Deck 7: Acids and Bases

Question 1

The following represents the structure of a hydronium ion.

Answer 1

True

Question 2

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.

Answer 2

False

Question 3

The following is an accurate description of the ionization of HBr in water.

Answer 3

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.

Question 5

Consider the following reaction.
CH₃OH(l) + CH₃OH(l) CH₃O^-(l) + CH₃OH₂⁺(l)
This reaction could be classified as both an autoionization reaction and a proton transfer reaction.

Question 6

A solution composed of HCl and NaCl would produce an effective buffer.

Question 7

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

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

Question 8

For a healthy individual, the pH of the blood in the veins is lower than in the arteries.

Question 9

Which of the following is present in pure water?

A)H₃O⁺
B)OH−
C)H₂O
D)All are present in pure water.

Question 10

The range of breaths per minute, also known as respiratory rate, for a normal, healthy adult is 12-20 breaths per minute. A breathing rate of higher than this is termed hyperventilation.

Question 11

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

Question 12

Adipic acid has the formula given below. This is a polyprotic acid.

Question 13

The molar concentration of H₃O⁺ in an aqueous solution would be increased by the addition of KOH.

Question 14

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

Question 15

In converting from the pH of a solution to the corresponding H₃O⁺ concentration, the following equation should be used.
[H₃O⁺] = 10^-pH

Question 16

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.

Question 17

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.

Question 18

Very rapid breathing can lead to a condition know as respiratory acidosis.

Question 19

H⁺, H₃O⁺, and OH⁺ are different ways of representing the species that causes a solution to be acidic.

Question 20

Adipic acid has the formula given below. Thus substance would be classified as amphiprotic.

Question 21

Which of the following is the conjugate acid of ammonia, NH₃?

A)H⁺
B)H₃O⁺
C)NH₂-
D)NH₄⁺

Question 22

Which of the following solutions can function as a buffer?

A)a solution containing HC₂H₃O₂ and NaC₂H₃O₂
B)a solution containing H₂CO₃ and NaHCO₃
C)a solution containing NH₃ and NH₄Cl
D)all of the above

Question 23

Ascorbic acid (Vitamin C), H₂C₆H₆O₆, has a pK_a of 4.10. A solution is 0.10 M in ascorbic acid and 0.20 M in sodium ascorbate, NaHC₆H₆O₆. What is the approximate pH of the solution?

A)4.10
B)slightly less than 4.10
C)slightly more than 4.10
D)The solution will have a pH of exactly 7.

Question 24

When a solution of HF (a weak acid) is added to a solution containing HPO₄^2- (here, a base), the equation for reaction that occurs is:

A)
B)
C)
D)

Question 25

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

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

Question 26

Consider the following reaction.
+ H₂O HN₃ + OH−
This reaction indicates that:

A) is a weak base.
B) is a strong base.
C) is a weak acid.
D) is a strong acid.

Question 27

Which of the following pH's corresponds to a highly acidic solution?

A)2.1
B)6.8
C)7.2
D)11.2

Question 28

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

A)
B)
C)
D)

Question 29

A sodium hydroxide solution has a pH of 12.40, what is the OH^- concentration in this solution?

A)4.0 × 10¹ M
B)4.0 × 10^-13 M
C)2.5 × 10^{- 2} M
D)2.5 × 10¹² M

Question 30

Which of the following is the conjugate base of H₃PO₄?

A)H₂PO₄^-
B)HPO₄^2-
C)PO₄^3-
D)OH^-
E)both H₂PO₄^- and HPO₄^2-

Question 31

Oxalic acid (H₂C₂O₄) is weak acid found in the leaves of rhubarb. Which of the following solutions will have the highest pH?

A)1.0 M H₂C₂O₄
B)0.5 M H₂C₂O₄
C)1.0 × 10^-4 M H₂C₂O₄
D)0.00075 M H₂C₂O₄

Question 32

Which of the following substances is amphiprotic?

A)HCO₃^-
B)HPO₄^3-
C)H₂PO₄^-
D)All are amphiprotic.

Question 33

In an aqueous solution. the [OH^-] is 2.0 × 10^-3 M. What is the [H₃O⁺] of this solution?

A)5.0 × 10^-12 M
B)2.0 × 10¹¹ M
C)2.0 × 10^-3 M
D)5.0 × 10¹² M

Question 34

Which of the following statements best describes the relationship between conjugate acids and bases?

A)As acid strength increases, the conjugate base strength increases.
B)As base strength increases, the conjugate acid strength decreases.
C)The conjugate base of a strong acid is always strong.
D)There is no specific correlation.

Question 35

A buffer is composed of ammonia (NH₃) and ammonium chloride (NH₄Cl). When base is added to the buffer, which of the following reactions occurs?

A)
B)
C)
D)

Question 36

Which of the following is a polyprotic acid?

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

Question 37

The chemical equation for the reaction of the base, ethoxide, CH₃CH₂O^-, with water would show the products:

A)CH₃CH₂OH and OH^-
B)CH₃CH₃ and H₃O⁺
C)CH₃CH₂OH and H₃O⁺
D)CH₃CH₃ and OH^-

Question 38

Which of the following is characteristic of a buffer?

A)The pH will go down significantly when H₃O⁺ is added to the buffer.
B)The pH will go down very slightly when H₃O⁺ is added to a buffer.
C)The pH will go up significantly when H₃O⁺ is added to the buffer.
D)The pH will go up very slightly when H₃O⁺ is added to the buffer.

Question 39

All of the following solutions are 0.025 M, which of the solutions contains the highest concentration of OH^-?

A)acetic acid (pH 3.17)
B)ascorbic acid (pH 6.70)
C)phenol (pH 5.73)
D)iodic acid (pH 1.60)

Question 40

A water solution is found to have an OH^- concentration of 6.3 × 10−¹⁰. The solution would be classified as:

A)acidic.
B)basic.
C)neutral.

Question 41

Consider the image which depicts the reaction between CH₃COOH and H₂O. Reactants:
Products:

If the composition of the equilibrium mixture is as represented below
CH₃COOH is classified as

A)strong electrolyte
B)weak electrolyte
C)nonelectrolyte

Question 42

Which of the following substances can react with both HCl and NaOH?.

A)Ca(HCO₃)₂
B)KCl
C)CH₃CH₂NH₂
D)H₂C₂O₄

Question 43

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 1, the missing base component is _________________________.

A)H₃C₂O₄⁺
B)HC₂O₄^-
C)C₃H₄O₃^2-
D)HC₃H₅O₃
E)C₂H₃O₂^-
F)H₂C₂H₃O₂
G)C₃H₅O₃^-

Question 44

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.
Buffer ______________________ would be the most effective buffer in basic solutions.

A)H₃C₂O₄⁺
B)HC₂O₄^-
C)C₃H₄O₃^2-
D)HC₃H₅O₃
E)C₂H₃O₂^-
F)H₂C₂H₃O₂
G)C₃H₅O₃^-

Question 45

Human blood contains which of the following buffers?

A)protein-H⁺/protein
B)H₂PO₄^-/HPO₄^2-
C)H₂CO₃/HCO₃^-
D)All of the above are involved.

Question 46

Which of the following is true of a buffer prepared with equal concentrations of an acid and its conjugate base?

A)pH = 7
B)pH = pK_a
C)The pH depends on the concentration of the buffer.
D)none of the above

Question 47

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.

A)H₃C₂O₄⁺
B)HC₂O₄^-
C)C₃H₄O₃^2-
D)HC₃H₅O₃
E)C₂H₃O₂^-
F)H₂C₂H₃O₂
G)C₃H₅O₃^-

Question 48

Which of the following is excreted by the kidneys to regulate the effect of excess protein in the diet?

A)NH₄⁺
B)H₃O⁺
C)HCO₃^-
D)H₂PO₄^-

Question 49

Which of the following is a cause of respiratory acidosis?

A)a poor diet
B)hyperventilation
C)hypoventilation
D)intense exercise

Question 50

When carbonated beverages are bottled or canned, the partial pressure of carbon dioxide above this liquid is maintained at a high pressure. This procedure cause the pH of the beverage to

A)increase.
B)decrease.
C)remain constant.

Question 51

Which of the following solutions is the most alkaline?

A)coffee (pH 5.12)
B)urine (pH 7.24)
C)dishwasher detergent (pH 2.38)
D)drain cleaner (pH 10.24)

Question 52

Consider the image which depicts the reaction between CH₃COOH and H₂O. Reactants:
Products:

If the composition of the equilibrium mixture is as represented below
A solution of KF in water will be

A)acidic.
B)basic.
C)neutral.

Question 53

When NaOH reacts with HCl, the net ionic equation for the reaction is:

A)H⁺ + OH^- → H₂O
B)Na⁺ + Cl^- → NaCl
C)NaOH + HCl → NaCl + H₂O
D)NaOH → Na⁺ + OH^-
E)HCl → H⁺ + Cl^-

Question 54

Which of the following is most likely to be a base?

A)NaCl
B)CH₄
C)CH₃NH₂
D)H₂C₂O₄

Question 55

Consider the image which depicts the reaction between CH₃COOH and H₂O. Reactants:
Products:

If the composition of the equilibrium mixture is as represented below
CH₃COOH is classified as

A)strong acid
B)weak acid
C)strong base
D)weak base

Question 56

Which of the following is most likely to be a salt?

A)Ca(NO₃)₂
B)CH₃Cl
C)CH₃CH₂NH₂
D)H₂C₂O₄

Question 57

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

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

Question 58

Which of the following will determine the pH of a buffer made using acetic acid (HC₂H₃O₂) and sodium acetate (NaC₂H₃O₂)?

A)the amount of water present
B)the concentration of C₂H₃O₂-
C)the concentration of HC₂H₃O₂
D)the ratio of the concentrations of C₂H₃O₂^- and HC₂H₃O₂

Question 59

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

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

Question 60

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_______________________.

A)H₃C₂O₄⁺
B)HC₂O₄^-
C)C₃H₄O₃^2-
D)HC₃H₅O₃
E)C₂H₃O₂^-
F)H₂C₂H₃O₂
G)C₃H₅O₃^-

Question 61

Write the equation for the ionization of the weak acid, formic acid, HCHO₂, in water.

Question 62

The buffer solution in the flask was prepared using one of the substances shown below.
citric acid (pK_a 3.08)
NaH₂PO₄ (pK_a 7.21)
NH₄Cl (pK_a 9.25)
Using the pH meter and solution shown in the image below, complete the following statements using one of the terms below.
increase
decrease
remain constant
citric acid
NaH₂PO₄
NH₄Cl
The buffer solution in the beaker could be prepared using__________.

Question 63

The buffer solution in the flask was prepared using one of the substances shown below.
citric acid (pK_a 3.08)
NaH₂PO₄ (pK_a 7.21)
NH₄Cl (pK_a 9.25)
Using the pH meter and solution shown in the image below, complete the following statements using one of the terms below.
increase
decrease
remain constant
citric acid
NaH₂PO₄
NH₄Cl
If HNO were added to the buffer solution the pH of the solution would __________.

Question 64

Consider the following three buffer reactions.
Buffer 1: protein-H⁺ and protein
Buffer 2: H₂CO₃ and HCO₃^-
Buffer 3: H₂PO₄^- and HPO₄^2-
Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described.
Buffer ______________________is involved in preventing blood pH fluctuations due to hypo- and hyperventilation.

Question 65

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.

Question 66

Consider the following three buffer reactions.
Buffer 1: protein-H⁺ and protein
Buffer 2: H₂CO₃ and HCO₃^-
Buffer 3: H₂PO₄^- and HPO₄^2-
Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described.
Buffer 1 works in conjunction with buffer ____________________to regulate the pH of intracellular fluid.

Question 67

Arterial blood gases (ABGs) were drawn on your patient. The following are the some of the results:
Respiratory Rate (RR) 10 breaths/min; pH 7.3; and Pressure of CO₂ 58 torr. The following questions are a basic step-by-step guide in evaluating ABGs.
a. If the normal range is 12 - 24 breaths/min , is this patient breathing within a normal range, hyperventilating, or hypoventilating?
b. Is this pH level on the acidic or basic side of the normal range?
c. Is this pressure of CO₂ level within normal range, high, or low?
d. With the above findings, what is this patient experiencing?

Question 68

Joshua has had high blood pressure for a number of years. At Joshua's last checkup, his doctor orders tests to measure the amount of creatinine in Joshua's blood and urine. Creatinine is a compound that forms whenever muscles break down creatine, a chemical that helps supply energy for muscle contractions.

A) Does everyone have creatine in their circulating blood?
B) Does everyone secrete creatinine in their urine? Why or why not?

Question 69

Consider the following three buffer reactions.
Buffer 1: protein-H⁺ and protein
Buffer 2: H₂CO₃ and HCO₃^-
Buffer 3: H₂PO₄^- and HPO₄^2-
Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described.
Buffer______________________can have a variable pK_a value.

Question 70

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.

Question 71

Consider the following three buffer reactions.
Buffer 1: protein-H⁺ and protein
Buffer 2: H₂CO₃ and HCO₃^-
Buffer 3: H₂PO₄^- and HPO₄^2-
Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described.
Buffer______________________ is the most effective regulator for a pH of 7.2.

Question 72

What is the pH of a solution prepared by dissolving 0.400 g of HCl in enough water to produce 300.0 mL of solution?

Question 73

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

Question 74

The buffer solution in the flask was prepared using one of the substances shown below.
citric acid (pK_a 3.08)
NaH₂PO₄ (pK_a 7.21)
NH₄Cl (pK_a 9.25)
Using the pH meter and solution shown in the image below, complete the following statements using one of the terms below.
increase
decrease
remain constant
citric acid
NaH₂PO₄
NH₄Cl
If KOH were added to the buffer solution the pH of the solution would __________.

Question 75

In a solution of phosphoric acid all of the following species are present. Which is the least abundant?
PO₄^3-
H₂PO₄^-
HPO₄^2-

Question 76

If a patient were in diabetic ketoacidosis (DKA), would you expect their pH level to be high or low?

Question 77

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 this reaction, the conjugate base of ammonia is the _______________________ ion.

Question 78

Consider the following three buffer reactions.
Buffer 1: protein-H⁺ and protein
Buffer 2: H₂CO₃ and HCO₃^-
Buffer 3: H₂PO₄^- and HPO₄^2-
Fill in the blank with the appropriate integer (1,2,or 3)to indicate the buffer system described.
Buffer__________________is found in both plasma and red blood cells.

Question 79

Write the equation for the ionization of weak base hydrazine, N₂H₄, in water.

Question 80

What is the pH of a 1 × 10^-1 M solution of CaCl? Enter a numerical value.