Question 1

How would an increase in hydrogen ions change the pH of blood?

Accepted Answer

A) Decrease it 
B) Increase it 
C) Would not change it 
A) Decrease it 
B) Increase it 
C) Would not change it

Question 2

The tendency for water molecules to stick or cling to another surface is called ________.

Accepted Answer

A) solubility 
B) adhesion 
C) cohesion 
D) reactivity 
A) solubility 
B) adhesion 
C) cohesion 
D) reactivity

Question 3

When added to an acidic solution, what color will Bromecresol purple buffer turn the solution?

Accepted Answer

A) Blue 
B) Yellow 
C) Purple 
D) Green 
A) Blue 
B) Yellow 
C) Purple 
D) Green

Question 4

Water molecules rely on ________ to hold them together.

Accepted Answer

A) ionic bonds 
B) hydrogen bonds 
C) polar covalent bonds 
D) nonpolar covalent bonds 
A) ionic bonds 
B) hydrogen bonds 
C) polar covalent bonds 
D) nonpolar covalent bonds

Question 5

A patient's blood pH has dropped from a normal of 7.4 to a low of 7.25. Describe the patient's blood pH.

Accepted Answer

A) The blood pH is now basic (alkaline) 
B) The blood pH is now acidotic. 
C) The blood has too little hydrogen ion. 
D) The blood pH is too high. 
A) The blood pH is now basic (alkaline) 
B) The blood pH is now acidotic. 
C) The blood has too little hydrogen ion. 
D) The blood pH is too high.

Question 6

What happens to blood hydrogen ion levels as carbon dioxide levels rise?

Accepted Answer

A) They go up. 
B) They go down. 
C) There is no change. 
A) They go up. 
B) They go down. 
C) There is no change.

Question 7

In general, when comparing the effectiveness of over-the-counter antacids to sodium bicarbonate, how effective was sodium bicarbonate at neutralizing the acidity?

Accepted Answer

A) It had no effect 
B) It was a lot more effective 
C) It was a lot less effective 
D) It had similar effectiveness 
A) It had no effect 
B) It was a lot more effective 
C) It was a lot less effective 
D) It had similar effectiveness

Question 8

What happens when an acid and a base are mixed?

Accepted Answer

A) They form salts and water. 
B) They release electrons and protons. 
C) They neutralize a solution. 
D) They buffer a solution. 
A) They form salts and water. 
B) They release electrons and protons. 
C) They neutralize a solution. 
D) They buffer a solution.

Question 9

Why is Bromecresol purple used when demonstrating the role of buffers?

Accepted Answer

A) It makes a solution more acidic. 
B) It stabilizes the pH of solution. 
C) It indicates if a solution has changed from an alkaline to an acidic pH. 
D) It reduces the acidity of a solution. 
A) It makes a solution more acidic. 
B) It stabilizes the pH of solution. 
C) It indicates if a solution has changed from an alkaline to an acidic pH. 
D) It reduces the acidity of a solution.

Question 10

Which solution is the most likely to have a pH of 3 or 4?

Accepted Answer

A) Baking soda 
B) Coffee 
C) Water 
D) Bleach 
A) Baking soda 
B) Coffee 
C) Water 
D) Bleach

Question 11

What tool would help you determine the hydrogen ion concentration of urine?

Accepted Answer

A) Deionized water 
B) Refractometer 
C) pH test strip 
D) Bromecresol purple 
A) Deionized water 
B) Refractometer 
C) pH test strip 
D) Bromecresol purple

Question 12

Glucose is a ________.

Accepted Answer

A) disaccharide 
B) monosaccharide 
C) polysaccharide 
D) polymer 
A) disaccharide 
B) monosaccharide 
C) polysaccharide 
D) polymer

Question 13

What does enzyme specificity mean?

Accepted Answer

A) Enzymes do not change or degrade after a reaction. 
B) An enzyme is able to speed up several different chemical reactions 
C) Enzymes can only bind to one type or shape of substrate . 
D) Enzymes require a specific temperature and pH for optimum activity 
A) Enzymes do not change or degrade after a reaction. 
B) An enzyme is able to speed up several different chemical reactions 
C) Enzymes can only bind to one type or shape of substrate . 
D) Enzymes require a specific temperature and pH for optimum activity

Question 14

Two hydrogen atoms share electrons equally between each other, forming a molecule. What type of bond is this?

Accepted Answer

A) Nonpolar covalent bond 
B) Ionic bond 
C) Hydrogen bond 
D) Polar covalent bond 
A) Nonpolar covalent bond 
B) Ionic bond 
C) Hydrogen bond 
D) Polar covalent bond

Question 15

Why does an increase in carbon dioxide increase the quantity of hydrogen ions in blood?

Accepted Answer

A) When carbon dioxides dissolves in water, it releases hydroxides. 
B) When carbon dioxide mixes with water, it loses two electrons. 
C) When carbon dioxide mixes with blood, it slows the transfers of hydrogen ions. 
D) When carbon dioxide is dissolved in water, it forms carbonic acid. 
A) When carbon dioxides dissolves in water, it releases hydroxides. 
B) When carbon dioxide mixes with water, it loses two electrons. 
C) When carbon dioxide mixes with blood, it slows the transfers of hydrogen ions. 
D) When carbon dioxide is dissolved in water, it forms carbonic acid.

Question 16

Where does an enzyme bind to a substrate?

Accepted Answer

A) Acid monomer receptor 
B) Active site 
C) Distal edge 
D) Receptor site 
A) Acid monomer receptor 
B) Active site 
C) Distal edge 
D) Receptor site

Question 17

The pH scale ________.

Accepted Answer

A) measures the hydrogen ion concentration of a solution 
B) defines neutral as a pH of 5 
C) ranges from 1 to 7 
D) measures the salt concentration of a solution 
A) measures the hydrogen ion concentration of a solution 
B) defines neutral as a pH of 5 
C) ranges from 1 to 7 
D) measures the salt concentration of a solution

Question 18

A buffer is ________.

Accepted Answer

A) a substance that stabilizes pH 
B) a protein that catalyzes a faster chemical reaction 
C) a string of multiple peptides 
D) a molecule that hydrolyzes sugar molecules 
A) a substance that stabilizes pH 
B) a protein that catalyzes a faster chemical reaction 
C) a string of multiple peptides 
D) a molecule that hydrolyzes sugar molecules

Question 19

Two water molecules are weakly attracted to each other when a slightly positive hydrogen atom in the first molecule is attracted to the slightly negative oxygen atom on the second molecule. What type of bond is this?

Accepted Answer

A) Ionic 
B) Polar covalent 
C) Nonpolar covalent 
D) Hydrogen bond 
A) Ionic 
B) Polar covalent 
C) Nonpolar covalent 
D) Hydrogen bond

Question 20

Which pH value is the most acidic?

Accepted Answer

A) 5 
B) 7 
C) 12 
D) 2 
A) 5 
B) 7 
C) 12 
D) 2

Exam 3: Chemistry

How would an increase in hydrogen ions change the pH of blood?

The tendency for water molecules to stick or cling to another surface is called ________.

When added to an acidic solution, what color will Bromecresol purple buffer turn the solution?

Water molecules rely on ________ to hold them together.

A patient's blood pH has dropped from a normal of 7.4 to a low of 7.25. Describe the patient's blood pH.

What happens to blood hydrogen ion levels as carbon dioxide levels rise?

In general, when comparing the effectiveness of over-the-counter antacids to sodium bicarbonate, how effective was sodium bicarbonate at neutralizing the acidity?

What happens when an acid and a base are mixed?

Why is Bromecresol purple used when demonstrating the role of buffers?

Which solution is the most likely to have a pH of 3 or 4?

What tool would help you determine the hydrogen ion concentration of urine?

Glucose is a ________.

What does enzyme specificity mean?

Two hydrogen atoms share electrons equally between each other, forming a molecule. What type of bond is this?

Why does an increase in carbon dioxide increase the quantity of hydrogen ions in blood?

Where does an enzyme bind to a substrate?

The pH scale ________.

A buffer is ________.

Two water molecules are weakly attracted to each other when a slightly positive hydrogen atom in the first molecule is attracted to the slightly negative oxygen atom on the second molecule. What type of bond is this?

Which pH value is the most acidic?

Introduction to Anatomy and Physiology

Introduction to the Organ Systems

The Microscope

The Cell

Histology

The Integumentary System

Introduction to the Skeletal System

The Axial Skeleton

The Appendicular Skeleton

Joints

Introduction to the Muscular System: Muscle Tissue

Gross Anatomy of the Muscular System

Introduction to the Nervous System

The Central Nervous System: Brain and Spinal Cord

The Peripheral Nervous System: Nerves and Autonomic Nervous System

General and Special Senses

The Endocrine System

Blood

Anatomy of the Heart

Physiology of the Heart

Anatomy of Blood Vessels

Circulatory Pathways and the Physiology of Blood Vessels

The Lymphatic System

Anatomy of the Respiratory System

Physiology of the Respiratory System

Anatomy of the Digestive System

Physiology of the Digestive System

Anatomy of the Urinary System

Physiology of the Urinary System

Reproductive and Development

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