combination of hydrogen ions and hydroxide ions to form water 
B) the dissociation of a strong acid to hydrogen ions and an anion 
C) the dissociation of a strong base into hydroxide ions and a cation 
D) the addition of water to ammonia to make ammonium hydroxide 
E) the combination of an acid with a base to make only water

Question 18

0.375 g of a monoprotic acid (MW = 245 g/mol)is dissolved in water to produce 25.0 mL of a solution with pH = 3.28.Determine the ionization constant of the acid.

Accepted Answer

A) 8.56 × 10-3  
B) 4.5 × 10-6  
C) 7.4 × 10-5  
D) 4.5 × 10-3  
E) 2.3 × 10-2  
A) 8.56 × 10-3  
B) 4.5 × 10-6  
C) 7.4 × 10-5  
D) 4.5 × 10-3  
E) 2.3 × 10-2

Question 19

The ionization constant for ammonia is 1.8 × 10-5.What is the pH of an aqueous solution labeled 0.50 M ammonia?

Accepted Answer

A) 7.30 
B) 9.12 
C) 10.26 
D) 11.48 
E) 12.52 
A) 7.30 
B) 9.12 
C) 10.26 
D) 11.48 
E) 12.52

Question 20

The pH of a solution of NH4C2H3O2 is approximately 7.The best explanation is:

Accepted Answer

A) This salt does not react with water. 
B) Ammonium acetate is a weak electrolyte. 
C) All salts of weak acids and weak bases are neutral. 
D) Aqueous ammonia and acetic acid have approximately equal ionization constants. 
E) The salt is a product of a strong acid and a strong base. 
A) This salt does not react with water. 
B) Ammonium acetate is a weak electrolyte. 
C) All salts of weak acids and weak bases are neutral. 
D) Aqueous ammonia and acetic acid have approximately equal ionization constants. 
E) The salt is a product of a strong acid and a strong base.

Exam 16: Acids and Bases

What is the pH of a 0.250 M aqueous solution of formic acid? Ka = 1.8 × 10-4

HNO3 is a strong acid.

What is the hydronium ion concentration of a 0.500 mol L-1 aqueous acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below:

For Na2CO3,predict whether the aqueous solution is acidic,basic or neutral and why.

A certain acid,HA,has a Ka given by: HA + H2O ⇌ H3O+ + A- Ka = 6.80 × 10-6 What is the pH of a 0.247 M aqueous solution of the acid's potassium salt,KA,which undergoes the hydrolysis reaction? A- + H2O ⇌ OH- + HA

Complete the following equation.List the conjugate acid base pairs.Put the base first in each pair. HCl + NH3 ⇌

Which one of the following salts,when dissolved in water,produces the solution with the lowest pH?

What is the pH of a 0.563 M aqueous solution of ethylammonium bromide? Kb (ethylammonia)= 4.3 × 10-4

Hypochlorous acid (HOCl)has an ionization constant of 3.2 × 10-8.What is its percent ionization in 1.0 M and 0.10 M solutions,respectively?

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

Calculate the pH of a 0.080 mol L-1 aqueous carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

List the following acids in order of increasing strength: H3PO4 H2SO4 HClO4

What is the pH of a 0.375 M aqueous solution of methylammonium chloride? Kb (CH3NH2)= 4.2 × 10-4

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCO3- + OH- ⇌ H2O + CO32-

What is the pH of a 0.175 M aqueous solution of potassium benzoate? Ka (benzoic acid)= 6.3 × 10-5

What is the pH of a 0.530 M aqueous solution of hypochlorus acid? Ka = 2.9 × 10-8

According to the Arrhenius theory,a neutralization reaction involves:

0.375 g of a monoprotic acid (MW = 245 g/mol)is dissolved in water to produce 25.0 mL of a solution with pH = 3.28.Determine the ionization constant of the acid.

The ionization constant for ammonia is 1.8 × 10-5.What is the pH of an aqueous solution labeled 0.50 M ammonia?

The pH of a solution of NH4C2H3O2 is approximately 7.The best explanation is:

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

What is the pH of a 0.250 M aqueous solution of formic acid? K_a = 1.8 × 10^-4

HNO₃ is a strong acid.

What is the hydronium ion concentration of a 0.500 mol L^-1 aqueous acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is below:

For Na₂CO₃,predict whether the aqueous solution is acidic,basic or neutral and why.

A certain acid,HA,has a K_a given by: HA + H₂O ⇌ H₃O⁺ + A^- K_a = 6.80 × 10^-6 What is the pH of a 0.247 M aqueous solution of the acid's potassium salt,KA,which undergoes the hydrolysis reaction? A^- + H₂O ⇌ OH^- + HA

Complete the following equation.List the conjugate acid base pairs.Put the base first in each pair. HCl + NH₃ ⇌

What is the pH of a 0.563 M aqueous solution of ethylammonium bromide? K_b (ethylammonia)= 4.3 × 10^-4

Hypochlorous acid (HOCl)has an ionization constant of 3.2 × 10^-8.What is its percent ionization in 1.0 M and 0.10 M solutions,respectively?

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

Calculate the pH of a 0.080 mol L^-1 aqueous carbonic acid solution,H₂CO_3(aq),that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

List the following acids in order of increasing strength: H₃PO₄ H₂SO₄ HClO₄

What is the pH of a 0.375 M aqueous solution of methylammonium chloride? K_b (CH₃NH₂)= 4.2 × 10^-4

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCO₃^- + OH^- ⇌ H₂O + CO₃^2-

What is the pH of a 0.175 M aqueous solution of potassium benzoate? Ka (benzoic acid)= 6.3 × 10^-5

What is the pH of a 0.530 M aqueous solution of hypochlorus acid? K_a = 2.9 × 10^-8

The ionization constant for ammonia is 1.8 × 10^-5.What is the pH of an aqueous solution labeled 0.50 M ammonia?

The pH of a solution of NH₄C₂H₃O₂ is approximately 7.The best explanation is: