Question 1

What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30?

Accepted Answer

A) respiratory acidosis 
B) respiratory alkalosis 
C) metabolic acidosis 
D) metabolic alkalosis 
E) diabetes mellitus 
A) respiratory acidosis 
B) respiratory alkalosis 
C) metabolic acidosis 
D) metabolic alkalosis 
E) diabetes mellitus A

Question 2

Which of the following is the weakest acid?

Accepted Answer

A) HF (Ka for HF is 7.2 × 10-4) 
B) HCN (Ka for HCN is 4.9 × 10-10) 
C) HCNO (Ka for HCNO is 2 × 10-4) 
D) H₃BO₃(Ka for H3BO3Is 5.4 × 10-10) 
A) HF (Ka for HF is 7.2 × 10-4) 
B) HCN (Ka for HCN is 4.9 × 10-10) 
C) HCNO (Ka for HCNO is 2 × 10-4) 
D) H₃BO₃(Ka for H3BO3Is 5.4 × 10-10) B

Question 3

Which solution has the lowest pH?

Accepted Answer

A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate 
B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate 
C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate 
D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate 
E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate. 
A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate 
B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate 
C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate 
D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate 
E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate. A

Question 4

What is the pH of a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate?

Accepted Answer

The answer of What is the pH of a buffer...

Question 5

If an acid has a Ka << 1, is it classified as a weak acid or a strong acid?

Accepted Answer

The answer of If an acid has a Ka <<...

Question 6

The conjugate acid of H2PO₄ 2- is ________.

Accepted Answer

Question 7

According to the Arrhenius concept, if HNO₃ were dissolved in water, it would act as

Accepted Answer

A) a base. 
B) an acid. 
C) a source of hydroxide ions. 
D) a source of H- ions. 
E) a proton acceptor. 
A) a base. 
B) an acid. 
C) a source of hydroxide ions. 
D) a source of H- ions. 
E) a proton acceptor.

Question 8

A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?

Accepted Answer

The answer of A student had 2.0 L of a...

Question 9

In which of the following are the pH values arranged from the most basic to the most acidic?

Accepted Answer

A) 1, 3, 6, 8, 11, 14 
B) 2, 5, 7, 9, 10, 11 
C) 14, 10, 7, 4, 3, 1 
D) 14, 10, 7, 1, 3, 5 
E) 7, 10, 14, 4, 3, 1 
A) 1, 3, 6, 8, 11, 14 
B) 2, 5, 7, 9, 10, 11 
C) 14, 10, 7, 4, 3, 1 
D) 14, 10, 7, 1, 3, 5 
E) 7, 10, 14, 4, 3, 1

Question 10

Which of the following is a buffer system?

Accepted Answer

A) NaCl and NaNO₃ 
B) HCl and NaOH 
C) H2CO3 And KHCO₃ 
D) NaCl and NaOH 
E) H2O and HCl 
A) NaCl and NaNO₃ 
B) HCl and NaOH 
C) H2CO3 And KHCO₃ 
D) NaCl and NaOH 
E) H2O and HCl

Question 11

The conjugate base of HCl is Cl-.

Accepted Answer

A) True 
 B)False

Question 12

A solution with a pH of 4.0 is basic.

Accepted Answer

A) True 
 B)False

Question 13

Which of the following is correctly identified?

Accepted Answer

A) NH₃, strong acid 
B) NaOH, strong base 
C) HCl, weak acid 
D) H2CO₃, strong acid 
E) Ca(OH)₂, weak base 
A) NH₃, strong acid 
B) NaOH, strong base 
C) HCl, weak acid 
D) H2CO₃, strong acid 
E) Ca(OH)₂, weak base

Question 14

Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?

Accepted Answer

A) In acids, [OH-] is greater than [ H₃O+]. 
B) In bases, [OH-] = [ H₃O+]. 
C) In neutral solutions, [ H₃O+] = [ H2O]. 
D) In bases, [OH-] is greater than [ H₃O+]. 
E) In bases, [OH-] is less than [ H₃O+]. 
A) In acids, [OH-] is greater than [ H₃O+]. 
B) In bases, [OH-] = [ H₃O+]. 
C) In neutral solutions, [ H₃O+] = [ H2O]. 
D) In bases, [OH-] is greater than [ H₃O+]. 
E) In bases, [OH-] is less than [ H₃O+].

Question 15

Which of the following is the correctly balanced equation for the complete neutralization of H₃ PO₄ with Ca(OH)₂ ?

Accepted Answer

A) H₃PO₄+ Ca(OH)₂→ CaHPO₄+ 2H2O 
B) 3H₃PO₄+ Ca(OH)₂→ Ca3(PO₄)₂+ 5H2O 
C) H₃PO₄+ Ca(OH)₂→ Ca3(PO₄)₂+ H2O 
D) 2H₃PO₄+ 3Ca(OH)₂→ Ca3(PO₄)₂+ 6H2O 
E) 4H₃PO₄+ 6Ca(OH)₂→ 2Ca3(PO₄)₂+ 12H2O 
A) H₃PO₄+ Ca(OH)₂→ CaHPO₄+ 2H2O 
B) 3H₃PO₄+ Ca(OH)₂→ Ca3(PO₄)₂+ 5H2O 
C) H₃PO₄+ Ca(OH)₂→ Ca3(PO₄)₂+ H2O 
D) 2H₃PO₄+ 3Ca(OH)₂→ Ca3(PO₄)₂+ 6H2O 
E) 4H₃PO₄+ 6Ca(OH)₂→ 2Ca3(PO₄)₂+ 12H2O

Question 16

For the problem(s) that follow, consider the reaction in which magnesium reacts with an HCl solution .
Mg(s) + 2HCl(aq) → MgCl₂(aq) + H2(g)
-If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution?

Accepted Answer

A) 1.65 M 
B) 80.0 M 
C) 8.00 M 
D) 0.823 M 
E) 3.29 M 
A) 1.65 M 
B) 80.0 M 
C) 8.00 M 
D) 0.823 M 
E) 3.29 M

Question 17

According to the Arrhenius concept, if NaOH were dissolved in water, it would act as

Accepted Answer

A) a base. 
B) an acid. 
C) a source of hydronium ions. 
D) a source of H- ions. 
E) a proton donor. 
A) a base. 
B) an acid. 
C) a source of hydronium ions. 
D) a source of H- ions. 
E) a proton donor.

Question 18

A solution which has [OH-] = 3.4 × 10-12 M is

Accepted Answer

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

Question 19

According to the Brønsted-Lowry definition,

Accepted Answer

A) an acid is a proton acceptor. 
B) a base produces H+ ions in aqueous solutions. 
C) a base is a proton donor. 
D) a base is a proton acceptor. 
E) an acid acts as the solvent. 
A) an acid is a proton acceptor. 
B) a base produces H+ ions in aqueous solutions. 
C) a base is a proton donor. 
D) a base is a proton acceptor. 
E) an acid acts as the solvent.

Question 20

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is

Accepted Answer

A) 0.212 M. 
B) 0.115 M. 
C) 0.500 M. 
D) 0.390 M. 
E) 0.137 M. 
A) 0.212 M. 
B) 0.115 M. 
C) 0.500 M. 
D) 0.390 M. 
E) 0.137 M.

Exam 11: Acids and Bases

What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30?

Which of the following is the weakest acid?

Which solution has the lowest pH?

What is the pH of a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate?

If an acid has a Ka << 1, is it classified as a weak acid or a strong acid?

The conjugate acid of H2PO₄ 2- is ________.

According to the Arrhenius concept, if HNO₃ were dissolved in water, it would act as

A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?

In which of the following are the pH values arranged from the most basic to the most acidic?

Which of the following is a buffer system?

The conjugate base of HCl is Cl-.

A solution with a pH of 4.0 is basic.

Which of the following is correctly identified?

Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?

Which of the following is the correctly balanced equation for the complete neutralization of H₃ PO₄ with Ca(OH)₂ ?

For the problem(s) that follow, consider the reaction in which magnesium reacts with an HCl solution . Mg(s) + 2HCl(aq) → MgCl₂(aq) + H2(g) -If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution?

According to the Arrhenius concept, if NaOH were dissolved in water, it would act as

A solution which has [OH-] = 3.4 × 10-12 M is

According to the Brønsted-Lowry definition,

25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is

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The conjugate acid of H₂PO₄ ^2- is ________.