Question 1

The pH of natural rainwater is 5.6 due to the carbon dioxide in the atmosphere.

Accepted Answer

A) True 
 B)False

Question 2

What is the pH of an aqueous solution that has a hydrogen-ion concentration of 4.83 × 10-9 mol/L?

Accepted Answer

Question 3

Which of the following qualifies as a Bronsted-Lowry acid?

Accepted Answer

A) KOH 
B) NH3 
C) Na+ 
D) NH4+ 
A) KOH 
B) NH3 
C) Na+ 
D) NH4+

Question 4

H2PO4- is the conjugate acid of PO42-.

Accepted Answer

A) True 
 B)False

Question 5

Which of the following is a weak electrolyte when dissolved in distilled water?

Accepted Answer

A) phosphoric acid 
B) nitric acid 
C) potassium chloride 
D) glucose 
A) phosphoric acid 
B) nitric acid 
C) potassium chloride 
D) glucose

Question 6

Which of the following is the weakest acid?

Accepted Answer

A) acetic acid, Ka = 1.8 × 10-5 
B) nitrous acid, Ka = 4.5 × 10-4 
C) hydrogen peroxide, Ka = 2.4 × 10-12 
D) hypochlorous acid, Ka = 3.5 × 10-8 
A) acetic acid, Ka = 1.8 × 10-5 
B) nitrous acid, Ka = 4.5 × 10-4 
C) hydrogen peroxide, Ka = 2.4 × 10-12 
D) hypochlorous acid, Ka = 3.5 × 10-8

Question 7

A saline solution will not conduct an electric current.

Accepted Answer

A) True 
 B)False

Question 8

The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving as a strong acid in water?

Accepted Answer

A) 
  
B) 
  
C) 
  
D) 
  
A) 
  
B) 
  
C) 
  
D)

Question 9

Match between columns
                        Premises: carbonic
sulfurous
phosphoric
acetic
hydrobromic
hypochlorous
sulfuric
nitric

Accepted Answer

The Answer of strong acid and weak acid is...

Question 10

Which of the following qualifies as a Bronsted-Lowry base?

Accepted Answer

A) CH4 
B) NH3 
C) SiH4 
D) H2 
A) CH4 
B) NH3 
C) SiH4 
D) H2

Question 11

The hydrogen-ion concentration of a solution of pOH 10.5 is 3.16 × 10-4 mol/L (remember that pH + pOH = 14 for aqueous systems).

Accepted Answer

A) True 
 B)False

Question 12

Basic solutions ________.

Accepted Answer

A) have a higher concentration of hydronium ions than hydroxide ions 
B) have a lower concentration of hydronium ions than hydroxide ions 
C) turn blue litmus paper to pink 
D) decolorize phenolphthalein solutions 
A) have a higher concentration of hydronium ions than hydroxide ions 
B) have a lower concentration of hydronium ions than hydroxide ions 
C) turn blue litmus paper to pink 
D) decolorize phenolphthalein solutions

Question 13

Which of the following is the strongest acid?

Accepted Answer

A) acetic acid, Ka = 1.8 × 10-5 
B) nitrous acid, Ka = 4.5 × 10-4 
C) hydrogen peroxide, Ka = 2.4 × 10-12 
D) hypochlorous acid, Ka = 3.5 × 10-8 
A) acetic acid, Ka = 1.8 × 10-5 
B) nitrous acid, Ka = 4.5 × 10-4 
C) hydrogen peroxide, Ka = 2.4 × 10-12 
D) hypochlorous acid, Ka = 3.5 × 10-8

Question 14

When ammonia is dissolved in water, the ionized species are ________.

Accepted Answer

A) NH4+ and OH- 
B) NH2- and H+ 
C) NH4+ and H- 
D) NH2+ and H- 
A) NH4+ and OH- 
B) NH2- and H+ 
C) NH4+ and H- 
D) NH2+ and H-

Question 15

Aqueous salt solution is a strong electrolyte.

Accepted Answer

A) True 
 B)False

Question 16

Which of the following is a strong acid?

Accepted Answer

A) acetic acid 
B) hydrofluoric acid 
C) phosphoric acid 
D) hydrochloric acid 
A) acetic acid 
B) hydrofluoric acid 
C) phosphoric acid 
D) hydrochloric acid

Question 17

Which of the following is the weakest base?

Accepted Answer

A) ammonia, Kb = 1.7 × 10-5 
B) aniline, Kb = 4.2 × 10-10 
C) trimethylamine, Kb = 7.4 × 10-5 
D) methylamine, Kb = 4.4 × 10-4 
A) ammonia, Kb = 1.7 × 10-5 
B) aniline, Kb = 4.2 × 10-10 
C) trimethylamine, Kb = 7.4 × 10-5 
D) methylamine, Kb = 4.4 × 10-4

Question 18

Approximately one out of every 555 million water molecules autoionize.

Accepted Answer

A) True 
 B)False

Question 19

Match between columns
                        Premises: pure water
aqueous rubbing alcohol
sports drink
seawater
tap water
aqueous hydrochloric acid solution
aqueous sucrose solution
solid sodium chloride
aqueous salt solution
gasoline
aqueous baking soda solution
aqueous sulfuric acid solution

Accepted Answer

The Answer of electrolyte and non-electrolyte is...

Question 20

The stomach is very sensitive to changes in pH (particularly highly acidic conditions). Suggest why aspirin, acetylsalicylic acid, causes stomach upset. What is the purpose of so-called buffered aspirin tablets?

Accepted Answer

Taking aspirin automatically lowers pH i

The pH of natural rainwater is 5.6 due to the carbon dioxide in the atmosphere.

What is the pH of an aqueous solution that has a hydrogen-ion concentration of 4.83 × 10^-⁹ mol/L?

Which of the following qualifies as a Bronsted-Lowry acid?

H₂PO₄^-is the conjugate acid of PO₄²^-.

Which of the following is a weak electrolyte when dissolved in distilled water?

Which of the following is the weakest acid?

A saline solution will not conduct an electric current.

The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving as a strong acid in water?

Which of the following qualifies as a Bronsted-Lowry base?

The hydrogen-ion concentration of a solution of pOH 10.5 is 3.16 × 10^-4 mol/L (remember that pH + pOH = 14 for aqueous systems).

Basic solutions ________.

Which of the following is the strongest acid?

When ammonia is dissolved in water, the ionized species are ________.

Aqueous salt solution is a strong electrolyte.

Which of the following is a strong acid?

Which of the following is the weakest base?

Approximately one out of every 555 million water molecules autoionize.

The stomach is very sensitive to changes in pH (particularly highly acidic conditions). Suggest why aspirin, acetylsalicylic acid, causes stomach upset. What is the purpose of so-called buffered aspirin tablets?

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Intermolecular Forces and the Phases of Matter

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces the Ideal Gas

Solutions

When Reactants Turn Into Products

Chemical Equilibrium

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

Exam 15: Electrolytes, Acids, and Bases

The pH of natural rainwater is 5.6 due to the carbon dioxide in the atmosphere.

What is the pH of an aqueous solution that has a hydrogen-ion concentration of 4.83 × 10-9 mol/L?

Which of the following qualifies as a Bronsted-Lowry acid?

H2PO4- is the conjugate acid of PO42-.

Which of the following is a weak electrolyte when dissolved in distilled water?

Which of the following is the weakest acid?

A saline solution will not conduct an electric current.

The compound HA is an acid that is soluble in water. Which of the "beakers" below shows HA behaving as a strong acid in water?

Which of the following qualifies as a Bronsted-Lowry base?

The hydrogen-ion concentration of a solution of pOH 10.5 is 3.16 × 10-4 mol/L (remember that pH + pOH = 14 for aqueous systems).

Basic solutions ________.

Which of the following is the strongest acid?

When ammonia is dissolved in water, the ionized species are ________.

Aqueous salt solution is a strong electrolyte.

Which of the following is a strong acid?

Which of the following is the weakest base?

Approximately one out of every 555 million water molecules autoionize.

The stomach is very sensitive to changes in pH (particularly highly acidic conditions). Suggest why aspirin, acetylsalicylic acid, causes stomach upset. What is the purpose of so-called buffered aspirin tablets?

What Is Chemistry

The Numerical Side of Chemistry

The Evolution of Atomic Theory

The Modern Model of the Atom

Chemical Bonding and Nomenclature

The Shape of Molecules

Intermolecular Forces and the Phases of Matter

Chemical Reactions

Stoichiometry and the Mole

Electron Transfer in Chemical Reactions

What If There Were No Intermolecular Forces the Ideal Gas

Solutions

When Reactants Turn Into Products

Chemical Equilibrium

Nuclear Chemistry

The Chemistry of Carbon

Synthetic and Biological Polymers

Filters

What is the pH of an aqueous solution that has a hydrogen-ion concentration of 4.83 × 10^-⁹ mol/L?

H₂PO₄^-is the conjugate acid of PO₄²^-.

The hydrogen-ion concentration of a solution of pOH 10.5 is 3.16 × 10^-4 mol/L (remember that pH + pOH = 14 for aqueous systems).