Question 1

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

Accepted Answer

A)    
B)    
C)    
D)  Both A and C are weak acids in water. 
A)    
B)    
C)    
D)  Both A and C are weak acids in water.

Question 2

Identify each [H?O+] / [OH-] / pH / pOH  as acidic or basic.
-pOH = 9.1

Accepted Answer

A) Basic 
B) Acidic 
A) Basic 
B) Acidic

Question 3

Milk is slightly basic.

Accepted Answer

A) True 
 B)False

Question 4

A drop of a full unit in the pH scale ________.

Accepted Answer

A)  reduces the acidity 10× 
B)  increases the acidity 10× 
C)  reduces the acidity 2× 
D)  increases the acidity 2× 
A)  reduces the acidity 10× 
B)  increases the acidity 10× 
C)  reduces the acidity 2× 
D)  increases the acidity 2×

Question 5

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

Question 6

Identify each of the substances as an electrolyte or non-electrolyte.
-aqueous rubbing alcohol

Accepted Answer

A) non-electrolyte 
B) electrolyte 
A) non-electrolyte 
B) electrolyte

Question 7

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

Accepted Answer

A)  sodium chloride 
B)  sucrose 
C)  acetone (nail polish remover) 
D)  ethyl alcohol 
A)  sodium chloride 
B)  sucrose 
C)  acetone (nail polish remover) 
D)  ethyl alcohol

Question 8

Match each of the acids with the maximum number of H?O+ produced per molecule of acid.
-hypochlorous acid

Accepted Answer

A) 3 
B) 1 
C) 2 
A) 3 
B) 1 
C) 2

Question 9

Which of the following acids can produce only one H₃O+ ion per molecule of acid when dissolved in water, although itself has other non-ionizable hydrogens?

Accepted Answer

A)  hydrobromic acid 
B)  sulfurous acid 
C)  hypochlorous acid 
D)  acetic acid 
A)  hydrobromic acid 
B)  sulfurous acid 
C)  hypochlorous acid 
D)  acetic acid

Question 10

Match each substance with its corresponding fact.
-SO?2-

Accepted Answer

A) It is the conjugate base of CH?CO?H. 
B) It does not have a conjugate base. 
C) It is the conjugate acid of HCO?-. 
D) Its conjugate acid is HSO?-. 
E) Its conjugate base is CO?2-.
F)Its conjugate base is HSO?-. 
A) It is the conjugate base of CH?CO?H. 
B) It does not have a conjugate base. 
C) It is the conjugate acid of HCO?-. 
D) Its conjugate acid is HSO?-. 
E) Its conjugate base is CO?2-.
F)Its conjugate base is HSO?-.

Question 11

PH₃ cannot serve as a Bronsted-Lowry base.

Accepted Answer

A) True 
 B)False

Question 12

Stomach juices have a pH close to ________.

Accepted Answer

A)  1.5 
B)  2.8 
C)  4.5 
D)  7.0 
A)  1.5 
B)  2.8 
C)  4.5 
D)  7.0

Question 13

HPO₄2- is the conjugate base of H₂PO₄-.

Accepted Answer

A) True 
 B)False

Question 14

Identify each of the substances as an electrolyte or non-electrolyte.
-aqueous sodium chloride solution

Accepted Answer

A) non-electrolyte 
B) electrolyte 
A) non-electrolyte 
B) electrolyte

Question 15

Identify each of the substances as an electrolyte or non-electrolyte.
-aqueous hydrochloric acid solution

Accepted Answer

A) non-electrolyte 
B) electrolyte 
A) non-electrolyte 
B) electrolyte

Question 16

Sucrose (table sugar) is a strong electrolyte.

Accepted Answer

A) True 
 B)False

Question 17

Identify each of the substances as an electrolyte or non-electrolyte.
-aqueous baking soda solution

Accepted Answer

A) non-electrolyte 
B) electrolyte 
A) non-electrolyte 
B) electrolyte

Question 18

Identify each of the substances as an electrolyte or non-electrolyte.
-seawater

Accepted Answer

A) non-electrolyte 
B) electrolyte 
A) non-electrolyte 
B) electrolyte

Question 19

Identify each of the acids as a strong acid or a weak acid.
-phosphoric acid

Accepted Answer

A) weak acid 
B) strong acid 
A) weak acid 
B) strong acid

Question 20

The pH of blood is approximately ________.

Accepted Answer

A)  5.2 
B)  7.0 
C)  7.4 
D)  9.1 
A)  5.2 
B)  7.0 
C)  7.4 
D)  9.1

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

Identify each [H?O+] / [OH-] / pH / pOH as acidic or basic. -pOH = 9.1

Milk is slightly basic.

A drop of a full unit in the pH scale ________.

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?

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous rubbing alcohol

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

Match each of the acids with the maximum number of H?O+ produced per molecule of acid. -hypochlorous acid

Which of the following acids can produce only one H₃O+ ion per molecule of acid when dissolved in water, although itself has other non-ionizable hydrogens?

Match each substance with its corresponding fact. -SO?2-

PH₃ cannot serve as a Bronsted-Lowry base.

Stomach juices have a pH close to ________.

HPO₄2- is the conjugate base of H₂PO₄-.

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous sodium chloride solution

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous hydrochloric acid solution

Sucrose (table sugar) is a strong electrolyte.

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous baking soda solution

Identify each of the substances as an electrolyte or non-electrolyte. -seawater

Identify each of the acids as a strong acid or a weak acid. -phosphoric acid

The pH of blood is approximately ________.

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

Identify each [H?O+] / [OH-] / pH / pOH as acidic or basic. -pOH = 9.1

Milk is slightly basic.

A drop of a full unit in the pH scale ________.

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?

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous rubbing alcohol

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

Match each of the acids with the maximum number of H?O+ produced per molecule of acid. -hypochlorous acid

Which of the following acids can produce only one H₃O+ ion per molecule of acid when dissolved in water, although itself has other non-ionizable hydrogens?

Match each substance with its corresponding fact. -SO?2-

PH₃ cannot serve as a Bronsted-Lowry base.

Stomach juices have a pH close to ________.

HPO₄2- is the conjugate base of H₂PO₄-.

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous sodium chloride solution

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous hydrochloric acid solution

Sucrose (table sugar) is a strong electrolyte.

Identify each of the substances as an electrolyte or non-electrolyte. -aqueous baking soda solution

Identify each of the substances as an electrolyte or non-electrolyte. -seawater

Identify each of the acids as a strong acid or a weak acid. -phosphoric acid

The pH of blood is approximately ________.

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