Question 1

Metabolic acidosis resulting from vigorous exercise is associated with increased production of which of the following?

Accepted Answer

A) citric acid 
B) formic acid 
C) lactic acid 
D) phosphoric acid 
A) citric acid 
B) formic acid 
C) lactic acid 
D) phosphoric acid

Question 2

Nitroaniline (C6H6N2O2) is a weak base. This would indicate that the pH of a 0.010 M solution of nitroaniline will be less than 7.

Accepted Answer

A) True 
 B)False

Question 3

Both the kidneys and the carbon dioxide-carbonic acid cycle help regulate blood pH.

Accepted Answer

A) True 
 B)False

Question 4

A solution is 0.10 M in ascorbic acid (Vitamin C), H2C6H6O6, and 0.10 M in sodium ascorbate, NaHC6H6O6. When base is added to the solution, H2C6H6O6 neutralizes the added base.

Accepted Answer

A) True 
 B)False

Question 5

Using the above table,fill in the blank with the appropriate integer (1 ,2,3,...)indicating the buffer and/or the letter indicating the formula below.
-In Buffer 2, the missing acid component is_______________________.

Accepted Answer

A) H3C2O4+ 
B) HC2O4- 
C) C3H4O32- 
D) HC3H5O3 
E) C2H3O2-
F)H2C2H3O2
G)C3H5O3- 
A) H3C2O4+ 
B) HC2O4- 
C) C3H4O32- 
D) HC3H5O3 
E) C2H3O2-
F)H2C2H3O2
G)C3H5O3-

Question 6

An aqueous solution contains a [H3O+] that is 1.0 × 10-3 M. What is the [OH-] of this solution?

Accepted Answer

A) 1.0 × 10-14 M 
B) 1.0 × 10-11 M 
C) 1.0 × 10-3 M 
D) 1.0 × 1011 M 
A) 1.0 × 10-14 M 
B) 1.0 × 10-11 M 
C) 1.0 × 10-3 M 
D) 1.0 × 1011 M

Question 7

The following solutions are ranked from the most acidic to the most basic.
Most acidic urine (pH 5.89) intestine contents (pH 8.06) blood (pH 7.30) Most basic

Accepted Answer

A) True 
 B)False

Question 8

Examine the structure given below   How many acidic hydrogen atoms are present? Enter a numerical value (1, 2, 3, ...).

Accepted Answer

The answer of Examine the structure given below  ...

Question 9

The following reaction represents the self-ionization of ammonia (NHS1U1B13S1U1B0).
NHS1U1B13S1U1B0(aq)+ NHS1U1B13S1U1B0(aq)   NHS1U1B12S1U1B0S1U1P1-S1S1P0(aq)+ NHS1U1B14S1U1B0S1U1P1+S1S1P0(aq)
amide ammonium
Fill in the blanks with the appropriate terms from those listed below.
ammonia
ammonium
amide
-In this reaction, the conjugate base of ammonia is the _______________________ ion.

Accepted Answer

The answer of The following reaction represents the self-ionization of...

Question 10

Which of the following is the conjugate base of H3PO4?

Accepted Answer

A) H2PO4- 
B) HPO42- 
C) PO43- 
D) OH- 
E) both H2PO4- and HPO42- 
A) H2PO4- 
B) HPO42- 
C) PO43- 
D) OH- 
E) both H2PO4- and HPO42-

Question 11

Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma?

Accepted Answer

A) causes an increase 
B) causes a decrease 
C) has no effect 
A) causes an increase 
B) causes a decrease 
C) has no effect

Question 12

Consider the following three buffer reactions.
Buffer 1: protein-HS1U1P1+S1S1P0 and protein
Buffer 2: HS1U1B12S1U1B0COS1U1B13S1U1B0 and HCOS1U1B13S1U1B0S1U1P1-S1S1P0
Buffer 3: HS1U1B12S1U1B0POS1U1B14S1U1B0S1U1P1-S1S1P0 and HPOS1U1B14S1U1B0S1U1P12-S1S1P0
Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described.
-Buffer______________________can have a variable pKa value.

Accepted Answer

Question 13

Below is the structure for the amino acid alanine.   Alanine can undergo an internal acid-base reaction.   In this reaction, the -NH2 group functions as a base.

Accepted Answer

A) True 
 B)False

Question 14

If you dissolve 0.10 mol of a generic acid HA in 1.0 L of solution, the pH is 3.5. Is HA a strong or weak acid? Explain your answer.

Accepted Answer

HA is a weak acid that is only partially

Question 15

When fumaric acid, H2C4H2O4 reacts with NaOH, the second reaction that occurs is

Accepted Answer

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

Question 16

An ammonia solution has a pH of 11.30, what is the H3O+ concentration in this solution?

Accepted Answer

A) 5.0 × 10-23 M 
B) 2.0 × 10-9 M 
C) 5.0 × 10-12 M 
D) 2.0 × 1011 M 
A) 5.0 × 10-23 M 
B) 2.0 × 10-9 M 
C) 5.0 × 10-12 M 
D) 2.0 × 1011 M

Question 17

The following reaction represents the self-ionization of ammonia (NHS1U1B13S1U1B0).
NHS1U1B13S1U1B0(aq)+ NHS1U1B13S1U1B0(aq)   NHS1U1B12S1U1B0S1U1P1-S1S1P0(aq)+ NHS1U1B14S1U1B0S1U1P1+S1S1P0(aq)
amide ammonium
Fill in the blanks with the appropriate terms from those listed below.
ammonia
ammonium
amide
-In the reverse reaction, __________________________ion functions as an acid.

Accepted Answer

The answer of The following reaction represents the self-ionization of...

Question 18

The pKa of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Accepted Answer

A) True 
 B)False

Question 19

Using the above table,fill in the blank with the appropriate integer (1 ,2,3,...)indicating the buffer and/or the letter indicating the formula below.
-In Buffer 2,_________________________ would react with added acid.

Accepted Answer

A) H3C2O4+ 
B) HC2O4- 
C) C3H4O32- 
D) HC3H5O3 
E) C2H3O2-
F)H2C2H3O2
G)C3H5O3- 
A) H3C2O4+ 
B) HC2O4- 
C) C3H4O32- 
D) HC3H5O3 
E) C2H3O2-
F)H2C2H3O2
G)C3H5O3-

Question 20

Which of the following is a polyprotic acid?

Accepted Answer

A) HCl 
B) HNO3 
C) H2SO4 
D) H3PO4 
E) both c and d 
A) HCl 
B) HNO3 
C) H2SO4 
D) H3PO4 
E) both c and d

Metabolic acidosis resulting from vigorous exercise is associated with increased production of which of the following?

Nitroaniline (C₆H₆N₂O₂) is a weak base. This would indicate that the pH of a 0.010 M solution of nitroaniline will be less than 7.

Both the kidneys and the carbon dioxide-carbonic acid cycle help regulate blood pH.

A solution is 0.10 M in ascorbic acid (Vitamin C), H₂C₆H₆O₆, and 0.10 M in sodium ascorbate, NaHC₆H₆O₆. When base is added to the solution, H₂C₆H₆O₆ neutralizes the added base.

Using the above table,fill in the blank with the appropriate integer (1 ,2,3,...)indicating the buffer and/or the letter indicating the formula below. -In Buffer 2, the missing acid component is_______________________.

An aqueous solution contains a [H₃O⁺] that is 1.0 × 10^-3 M. What is the [OH^-] of this solution?

The following solutions are ranked from the most acidic to the most basic. Most acidic urine (pH 5.89) intestine contents (pH 8.06) blood (pH 7.30) Most basic

Examine the structure given below How many acidic hydrogen atoms are present? Enter a numerical value (1, 2, 3, ...).

Which of the following is the conjugate base of H₃PO₄?

Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma?

Below is the structure for the amino acid alanine. Alanine can undergo an internal acid-base reaction. In this reaction, the -NH₂ group functions as a base.

If you dissolve 0.10 mol of a generic acid HA in 1.0 L of solution, the pH is 3.5. Is HA a strong or weak acid? Explain your answer.

When fumaric acid, H₂C₄H₂O₄ reacts with NaOH, the second reaction that occurs is

An ammonia solution has a pH of 11.30, what is the H₃O⁺ concentration in this solution?

The pK_a of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Using the above table,fill in the blank with the appropriate integer (1 ,2,3,...)indicating the buffer and/or the letter indicating the formula below. -In Buffer 2,_________________________ would react with added acid.

Which of the following is a polyprotic acid?

Measurements in Science and Medicine

Atoms, Elements, and Compounds

Chemical Bonds

Energy and Physical Properties

Solution Concentration

Chemical Reactions

Nuclear Chemistry

Hydrocarbons: An Introduction to Organic Molecules

Hydration, Dehydration, and Alcohols

Carbonyl Compounds and Redox Reactions

Organic Acids and Bases

Condensation and Hydrolysis Reactions

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Exam 7: Acids and Bases

Metabolic acidosis resulting from vigorous exercise is associated with increased production of which of the following?

Nitroaniline (C6H6N2O2) is a weak base. This would indicate that the pH of a 0.010 M solution of nitroaniline will be less than 7.

Both the kidneys and the carbon dioxide-carbonic acid cycle help regulate blood pH.

A solution is 0.10 M in ascorbic acid (Vitamin C), H2C6H6O6, and 0.10 M in sodium ascorbate, NaHC6H6O6. When base is added to the solution, H2C6H6O6 neutralizes the added base.

Using the above table,fill in the blank with the appropriate integer (1 ,2,3,...)indicating the buffer and/or the letter indicating the formula below. -In Buffer 2, the missing acid component is_______________________.

An aqueous solution contains a [H3O+] that is 1.0 × 10-3 M. What is the [OH-] of this solution?

The following solutions are ranked from the most acidic to the most basic. Most acidic urine (pH 5.89) intestine contents (pH 8.06) blood (pH 7.30) Most basic

Examine the structure given below How many acidic hydrogen atoms are present? Enter a numerical value (1, 2, 3, ...).

Which of the following is the conjugate base of H3PO4?

Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma?

Consider the following three buffer reactions. Buffer 1: protein-H+ and protein Buffer 2: H2CO3 and HCO3- Buffer 3: H2PO4- and HPO42- Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described. -Buffer______________________can have a variable pKa value.

Below is the structure for the amino acid alanine. Alanine can undergo an internal acid-base reaction. In this reaction, the -NH2 group functions as a base.

If you dissolve 0.10 mol of a generic acid HA in 1.0 L of solution, the pH is 3.5. Is HA a strong or weak acid? Explain your answer.

When fumaric acid, H2C4H2O4 reacts with NaOH, the second reaction that occurs is

An ammonia solution has a pH of 11.30, what is the H3O+ concentration in this solution?

The following reaction represents the self-ionization of ammonia (NH3). NH3(aq)+ NH3(aq) NH2-(aq)+ NH4+(aq) amide ammonium Fill in the blanks with the appropriate terms from those listed below. ammonia ammonium amide -In the reverse reaction, __________________________ion functions as an acid.

The pKa of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Using the above table,fill in the blank with the appropriate integer (1 ,2,3,...)indicating the buffer and/or the letter indicating the formula below. -In Buffer 2,_________________________ would react with added acid.

Which of the following is a polyprotic acid?

Measurements in Science and Medicine

Atoms, Elements, and Compounds

Chemical Bonds

Energy and Physical Properties

Solution Concentration

Chemical Reactions

Nuclear Chemistry

Hydrocarbons: An Introduction to Organic Molecules

Hydration, Dehydration, and Alcohols

Carbonyl Compounds and Redox Reactions

Organic Acids and Bases

Condensation and Hydrolysis Reactions

Proteins

Carbohydrates

Lipids and Membranes

Nucleic Acids, Protein Synthesis, and Heredity

Filters

Nitroaniline (C₆H₆N₂O₂) is a weak base. This would indicate that the pH of a 0.010 M solution of nitroaniline will be less than 7.

A solution is 0.10 M in ascorbic acid (Vitamin C), H₂C₆H₆O₆, and 0.10 M in sodium ascorbate, NaHC₆H₆O₆. When base is added to the solution, H₂C₆H₆O₆ neutralizes the added base.

An aqueous solution contains a [H₃O⁺] that is 1.0 × 10^-3 M. What is the [OH^-] of this solution?

Which of the following is the conjugate base of H₃PO₄?

Below is the structure for the amino acid alanine. Alanine can undergo an internal acid-base reaction. In this reaction, the -NH₂ group functions as a base.

When fumaric acid, H₂C₄H₂O₄ reacts with NaOH, the second reaction that occurs is

An ammonia solution has a pH of 11.30, what is the H₃O⁺ concentration in this solution?

The pK_a of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.