Question 1

A base is always the titrant.

Accepted Answer

A) True 
 B)False

Question 2

HN3 and NH3 can make a buffer.

Accepted Answer

A) True 
 B)False

Question 3

Which of the following is formed when H2SO3 reacts with KOH?

Accepted Answer

A)  K2SO4 
B)  K2SO3 
C)  K2(SO4)3 
D)  KH 
E)  KOH 
A)  K2SO4 
B)  K2SO3 
C)  K2(SO4)3 
D)  KH 
E)  KOH

Question 4

What is [OH−] for an aqueous solution whose pH is 3.89?

Accepted Answer

A)  7.76 *10-11 M 
B)  1.29*10-12 M 
C)  1.29 * 1012 M 
D)  2.58 * 1012 M 
E)  3.86 * 10-12 M 
A)  7.76 *10-11 M 
B)  1.29*10-12 M 
C)  1.29 * 1012 M 
D)  2.58 * 1012 M 
E)  3.86 * 10-12 M

Question 5

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. H2C2O4 + 2F−$\rightarrow$ ?

Accepted Answer

A)  2H2C2O4 and F− 
B)  C2O42− and 2HF 
C)  C2O4 and 2F− 
D)  H2C2O3- and F2 
E)  C2O3- and 2F2 
A)  2H2C2O4 and F− 
B)  C2O42− and 2HF 
C)  C2O4 and 2F− 
D)  H2C2O3- and F2 
E)  C2O3- and 2F2

Question 6

A _____is any ionic compound made by combining an acid with a base.

Accepted Answer

The answer of A _____is any ionic compound made by...

Question 7

What is [H+] for an aqueous solution whose pOH is 9.89?

Accepted Answer

A)  2.33 * 10-6 M 
B)  7.76 *10-5 M 
C)  2.33 * 106 M 
D)  4.11 M 
E)  1.55*10-6 M 
A)  2.33 * 10-6 M 
B)  7.76 *10-5 M 
C)  2.33 * 106 M 
D)  4.11 M 
E)  1.55*10-6 M

Question 8

Which of the following is an Arrhenius base?

Accepted Answer

A)  HC2H3O2 
B)  HClO3 
C)  Al(OH)3 
D)  PCl5 
E)  HgCl2 
A)  HC2H3O2 
B)  HClO3 
C)  Al(OH)3 
D)  PCl5 
E)  HgCl2

Question 9

An Arrhenius acid is a compound that increases the hydroxide ion concentration in aqueous solution.

Accepted Answer

A) True 
 B)False

Question 10

H+ ions and H3O+ ions are often considered interchangeable when writing chemical equations.

Accepted Answer

A) True 
 B)False

Question 11

The product of the two concentrations-[H+][OH−]-is always equal to 1.0 × 10−14. This is known as the _____.

Accepted Answer

autoioniza

Question 12

What is the conjugate base of HClO3?

Accepted Answer

A)  HClO3- 
B)  HClO3+ 
C)  ClO3- 
D)  H2ClO3- 
E)  ClO4- 
A)  HClO3- 
B)  HClO3+ 
C)  ClO3- 
D)  H2ClO3- 
E)  ClO4-

Question 13

Explain neutralization reactions with examples.

Accepted Answer

A reaction between an acid and a base is

Question 14

The Brønsted-Lowry definition of acid and base is limited to aqueous (that is, water) solutions.

Accepted Answer

A) True 
 B)False

Question 15

What is the pH of a solution when [OH-] is 8.04 × 10−13 M?

Accepted Answer

A)  0.904 
B)  1.91 
C)  0.975 
D)  14.0 
E)  12.09 
A)  0.904 
B)  1.91 
C)  0.975 
D)  14.0 
E)  12.09

Question 16

Which of the following acids ionizes 100% in aqueous solution?

Accepted Answer

A)  HBr 
B)  HBrO3 
C)  HNO2 
D)  HCOOH 
E)  CH3COOH 
A)  HBr 
B)  HBrO3 
C)  HNO2 
D)  HCOOH 
E)  CH3COOH

Question 17

Describe the process of titration.

Accepted Answer

Performing chemical reactions quantitati

Question 18

Differentiate Brønsted-Lowry acids and Brønsted-Lowry bases.

Accepted Answer

A Brønsted-Lowry acid is any species tha

Question 19

When ammonia reacts with water, ammonia acts like a Brønsted-Lowry base.

Accepted Answer

A) True 
 B)False

Question 20

What is [OH-] in a 0.077 M solution of HClO4?

Accepted Answer

A)  7.6 *10-13 M 
B)  1.3 *10-13 M 
C)  6.5 * 10-14 M 
D)  6.5 * 1014 M 
E)  0.077 M 
A)  7.6 *10-13 M 
B)  1.3 *10-13 M 
C)  6.5 * 10-14 M 
D)  6.5 * 1014 M 
E)  0.077 M

A base is always the titrant.

HN₃ and NH₃ can make a buffer.

Which of the following is formed when H₂SO₃ reacts with KOH?

What is [OH⁻] for an aqueous solution whose pH is 3.89?

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. H₂C₂O₄ + 2F⁻ $\rightarrow$ ?

A _____is any ionic compound made by combining an acid with a base.

What is [H⁺] for an aqueous solution whose pOH is 9.89?

Which of the following is an Arrhenius base?

An Arrhenius acid is a compound that increases the hydroxide ion concentration in aqueous solution.

H⁺ ions and H₃O⁺ ions are often considered interchangeable when writing chemical equations.

The product of the two concentrations-[H⁺][OH⁻]-is always equal to 1.0 × 10⁻¹⁴. This is known as the _____.

What is the conjugate base of HClO₃?

Explain neutralization reactions with examples.

The Brønsted-Lowry definition of acid and base is limited to aqueous (that is, water) solutions.

What is the pH of a solution when [OH^-] is 8.04 × 10⁻¹³ M?

Which of the following acids ionizes 100% in aqueous solution?

Describe the process of titration.

Differentiate Brønsted-Lowry acids and Brønsted-Lowry bases.

When ammonia reacts with water, ammonia acts like a Brønsted-Lowry base.

What is [OH^-] in a 0.077 M solution of HClO₄?

What Is Chemistry

Measurements

Atoms, Molecules, and Ions

Chemical Reactions and Equations

Stoichiometry and the Mole

Gases

Energy and Chemistry

Electronic Structure

Chemical Bonds

Solids and Liquids

Solutions

Chemical Equilibrium

Oxidation and Reduction

Nuclear Chemistry

Organic Chemistry

Filters

Exam 12: Acids and Bases

A base is always the titrant.

HN3 and NH3 can make a buffer.

Which of the following is formed when H2SO3 reacts with KOH?

What is [OH−] for an aqueous solution whose pH is 3.89?

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. H2C2O4 + 2F− →\rightarrow→ ?

A _____is any ionic compound made by combining an acid with a base.

What is [H+] for an aqueous solution whose pOH is 9.89?

Which of the following is an Arrhenius base?

An Arrhenius acid is a compound that increases the hydroxide ion concentration in aqueous solution.

H+ ions and H3O+ ions are often considered interchangeable when writing chemical equations.

The product of the two concentrations-[H+][OH−]-is always equal to 1.0 × 10−14. This is known as the _____.

What is the conjugate base of HClO3?

Explain neutralization reactions with examples.

The Brønsted-Lowry definition of acid and base is limited to aqueous (that is, water) solutions.

What is the pH of a solution when [OH-] is 8.04 × 10−13 M?

Which of the following acids ionizes 100% in aqueous solution?

Describe the process of titration.

Differentiate Brønsted-Lowry acids and Brønsted-Lowry bases.

When ammonia reacts with water, ammonia acts like a Brønsted-Lowry base.

What is [OH-] in a 0.077 M solution of HClO4?

What Is Chemistry

Measurements

Atoms, Molecules, and Ions

Chemical Reactions and Equations

Stoichiometry and the Mole

Gases

Energy and Chemistry

Electronic Structure

Chemical Bonds

Solids and Liquids

Solutions

Chemical Equilibrium

Oxidation and Reduction

Nuclear Chemistry

Organic Chemistry

Filters

HN₃ and NH₃ can make a buffer.

Which of the following is formed when H₂SO₃ reacts with KOH?

What is [OH⁻] for an aqueous solution whose pH is 3.89?

Predict the products of this reaction, assuming it undergoes a Brønsted-Lowry acid-base reaction. H₂C₂O₄ + 2F⁻ $\rightarrow$ ?

What is [H⁺] for an aqueous solution whose pOH is 9.89?

H⁺ ions and H₃O⁺ ions are often considered interchangeable when writing chemical equations.

The product of the two concentrations-[H⁺][OH⁻]-is always equal to 1.0 × 10⁻¹⁴. This is known as the _____.

What is the conjugate base of HClO₃?

What is the pH of a solution when [OH^-] is 8.04 × 10⁻¹³ M?

What is [OH^-] in a 0.077 M solution of HClO₄?