Question 1

Sucrose (table sugar)is a strong electrolyte.

Accepted Answer

A) True 
 B)False

Question 2

Which is a weak acid?

Accepted Answer

A) sulfuric 
B) hydrochloric 
C) nitric 
D) carbonic 
A) sulfuric 
B) hydrochloric 
C) nitric 
D) carbonic

Question 3

Which of the following produces more than one H3O+ ion per molecule of acid when dissolved in water?

Accepted Answer

A) hydrobromic 
B) carbonic 
C) hypochlorous 
D) acetic 
A) hydrobromic 
B) carbonic 
C) hypochlorous 
D) acetic

Question 4

Which is the most acidic solution?

Accepted Answer

A) a solution whose [H+] = 10-1 
B) a solution whose [OH-] = 10-10 
C) a solution whose pH = 0 
D) All of the above have the same degree of acidity. 
A) a solution whose [H+] = 10-1 
B) a solution whose [OH-] = 10-10 
C) a solution whose pH = 0 
D) All of the above have the same degree of acidity.

Question 5

Which substance is the most acidic?

Accepted Answer

A) coffee 
B) milk 
C) oven cleaner 
D) baking soda 
A) coffee 
B) milk 
C) oven cleaner 
D) baking soda

Question 6

Arrhenius' definition of a base is an electrolyte that contains a metal and hydroxide ions that ionize when placed in water.

Accepted Answer

A) True 
 B)False

Question 7

Which of the following is a diprotic acid when dissolved in water?

Accepted Answer

A) hydrobromic 
B) sulfuric 
C) hypochlorous 
D) phosphoric 
A) hydrobromic 
B) sulfuric 
C) hypochlorous 
D) phosphoric

Question 8

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

Accepted Answer

A) sodium chloride 
B) hydrochloric acid 
C) sodium hydroxide 
D) ethyl alcohol 
A) sodium chloride 
B) hydrochloric acid 
C) sodium hydroxide 
D) ethyl alcohol

Question 9

Acidic 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 red litmus paper to blue 
D) colorize 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 red litmus paper to blue 
D) colorize phenolphthalein solutions

Question 10

Which of the following is not a weak electrolyte when dissolved in distilled water?

Accepted Answer

A) ammonia 
B) acetic acid (vinegar) 
C) potassium chloride 
D) hydrogen fluoride 
A) ammonia 
B) acetic acid (vinegar) 
C) potassium chloride 
D) hydrogen fluoride

Question 11

Which is a strong base?

Accepted Answer

A) potassium hydroxide 
B) ammonium hydroxide 
C) aluminum hydroxide 
D) fluoride ion 
A) potassium hydroxide 
B) ammonium hydroxide 
C) aluminum hydroxide 
D) fluoride ion

Question 12

What is the hydrogen-ion concentration of an aqueous solution having a pH of 4.72?

Accepted Answer

A) 4.7 × 10-5 mol/L 
B) 4.7 mol/L 
C) 0.67 mol/L 
D) 1.9 × 10-5 mol/L 
A) 4.7 × 10-5 mol/L 
B) 4.7 mol/L 
C) 0.67 mol/L 
D) 1.9 × 10-5 mol/L

Question 13

Which of the following could be considered an Arrhenius base?

Accepted Answer

A) HCl 
B) CH3COOH 
C) KOH 
D) HF 
A) HCl 
B) CH3COOH 
C) KOH 
D) HF

Question 14

A change in pH from 10 to 7 ________.

Accepted Answer

A) increases the acidity 1000× 
B) reduces the acidity 3000× 
C) increases the acidity 3× 
D) increases the acidity 3000× 
A) increases the acidity 1000× 
B) reduces the acidity 3000× 
C) increases the acidity 3× 
D) increases the acidity 3000×

Question 15

The conjugate base of HCO3- is ________.

Accepted Answer

A) H2CO3 
B) CO3-2 
C) CO2-2 
D) H3CO3+ 
A) H2CO3 
B) CO3-2 
C) CO2-2 
D) H3CO3+

Question 16

What is the hydroxide-ion concentration of an aqueous solution having a hydrogen-ion concentration of 4.75 × 10-5 mol/L?

Accepted Answer

A) 2.10 × 10-10 mol/L 
B) 5.25 × 10-10 mol/L 
C) 4.75 × 10-5 mol/L 
D) -4.75 × 10-5 mol/L 
A) 2.10 × 10-10 mol/L 
B) 5.25 × 10-10 mol/L 
C) 4.75 × 10-5 mol/L 
D) -4.75 × 10-5 mol/L

Question 17

Which of the following solutions would you expect not to conduct electricity?

Accepted Answer

A) NaCl in water 
B) CO in water 
C) HCl in water 
D) H2SO4 in water 
A) NaCl in water 
B) CO in water 
C) HCl in water 
D) H2SO4 in water

Question 18

The compound HCl is considered a Bronsted-Lowry base because it increases the concentration of H3O+ when it dissociates in water.

Accepted Answer

A) True 
 B)False

Question 19

What were the defining characteristics of bases as known to the alchemists?

Accepted Answer

1)a bitter taste
2)turned litm

Question 20

What is the hydroxide-ion concentration of an aqueous solution having a pH of 4.72?

Accepted Answer

A) 4.7 × 10-5 mol/L 
B) 1.9 × 10-14 mol/L 
C) 5.3 × 10-10 mol/L 
D) 1.9 × 10-5 mol/L 
A) 4.7 × 10-5 mol/L 
B) 1.9 × 10-14 mol/L 
C) 5.3 × 10-10 mol/L 
D) 1.9 × 10-5 mol/L

Sucrose (table sugar)is a strong electrolyte.

Which is a weak acid?

Which of the following produces more than one H₃O⁺ ion per molecule of acid when dissolved in water?

Which is the most acidic solution?

Which substance is the most acidic?

Arrhenius' definition of a base is an electrolyte that contains a metal and hydroxide ions that ionize when placed in water.

Which of the following is a diprotic acid when dissolved in water?

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

Acidic solutions ________.

Which of the following is not a weak electrolyte when dissolved in distilled water?

Which is a strong base?

What is the hydrogen-ion concentration of an aqueous solution having a pH of 4.72?

Which of the following could be considered an Arrhenius base?

A change in pH from 10 to 7 ________.

The conjugate base of HCO₃^- is ________.

What is the hydroxide-ion concentration of an aqueous solution having a hydrogen-ion concentration of 4.75 × 10^-5 mol/L?

Which of the following solutions would you expect not to conduct electricity?

The compound HCl is considered a Bronsted-Lowry base because it increases the concentration of H₃O⁺ when it dissociates in water.

What were the defining characteristics of bases as known to the alchemists?

What is the hydroxide-ion concentration of an aqueous solution having a pH of 4.72?

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

Sucrose (table sugar)is a strong electrolyte.

Which is a weak acid?

Which of the following produces more than one H3O+ ion per molecule of acid when dissolved in water?

Which is the most acidic solution?

Which substance is the most acidic?

Arrhenius' definition of a base is an electrolyte that contains a metal and hydroxide ions that ionize when placed in water.

Which of the following is a diprotic acid when dissolved in water?

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

Acidic solutions ________.

Which of the following is not a weak electrolyte when dissolved in distilled water?

Which is a strong base?

What is the hydrogen-ion concentration of an aqueous solution having a pH of 4.72?

Which of the following could be considered an Arrhenius base?

A change in pH from 10 to 7 ________.

The conjugate base of HCO3- is ________.

What is the hydroxide-ion concentration of an aqueous solution having a hydrogen-ion concentration of 4.75 × 10-5 mol/L?

Which of the following solutions would you expect not to conduct electricity?

The compound HCl is considered a Bronsted-Lowry base because it increases the concentration of H3O+ when it dissociates in water.

What were the defining characteristics of bases as known to the alchemists?

What is the hydroxide-ion concentration of an aqueous solution having a pH of 4.72?

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

Which of the following produces more than one H₃O⁺ ion per molecule of acid when dissolved in water?

The conjugate base of HCO₃^- is ________.

What is the hydroxide-ion concentration of an aqueous solution having a hydrogen-ion concentration of 4.75 × 10^-5 mol/L?

The compound HCl is considered a Bronsted-Lowry base because it increases the concentration of H₃O⁺ when it dissociates in water.