Question 1

A student had 25.0 mL of 0.100 M H₂SO₄ solution. How many mL of a 0.100 M NaOH solution will the sulfuric acid neutralize?

Accepted Answer

The answer of A student had 25.0 mL of 0.100...

Question 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?

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 3

In a neutralization reaction

Accepted Answer

A)  two acids react to form water. 
B)  water and a salt react to form an acid and a base. 
C)  an acid and a salt react to form water and a base. 
D)  a base and a salt react to form water and an acid. 
E)  an acid and a base react to form a salt and water. 
A)  two acids react to form water. 
B)  water and a salt react to form an acid and a base. 
C)  an acid and a salt react to form water and a base. 
D)  a base and a salt react to form water and an acid. 
E)  an acid and a base react to form a salt and water.

Question 4

Write the proper Ka expression for the ionization of acetic acid, HC2H3O₂.

Accepted Answer

Ka = [C₂H₃O₂

Question 5

A 25.0 mL sample of H₂SO₄ requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid?
 H₂SO₄ + 2KOH → K2SO₄ + 2H₂O

Accepted Answer

A)  2.00 M 
B)  2.50 M 
C)  0.800 M 
D)  1.60 M 
E)  1.25 M 
A)  2.00 M 
B)  2.50 M 
C)  0.800 M 
D)  1.60 M 
E)  1.25 M

Question 6

According to the Bronsted-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 7

Which solution has the highest 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.

Question 8

Magnesium metal is not attacked by sulfuric acid solutions.

Accepted Answer

A) True 
 B)False

Question 9

How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M HCl?

Accepted Answer

A)  50.0 mL 
B)  40.0 mL 
C)  0.100 mL 
D)  20.0 mL 
E)  10.0 mL 
A)  50.0 mL 
B)  40.0 mL 
C)  0.100 mL 
D)  20.0 mL 
E)  10.0 mL

Question 10

In a neutralization reaction, how many moles of HClO₄ react with 1 mole of Al(OH)3?

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 11

Which of the following could be a buffer?

Accepted Answer

A)  NaF 
B)  HF + NaF 
C)  HF + H₂O 
D)  NaF + H₂O 
E)  NaCl + HF 
A)  NaF 
B)  HF + NaF 
C)  HF + H₂O 
D)  NaF + H₂O 
E)  NaCl + HF

Question 12

Which of the following is the correctly balanced equation for the complete neutralization of H3PO₄ 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+ 12H3O 
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+ 12H3O

Question 13

The name given to an aqueous solution of HNO₃ is

Accepted Answer

A)  nitric acid. 
B)  nitrous acid. 
C)  hydrogen nitrate. 
D)  hydronitrogen acid. 
E)  hyponitric acid. 
A)  nitric acid. 
B)  nitrous acid. 
C)  hydrogen nitrate. 
D)  hydronitrogen acid. 
E)  hyponitric acid.

Question 14

What is the [OH-] in a solution that has a [H3O+] = 2.0 × 10-4 M?

Accepted Answer

A)  2.0 × 10-10 M 
B)  5.0 × 10-10 M 
C)  1.0 × 10-10 M 
D)  2.0 × 10-4 M 
E)  5.0 × 10-11 M 
A)  2.0 × 10-10 M 
B)  5.0 × 10-10 M 
C)  1.0 × 10-10 M 
D)  2.0 × 10-4 M 
E)  5.0 × 10-11 M

Question 15

Alkalosis is the blood condition in which the blood pH is higher than normal.

Accepted Answer

A) True 
 B)False

Question 16

What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?

Accepted Answer

A)  3.0 × 10-3 
B)  2.52 
C)  3.0 
D)  -2.52 
E)  9.0 
A)  3.0 × 10-3 
B)  2.52 
C)  3.0 
D)  -2.52 
E)  9.0

Question 17

What is the pH of a solution with [OH-] = 2.0 × 10-10 M?

Accepted Answer

A)  9.70 
B)  -9.70 
C)  4.30 
D)  -4.30 
E)  2.0 × 10-10 
A)  9.70 
B)  -9.70 
C)  4.30 
D)  -4.30 
E)  2.0 × 10-10

Question 18

Which of the following is the strongest acid?

Accepted Answer

A)  H3PO₄ 
B)  NH4+ 
C)  NaOH 
D)  H₂CO₃ 
E)  HCl 
A)  H3PO₄ 
B)  NH4+ 
C)  NaOH 
D)  H₂CO₃ 
E)  HCl

Question 19

A major cause of acid rain is

Accepted Answer

A)  CO₂ production. 
B)  CaCO₃ production. 
C)  SO₂ production. 
D)  NH3 production. 
A)  CO₂ production. 
B)  CaCO₃ production. 
C)  SO₂ production. 
D)  NH3 production.

Question 20

The stronger the acid, the __________ the conjugate base.

Accepted Answer

A)  stronger 
B)  weaker 
A)  stronger 
B)  weaker

Exam 10: Acids and Bases

A student had 25.0 mL of 0.100 M H₂SO₄ solution. How many mL of a 0.100 M NaOH solution will the sulfuric acid neutralize?

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?

In a neutralization reaction

Write the proper Ka expression for the ionization of acetic acid, HC2H3O₂.

A 25.0 mL sample of H₂SO₄ requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid? H₂SO₄ + 2KOH → K2SO₄ + 2H₂O

According to the Bronsted-Lowry definition,

Which solution has the highest pH?

Magnesium metal is not attacked by sulfuric acid solutions.

How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M HCl?

In a neutralization reaction, how many moles of HClO₄ react with 1 mole of Al(OH)3?

Which of the following could be a buffer?

Which of the following is the correctly balanced equation for the complete neutralization of H3PO₄ with Ca(OH)₂?

The name given to an aqueous solution of HNO₃ is

What is the [OH-] in a solution that has a [H3O+] = 2.0 × 10-4 M?

Alkalosis is the blood condition in which the blood pH is higher than normal.

What is the pH of a solution with [H3O+] = 3.0 × 10-3 M?

What is the pH of a solution with [OH-] = 2.0 × 10-10 M?

Which of the following is the strongest acid?

A major cause of acid rain is

The stronger the acid, the __________ the conjugate base.

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Filters

Write the proper Ka expression for the ionization of acetic acid, HC₂H₃O₂.

A 25.0 mL sample of H₂SO₄ requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid? H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O

In a neutralization reaction, how many moles of HClO₄ react with 1 mole of Al(OH)₃?

Which of the following is the correctly balanced equation for the complete neutralization of H₃PO₄ with Ca(OH)₂?

What is the [OH-] in a solution that has a [H₃O+] = 2.0 × 10^-4 M?

What is the pH of a solution with [H₃O+] = 3.0 × 10^-3 M?

What is the pH of a solution with [OH-] = 2.0 × 10^-10M?