Question 1

Which are definitions of an acid according to the Bronsted-Lowry and Lewis theories?

Accepted Answer

Bronsted-Lowry theory (proton donor) ; Lewis theory (electron pair acceptor)

Answer

Bronsted-Lowry theory (proton acceptor) ; Lewis theory (electron pair acceptor)

Answer

Bronsted-Lowry theory (proton acceptor) ; Lewis theory (electron pair donor)

Answer

Bronsted-Lowry theory (proton donor) ; Lewis theory (electron pair donor)

Question 2

What is the formula of the conjugate base of the hydrogenphosphate ion, HPO₄^2-?

Accepted Answer

PO43-

Answer

H2PO4

Answer

HPO4 -

Answer

H3PO4

Question 3

Which species behave as Bronsted-Lowry acids in the following reversible reaction?

H₂PO₄^- (aq) + CN^- (aq) $\leftrightarrow$ HCN (aq) + HPO₄^2- (aq)

Accepted Answer

HCN and H₂PO₄^-

Answer

HCN and CN^-

Answer

H₂PO₄^- and HPO₄^2-

Answer

HCN and HPO₄^2-

Question 4

What is the conjugate base of H₂CO₃ according to the Bronsted-Lowry theory?

Accepted Answer

HCO3-

Answer

CO2

Answer

H₃CO₃⁺

Answer

CO32-

Question 5

Consider the equilibrium below.

CH₃CH₂COOH (aq) + H₂O (l) ⇌ CH₃CH₂COO^–(aq) + H₃O⁺(aq)

Which species represent a conjugate acid-base pair?

Accepted Answer

H3O⁺ and H₂O

Answer

CH₃CH₂COO^– and H₃O⁺

Answer

H₂O and CH₃CH₂COO^–

Answer

CH₃CH₂COOH and H₂O

Question 6

Which compound reacts with calcium oxide, CaO?

Accepted Answer

SO2

Answer

Na2O

Answer

MgO

Answer

K2O

Question 7

Which gas in the atmosphere causes the pH of unpolluted rain to be approximately 6?

Accepted Answer

Carbon dioxide

Answer

Oxygen

Answer

Nitrogen

Answer

Sulfur dioxide

Question 8

What occurs when solid sodium hydrogen carbonate reacts with aqueous sulfuric acid?

Accepted Answer

Bubbles of carbon dioxide form.

Answer

Bubbles of both hydrogen and carbon dioxide form.

Answer

Bubbles of hydrogen form.

Answer

Bubbles of sulfur dioxide form.

Question 9

A student carried out a titration to determine the concentration of an acid and found that his value had good precision but poor accuracy. Which process explains this outcome?

Accepted Answer

Consistently overshooting the volume of solution from the burette into the flask.

Answer

Forgetting to rinse the flask after one of the titrations.

Answer

Reading the meniscus in the burette at a different angle each time.

Answer

Collection of insufficient titration data.

Question 10

What are the products of the reaction between sulfuric acid and sodium hydrogen carbonate?

Accepted Answer

Na₂SO₄ + H₂O + CO₂

Answer

NaSO₄ + H₂CO₃

Answer

Na₂SO₄ + CO₂

Answer

NaSO₄ + H₂O + CO₂

Question 11

An example of a strong acid solution is perchloric acid, , in water. Which statement iscorrect for this solution?

Accepted Answer

HClO₄ is completely dissociated in the solution.

Answer

HClO₄ exist mainly as molecules in the solution.

Answer

The solution has a pH value greater than 7.

Answer

The solution reacts only with strong bases.

Question 12

The pH of a solution changes from pH = 2 to pH = 5. What happens to the concentration of the hydrogen ions during this pH change?

Accepted Answer

It decreases by a factor of 1000

Answer

It increases by a factor of 1000

Answer

It increases by a factor of 100

Answer

It decreases by a factor of 100

Question 13

What is the pH of the solution formed when of HCl(aq) with pH 1.0 is added to of water?

Accepted Answer

3.0

Answer

2.5

Answer

2.0

Answer

1.5

Question 14

Three aqueous solutions of nitric acid are listed below.

W. 0.100 mol/L HNO₃ (aq)

X. 0.001 mol/L HNO₃(aq)

Y. 0.010 mol/L HNO₃ (aq)

What is the correct order of increasing pH of these solutions?

Accepted Answer

W < Y < X

Answer

W < X < Y

Answer

X < Y < W

Answer

X < W < Y

Question 15

A solution of acid HX has a pH = 1 and a solution of acid HY has a pH = 3. Which statement must be correct?

Accepted Answer

The [H+] in the solution of HX is 100 times greater than the in the solution of HY.

Answer

HY is a stronger acid than HX.

Answer

The [H+] in the solution of HY is 100 times greater than the in the solution of HX.

Answer

HX is a stronger acid than HY.

Question 16

For equal volumes of 1.0 mol/L solutions of hydrochloric acid, HCl(aq), and methanoic acid, HCOOH (aq), which statements are correct?

I. HCl dissociates more than HCOOH

II. HCl is a better electrical conductor than HCOOH

III. HCl will neutralize more NaOH than HCOOH

Accepted Answer

I and II only

Answer

I and III only

Answer

I, II and III

Answer

II and III only

Question 17

When equal volumes of four solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?

Accepted Answer

HNO₃ < CH₃COOH < CH₃CH₂NH₂ < KOH

Answer

CH₃COOH < HNO₃ < CH₃CH₂NH₂ < KOH

Answer

CH₃CH₂NH₂ < HNO₃ < CH₃COOH < KOH

Answer

KOH < CH₃CH₂NH₂ < CH₃COOH < HNO₃

Question 18

Which list contains only strong acids?

Accepted Answer

HCl, HNO₃, H₂SO₄

Answer

HCl, HNO₃, H₂CO₃

Answer

CH₃COOH, HNO₃, H₂SO₄

Answer

CH₃COOH, H₂CO₃, H₃PO₄

Question 19

An example of a strong acid solution is perchloric acid, HClO₄, in water. Which statement is correct for this solution?

Accepted Answer

HClO₄ is completely dissociated in the solution.

Answer

The solution reacts only with strong bases.

Answer

HClO₄exists mainly as molecules in the solution.

Answer

The solution has a pH value greater than 7.

Question 20

Which of the following are weak acids in aqueous solution?

I. CH₃COOH

II. H₂CO₃

III. HCL

Accepted Answer

I and II only

Answer

I, II, and III

Answer

II and III only

Answer

I and III only

Question 21

Which causes acid deposition?

Accepted Answer

SO2

Answer

SiO2

Answer

CO2

Answer

SrO

Question 22

Which pH value is that of an aqueous solution of carbon dioxide?

Accepted Answer

5.6

Answer

9.8

Answer

2.1

Answer

12.2

Question 23

Which of the following gases does not result in acid deposition?

Accepted Answer

CO2

Answer

NO2

Answer

NO

Answer

SO2

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