Question 1

A water solution is considered acidic when what is true?

Accepted Answer

A) [H+] = [OH-] 
B) [H+] -] 
C) [OH- ] > [H+] 
D) [H+] > [OH-] 
E) [H+] = Kw 
A) [H+] = [OH-] 
B) [H+] -] 
C) [OH- ] > [H+] 
D) [H+] > [OH-] 
E) [H+] = Kw

Question 2

Consider the following image which depicts the reactants in an acid-base reaction.Atoms other than H are labeled with the element symbol.   The products of this reaction are shown below.  
Which of the following is a correct interpretation of this reaction?

Accepted Answer

A) 1 and 2 are a conjugate acid-base pair. 
B) 3 and 4are a conjugate acid-base pair. 
C) 1 and 4 are a conjugate acid-base pair. 
D) 2 and 4 are a conjugate acid-base pair. 
E) 1 and 3 are a conjugate acid-base pair. 
A) 1 and 2 are a conjugate acid-base pair. 
B) 3 and 4are a conjugate acid-base pair. 
C) 1 and 4 are a conjugate acid-base pair. 
D) 2 and 4 are a conjugate acid-base pair. 
E) 1 and 3 are a conjugate acid-base pair.

Question 3

What is the conjugate base of H3C6H5O7?

Accepted Answer

A) C6H5O73- 
B) H2C6H5O7- 
C) H3C6H5O7- 
D) H4C6H5O7+ 
E) H3C6H5O7(OH)- 
A) C6H5O73- 
B) H2C6H5O7- 
C) H3C6H5O7- 
D) H4C6H5O7+ 
E) H3C6H5O7(OH)-

Question 4

Which of the following statements is incorrect?

Accepted Answer

A) Acid-base reactions involve a transfer of protons; redox reactions,a transfer of electrons 
B) In both redox and acid-base reactions,the reactants are given special names to indicate their roles in the transfer process 
C) Just as certain species can either donate or accept protons and thereby behave as an acid in one reaction and a base in another,certain species can either accept or donate electrons,acting as an oxidizing agent in one reaction and a reducing agent in another 
D) Just as acids and bases may be classified as "strong" or "weak" depending on how readily they donate or accept protons,the strengths of oxidizing and reducing agents may be compared according to their tendencies to attract or release electrons 
E) Unlike most acid-base reactions in solution,which reach a state of equilibrium,most aqueous redox reactions do not reach a state of equilibrium and proceed entirely either in the forward or reverse direction 
A) Acid-base reactions involve a transfer of protons; redox reactions,a transfer of electrons 
B) In both redox and acid-base reactions,the reactants are given special names to indicate their roles in the transfer process 
C) Just as certain species can either donate or accept protons and thereby behave as an acid in one reaction and a base in another,certain species can either accept or donate electrons,acting as an oxidizing agent in one reaction and a reducing agent in another 
D) Just as acids and bases may be classified as "strong" or "weak" depending on how readily they donate or accept protons,the strengths of oxidizing and reducing agents may be compared according to their tendencies to attract or release electrons 
E) Unlike most acid-base reactions in solution,which reach a state of equilibrium,most aqueous redox reactions do not reach a state of equilibrium and proceed entirely either in the forward or reverse direction

Question 5

A solution has a hydroxide ion concentration of 1 * 10-11 M.What is the pH of the solution,and is it acidic or basic?

Accepted Answer

A) pH = 11,basic 
B) pH = 3,basic 
C) pH = 3,acidic 
D) pH = -11 acidic 
E) pH = -11,basic 
A) pH = 11,basic 
B) pH = 3,basic 
C) pH = 3,acidic 
D) pH = -11 acidic 
E) pH = -11,basic

Question 6

Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

Accepted Answer

A) HSO3-(aq) 
B) NaOH(s) 
C) NH4+(aq) 
D) Al(OH)3(s) 
E) NH4OH(aq) 
A) HSO3-(aq) 
B) NaOH(s) 
C) NH4+(aq) 
D) Al(OH)3(s) 
E) NH4OH(aq)

Question 7

What is the hydrogen ion concentration in a solution with pH = 11.27? Is the solution acidic or basic?

Accepted Answer

A) 5.4 * 10-12 M basic 
B) 1.86 *0-3 M basic 
C) 5.37 * 10-12 M acidic 
D) 1.86 *10-3 M acidic 
E) 2.73 M acidic 
A) 5.4 * 10-12 M basic 
B) 1.86 *0-3 M basic 
C) 5.37 * 10-12 M acidic 
D) 1.86 *10-3 M acidic 
E) 2.73 M acidic

Question 8

Which pair below cannot have a Brønsted-Lowry acid base reaction between them?

Accepted Answer

A) OH- and NH 
B) PO43- and ClO- 
C) HCO3- and SO32- 
D) HClO4 and HNO2 
E) HSO4- and HCl 
A) OH- and NH 
B) PO43- and ClO- 
C) HCO3- and SO32- 
D) HClO4 and HNO2 
E) HSO4- and HCl

Question 9

A pH meter is used to test the pH of a solution.See the figure below.   How is the solution classified?

Accepted Answer

A) neutral 
B) acidic 
C) basic 
A) neutral 
B) acidic 
C) basic

Question 10

Which of the following conforms to the Arrhenius definition of an acid?

Accepted Answer

A) H2O(   ) 
B) HBrO3(aq) 
C) HCO3-(aq) 
D) Al3+(aq) 
E) Mg(OH)2(s) 
A) H2O(   ) 
B) HBrO3(aq) 
C) HCO3-(aq) 
D) Al3+(aq) 
E) Mg(OH)2(s)

Question 11

The pH of a solution is 5.330.Find [OH-].

Accepted Answer

A) [OH-] = 2.14*10-9 molar 
B) [OH-] = 4.70 *10-11 molar 
C) [OH-] = 5.33 *10-7 molar 
D) [OH-] = 4.70 * 10-6 molar 
E) [OH-] = 5.33 molar 
A) [OH-] = 2.14*10-9 molar 
B) [OH-] = 4.70 *10-11 molar 
C) [OH-] = 5.33 *10-7 molar 
D) [OH-] = 4.70 * 10-6 molar 
E) [OH-] = 5.33 molar

Question 12

What are the [H+] and [OH-] of a solution made by dissolving 0.0001 mole of HI in sufficient water to make 1.00 liter of solution?

Accepted Answer

A) [H+] = 4 M [OH-] = 10 M 
B) [H+] = 1 *10-14 M [OH-] = 1 *10-4 M 
C) [H+] = 1*10-10 M [OH-] = 1 * 10-4 M 
D) [H+] = 1 *10-4 M [OH-] = 1 *10-14 M 
E) [H+] = 1 *10-4 M [OH-] = 1 *10-10 M 
A) [H+] = 4 M [OH-] = 10 M 
B) [H+] = 1 *10-14 M [OH-] = 1 *10-4 M 
C) [H+] = 1*10-10 M [OH-] = 1 * 10-4 M 
D) [H+] = 1 *10-4 M [OH-] = 1 *10-14 M 
E) [H+] = 1 *10-4 M [OH-] = 1 *10-10 M

Question 13

A solution is made by dissolving 0.0010 mole KOH in enough water to make 1.00 liter of solution.What are the pH and the pOH of the solution?

Accepted Answer

A) pH = 3,pOH = 11 
B) pH = 3,pOH = 3 
C) pH = -11,pOH = -3 
D) pH = 11,pOH = 3 
E) pH = 10-11,pOH = 10-3 
A) pH = 3,pOH = 11 
B) pH = 3,pOH = 3 
C) pH = -11,pOH = -3 
D) pH = 11,pOH = 3 
E) pH = 10-11,pOH = 10-3

Question 14

What is the pH of a solution if [H+] = 3.1 *10-4 molar?

Accepted Answer

A) pH = 4.31 
B) pH = 10.49 
C) pH = -9.69 
D) pH = -3.51 
E) pH = 3.51 
A) pH = 4.31 
B) pH = 10.49 
C) pH = -9.69 
D) pH = -3.51 
E) pH = 3.51

Question 15

Which is the correct net ionic equation for the reaction between HC2O4- and HPO42-? (Note: H2C2O4 is a stronger acid than H2PO4-.)

Accepted Answer

A) HC2O4- + HPO42-   H+ + H2O42- + HPO42- 
B) HC2O4- + HPO42-   H+ + HC2O4- + PO43- 
C) HC2O4- + HPO42-   C2O42- + H2PO4- 
D) HC2O4- + HPO42-      H2C2O4 + PO43- 
E) HC2O4- + HPO42-      H2 + C2O42- + PO43- 
A) HC2O4- + HPO42-   H+ + H2O42- + HPO42- 
B) HC2O4- + HPO42-   H+ + HC2O4- + PO43- 
C) HC2O4- + HPO42-   C2O42- + H2PO4- 
D) HC2O4- + HPO42-      H2C2O4 + PO43- 
E) HC2O4- + HPO42-      H2 + C2O42- + PO43-

Question 16

Which of the following properties is traditionally associated with Arrhenius bases?

Accepted Answer

A) They cause blue litmus indicator to turn red 
B) They form precipitates with solutions of most metals 
C) They react with carbonates to release CO2 
D) They release hydrogen when zinc is added 
E) They contain hydronium ions 
A) They cause blue litmus indicator to turn red 
B) They form precipitates with solutions of most metals 
C) They react with carbonates to release CO2 
D) They release hydrogen when zinc is added 
E) They contain hydronium ions

Question 17

A substance that can act as both a proton source and a proton remover is called ...

Accepted Answer

A) a Brønsted-Lowry acid 
B) a Lewis acid 
C) amphibious 
D) amphoteric 
E) neither an acid nor a base 
A) a Brønsted-Lowry acid 
B) a Lewis acid 
C) amphibious 
D) amphoteric 
E) neither an acid nor a base

Question 18

Consider the following generalized reaction.   For this reaction,which of the following is correct?

Accepted Answer

A) A is proton source. 
B) B is a proton remover. 
C) A is an electron pair donor. 
D) B is an electron pair acceptor. 
E) This a Lewis acid-base reaction. 
A) A is proton source. 
B) B is a proton remover. 
C) A is an electron pair donor. 
D) B is an electron pair acceptor. 
E) This a Lewis acid-base reaction.

Question 19

The hydrogen ion concentration of a solution is 1 * 10-4 M.What is the pH of the solution,and is it acidic or basic?

Accepted Answer

A) pH = 10,acidic 
B) pH = 10,basic 
C) pH =13,basic 
D) pH = -4,basic 
E) pH = 4,acidic 
A) pH = 10,acidic 
B) pH = 10,basic 
C) pH =13,basic 
D) pH = -4,basic 
E) pH = 4,acidic

Question 20

What is the conjugate acid of HPO42-(aq)?

Accepted Answer

A) H3PO4(aq) 
B) HPO42-(aq) 
C) H2PO4-(aq) 
D) PO43-(aq) 
E) H3O+(aq) 
A) H3PO4(aq) 
B) HPO42-(aq) 
C) H2PO4-(aq) 
D) PO43-(aq) 
E) H3O+(aq)

Exam 17: Acid-Base Proton-Transferreactions

A water solution is considered acidic when what is true?

Consider the following image which depicts the reactants in an acid-base reaction.Atoms other than H are labeled with the element symbol. The products of this reaction are shown below. Which of the following is a correct interpretation of this reaction?

What is the conjugate base of H3C6H5O7?

Which of the following statements is incorrect?

A solution has a hydroxide ion concentration of 1 * 10-11 M.What is the pH of the solution,and is it acidic or basic?

Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

What is the hydrogen ion concentration in a solution with pH = 11.27? Is the solution acidic or basic?

Which pair below cannot have a Brønsted-Lowry acid base reaction between them?

A pH meter is used to test the pH of a solution.See the figure below. How is the solution classified?

Which of the following conforms to the Arrhenius definition of an acid?

The pH of a solution is 5.330.Find [OH-].

What are the [H+] and [OH-] of a solution made by dissolving 0.0001 mole of HI in sufficient water to make 1.00 liter of solution?

A solution is made by dissolving 0.0010 mole KOH in enough water to make 1.00 liter of solution.What are the pH and the pOH of the solution?

What is the pH of a solution if [H+] = 3.1 *10-4 molar?

Which is the correct net ionic equation for the reaction between HC2O4- and HPO42-? (Note: H2C2O4 is a stronger acid than H2PO4-.)

Which of the following properties is traditionally associated with Arrhenius bases?

A substance that can act as both a proton source and a proton remover is called ...

Consider the following generalized reaction. For this reaction,which of the following is correct?

The hydrogen ion concentration of a solution is 1 * 10-4 M.What is the pH of the solution,and is it acidic or basic?

What is the conjugate acid of HPO42-(aq)?

Matter and Energy

Measurement and Chemical Calculations

Introduction to Gases

Atomic Theory: the Nuclear Model of the Atom

Chemical Nomenclature

Chemical Formula Relationships

Chemical Reactions

Chemical Change

Quantity Relationships in Chemical Reactions

Atomic Theory: the Quantum Model of the Atom

Chemical Bonding

Structure and Shape

The Ideal Gas Law and Its Applications

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Chemical Equilibrium

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Filters

What is the conjugate base of H₃C₆H₅O₇?

A solution has a hydroxide ion concentration of 1 * 10^-¹¹ M.What is the pH of the solution,and is it acidic or basic?

The pH of a solution is 5.330.Find [OH^-].

What are the [H⁺] and [OH^-] of a solution made by dissolving 0.0001 mole of HI in sufficient water to make 1.00 liter of solution?

What is the pH of a solution if [H⁺] = 3.1 *10^-⁴ molar?

Which is the correct net ionic equation for the reaction between HC₂O₄^- and HPO₄²^-? (Note: H₂C₂O₄ is a stronger acid than H₂PO₄^-.)

The hydrogen ion concentration of a solution is 1 * 10^-⁴ M.What is the pH of the solution,and is it acidic or basic?

What is the conjugate acid of HPO₄²^-(aq)?