Question 1

Which solution has the highest pH?

Accepted Answer

A) 4.3 × 10-8 M H3O+ 
B) 1.0 × 10-7 M H3O+ 
C) 5.1 × 10-2 M H3O+ 
D) 1.9 × 10-8 M H3O+ 
E) 1.0 × 10-2 M H3O+ 
A) 4.3 × 10-8 M H3O+ 
B) 1.0 × 10-7 M H3O+ 
C) 5.1 × 10-2 M H3O+ 
D) 1.9 × 10-8 M H3O+ 
E) 1.0 × 10-2 M H3O+ D

Question 2

Each day, the stomach produces 2.0 L of gastric juice that contains 0.10 M HCl. Phillips Milk of Magnesia is a white-colored, aqueous, mildly alkaline suspension of magnesium hydroxide formulated at 8.0 % (w/v). It would take _____ mL of milk of magnesia to titrate the stomach acid produced in each day. (Mg(OH)2 molar mass = 58.32 g/mol)

Accepted Answer

73

Question 3

Which species is the conjugate base of NH3?

Accepted Answer

A) NH4+ 
B) NH2 
C) NH2- 
D) H2O 
E) NH4OH 
A) NH4+ 
B) NH2 
C) NH2- 
D) H2O 
E) NH4OH C

Question 4

In a reversible acid-base reaction, equilibrium favors the formation of the acid with the smaller Ka value.

Accepted Answer

A) True 
 B)False

Question 5

What is the balanced equation for the acid-base reaction of nitrous acid with lithium hydroxide?

Accepted Answer

A) LiOH(aq)+ HNO3(aq)   H2O(l)+ LiNO3(aq) 
B) Li(OH)2(aq)+ 2 HNO3(aq)   2 H2O(l)+ Li(NO3)2(aq) 
C) LiOH(aq)+ HNO2(aq)   H2O(l)+ LiNO2(aq) 
D) 2 LiOH(aq)+ H2NO2(aq)   2 H2O(l)+ Li2NO2(aq) 
A) LiOH(aq)+ HNO3(aq)   H2O(l)+ LiNO3(aq) 
B) Li(OH)2(aq)+ 2 HNO3(aq)   2 H2O(l)+ Li(NO3)2(aq) 
C) LiOH(aq)+ HNO2(aq)   H2O(l)+ LiNO2(aq) 
D) 2 LiOH(aq)+ H2NO2(aq)   2 H2O(l)+ Li2NO2(aq)

Question 6

In the acid-base reaction: F-(aq)+ HNO3(aq)   HF(aq)+ NO3-(aq)

Accepted Answer

A) F- is the acid and its conjugate base is HF, and HNO3 is the base and its conjugate acid is NO3-(aq). 
B) HNO3 is the acid and its conjugate base is NO3-(aq), and F- is the base and its conjugate acid is HF. 
C) F- is the acid and its conjugate base is NO3-(aq), and HNO3 is the base and its conjugate acid is HF. 
D) HNO3 is the acid and its conjugate base is HF, and F- is the base and its conjugate acid is NO3-(aq). 
A) F- is the acid and its conjugate base is HF, and HNO3 is the base and its conjugate acid is NO3-(aq). 
B) HNO3 is the acid and its conjugate base is NO3-(aq), and F- is the base and its conjugate acid is HF. 
C) F- is the acid and its conjugate base is NO3-(aq), and HNO3 is the base and its conjugate acid is HF. 
D) HNO3 is the acid and its conjugate base is HF, and F- is the base and its conjugate acid is NO3-(aq).

Question 7

A solution in which [-OH] = 6.3 × 10-7 M has a higher pH than a solution with a [-OH] = 4.3 × 10-2 M.

Accepted Answer

A) True 
 B)False

Question 8

What is the expression for Kw, the ion-product constant for water?

Accepted Answer

A) Kw = [H2O]2   
B) Kw =   
C) Kw =   
D) Kw =   
A) Kw = [H2O]2   
B) Kw =   
C) Kw =   
D) Kw =

Question 9

What is the pH of a peach with a [-OH] = 3.2 × 10-11 M -OH?

Accepted Answer

A) 11.32 
B) 10.49 
C) 3.51 
D) 3.2 
A) 11.32 
B) 10.49 
C) 3.51 
D) 3.2

Question 10

OH- and NH4+ are both examples of Brønsted-Lowry bases.

Accepted Answer

A) True 
 B)False

Question 11

The pH of a 1.0 × 10-5 M H3O+ solution is 5.00.

Accepted Answer

A) True 
 B)False

Question 12

The reactants are favored in the acid-base reaction: HF(aq)+ -OH(aq)   F-(aq)+ H2O(l).

Accepted Answer

A) True 
 B)False

Question 13

How many milliliters of 0.653 M NaOH are needed to neutralize 25.0 mL of a 1.02 M HBr solution? The neutralization reaction is: NaOH(aq)+ HBr(aq)$\rightarrow$ H2O(l)+ NaBr(aq)

Accepted Answer

A) 16.0 mL NaOH 
B) 25.5 mL NaOH 
C) 39.1 mL NaOH 
D) 16.3 mL NaOH 
A) 16.0 mL NaOH 
B) 25.5 mL NaOH 
C) 39.1 mL NaOH 
D) 16.3 mL NaOH

Question 14

What is the pH of a cleaning solution with a [H3O+] = 7.4 × 10-9 M H3O+?

Accepted Answer

A) 5.9 
B) 7.13 
C) 8.13 
D) 5.87 
A) 5.9 
B) 7.13 
C) 8.13 
D) 5.87

Question 15

The pH of a 1.0 × 10-6 M -OH solution is 6.00.

Accepted Answer

A) True 
 B)False

Question 16

The value of Kw = 1.0 × 10-14 at all temperatures below 100 °C.

Accepted Answer

A) True 
 B)False

Question 17

A compound that contains both a hydrogen atom and a lone pair of electrons can be either an acid or a base, depending on the particular reaction. Such a compound is said to be _____.

Accepted Answer

The answer of A compound that contains both a hydrogen...

Question 18

A solution in which [H3O+] = 7.4 × 10-5 M has a higher pH than a solution with a [-OH] = 4.8 × 10-8 M.

Accepted Answer

A) True 
 B)False

Question 19

The pH of a lime is 1.90. What is the [H3O+]?

Accepted Answer

A) 1.3 × 10-2 M H3O+ 
B) 1.3 × 1012 M H3O+ 
C) 7.9 × 101 M H3O+ 
D) 7.9 × 10-13 M H3O+ 
E) 1.9 M H3O+ 
A) 1.3 × 10-2 M H3O+ 
B) 1.3 × 1012 M H3O+ 
C) 7.9 × 101 M H3O+ 
D) 7.9 × 10-13 M H3O+ 
E) 1.9 M H3O+

Question 20

What are the products of the acid-base reaction of sodium carbonate with acetic acid?

Accepted Answer

A) CO2(g)+ H2O(l)+ 2 NaCH3COO(aq) 
B) 5 CO2(g)+ 2 H2O(l)+ 2 NaOH(aq) 
C) H2CO3(aq)+ H2O(l)+ 2 NaOH(aq) 
D) CO(g)+ H2O(l)+ 2 NaCH3COO(aq) 
A) CO2(g)+ H2O(l)+ 2 NaCH3COO(aq) 
B) 5 CO2(g)+ 2 H2O(l)+ 2 NaOH(aq) 
C) H2CO3(aq)+ H2O(l)+ 2 NaOH(aq) 
D) CO(g)+ H2O(l)+ 2 NaCH3COO(aq)

Exam 9: Acids and Bases

Which solution has the highest pH?

Which species is the conjugate base of NH3?

In a reversible acid-base reaction, equilibrium favors the formation of the acid with the smaller Ka value.

What is the balanced equation for the acid-base reaction of nitrous acid with lithium hydroxide?

In the acid-base reaction: F-(aq)+ HNO3(aq) HF(aq)+ NO3-(aq)

A solution in which [-OH] = 6.3 × 10-7 M has a higher pH than a solution with a [-OH] = 4.3 × 10-2 M.

What is the expression for Kw, the ion-product constant for water?

What is the pH of a peach with a [-OH] = 3.2 × 10-11 M -OH?

OH- and NH4+ are both examples of Brønsted-Lowry bases.

The pH of a 1.0 × 10-5 M H3O+ solution is 5.00.

The reactants are favored in the acid-base reaction: HF(aq)+ -OH(aq) F-(aq)+ H2O(l).

How many milliliters of 0.653 M NaOH are needed to neutralize 25.0 mL of a 1.02 M HBr solution? The neutralization reaction is: NaOH(aq)+ HBr(aq) →\rightarrow→ H2O(l)+ NaBr(aq)

What is the pH of a cleaning solution with a [H3O+] = 7.4 × 10-9 M H3O+?

The pH of a 1.0 × 10-6 M -OH solution is 6.00.

The value of Kw = 1.0 × 10-14 at all temperatures below 100 °C.

A compound that contains both a hydrogen atom and a lone pair of electrons can be either an acid or a base, depending on the particular reaction. Such a compound is said to be _____.

A solution in which [H3O+] = 7.4 × 10-5 M has a higher pH than a solution with a [-OH] = 4.8 × 10-8 M.

The pH of a lime is 1.90. What is the [H3O+]?

What are the products of the acid-base reaction of sodium carbonate with acetic acid?

Matter and Measurement

Atoms and the Periodic Table

Ionic Compounds

Covalent Compounds

Chemical Reactions

Energy Changes, Reaction Rates, and Equilibrium

Gases, Liquids, and Solids

Solutions

Nuclear Chemistry

Introduction to Organic Molecules and Functional Groups

Alkanes

Unsaturated Hydrocarbons

Organic Compounds That Contain Oxygen, Halogen, or Sulfur

The Three-Dimensional Shape of Molecules

Aldehydes and Ketones

Carboxylic Acids, Esters, and Amides

Amines and Neurotransmitters

Lipids

Carbohydrates

Amino Acids, Proteins, and Enzymes

Nucleic Acids and Protein Synthesis

Digestion and the Conversion of Food Into Energy

Carbohydrate, Lipid, and Protein Metabolism

Filters

Which species is the conjugate base of NH₃?

In a reversible acid-base reaction, equilibrium favors the formation of the acid with the smaller K_a value.

In the acid-base reaction: F^-(aq)+ HNO₃(aq) HF(aq)+ NO₃^-(aq)

A solution in which [^-OH] = 6.3 × 10^-7M has a higher pH than a solution with a [^-OH] = 4.3 × 10^-2M.

What is the expression for K_w, the ion-product constant for water?

What is the pH of a peach with a [^-OH] = 3.2 × 10^-11M ^-OH?

OH^- and NH₄⁺ are both examples of Brønsted-Lowry bases.

The pH of a 1.0 × 10^-5M H₃O⁺solution is 5.00.

The reactants are favored in the acid-base reaction: HF(aq)+ ^-OH(aq) F^-(aq)+ H₂O(l).

How many milliliters of 0.653 M NaOH are needed to neutralize 25.0 mL of a 1.02 M HBr solution? The neutralization reaction is: NaOH(aq)+ HBr(aq) $\rightarrow$ H₂O(l)+ NaBr(aq)

What is the pH of a cleaning solution with a [H₃O⁺] = 7.4 × 10^-9M H₃O⁺?

The pH of a 1.0 × 10^-6M ^-OHsolution is 6.00.

The value of K_w = 1.0 × 10^-14 at all temperatures below 100 °C.

A solution in which [H₃O⁺] = 7.4 × 10^-5M has a higher pH than a solution with a [^-OH] = 4.8 × 10^-8M.

The pH of a lime is 1.90. What is the [H₃O⁺]?