Which two species act as Brønsted–Lowry acids in the reaction? H 2 PO 4 − (aq) + OH − (aq) ⇌ HPO 4 2− (aq) + H 2 O (l)

H 2 PO 4 − (aq) and H 2 O (l)

HPO 4 2− (aq) and OH − (aq)

H 2 PO 4 − (aq) and HPO 4 2− (aq)

Which of the following is an example of a Lewis acid–base reaction, but not a Brønsted–Lowry acid–base reaction?

Co(H 2 O) 2 +6 (aq) + 4HCl(aq) → CoCl 2 −4 (aq) + 4H + (aq) + 6H 2 O(l)

2CrO 2 −4 (aq) + 2H + (aq) → Cr 2 O 2 −7 (aq) + H 2 O(l)

NH 3 (aq) + H + (aq) → NH +4 (aq)

CH3COO − (aq) + H2O(l) → CH3COOH(aq) + OH − (aq)

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

Bubbles of carbon dioxide form.

Bubbles of sulfur dioxide form.

Bubbles of both hydrogen and carbon dioxide form.

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?

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

Collection of insufficient titration data.

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

Forgetting to rinse the flask after one of the titrations.

Which solution is basic at 25 °C? K w = 1.0 × 10 −14

[H 3 O + ] = 1.0 × 10 −13 mol dm −3

[H + ] = 1.0 × 10 −3 mol dm −3

[OH − ] = 1.0 × 10 −13 mol dm −3

What will happen if the pressure is increased in the following reaction mixture at equilibrium? CO 2 (g) + H 2 O (l) ⇌ H + (aq) + HCO 3 − (aq)

The equilibrium will shift to the right and pH will decrease.

The equilibrium will shift to the right and pH will increase.

The equilibrium will shift to the left and pH will increase.

The equilibrium will shift to the left and pH will decrease.

Which statement is incorrect for a 0.10 mol dm –3 HCOOH solution?

[HCOO – ] is approximately equal to [H + ]

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

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

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?

It decreases by a factor of 1000

It increases by a factor of 1000

It decreases by a factor of 100

It increases by a factor of 100

An example of a strong acid solution is perchloric acid, HClO 4 , in water. Which statement is correct for this solution?

HClO 4 is completely dissociated in the solution.

HClO 4 exists mainly as molecules in the solution.

The solution reacts only with strong bases.

The solution has a pH value greater than 7.

What is the correct expression for the ionic product constant of water, K w ?

K w = [ H + ] [ O H − ] K_w=\left[H^+\right]\left[OH^-\right] K w = [ H + ] [ O H − ]

K w = [ H + ] [ O H − ] K_w=\frac{\left[H^+\right]}{\left[OH^-\right]} K w = [ O H − ] [ H + ]

K w = [ H 2 O ] [ H + ] [ O H − ] K_w=\frac{\left[H_2O\right]}{\left[H^+\right]\left[OH^-\right]} K w = [ H + ] [ O H − ] [ H 2 O ]

K w = [ H + ] + [ O H − ] K_w=\left[H^+\right]+\left[OH^-\right] K w = [ H + ] + [ O H − ]

What is the order of increasing pH for the following solutions of the same concentration?

HCl (aq) < CH 3 COOH (aq) < NH 3 (aq) < NaOH (aq)

HCl (aq) < NH 3 (aq) < NaOH (aq) < CH 3 COOH (aq)

CH 3 COOH (aq) < HCl (aq) < NH 3 (aq) < NaOH (aq)

NaOH (aq) < NH 3 (aq) < CH 3 COOH (aq) < HCl (aq)

Which statement is correct?

A strong acid is a good proton donor and has a weak conjugate base.

A strong acid is a good proton donor and has a strong conjugate base.

A weak acid is a poor proton acceptor and has a strong conjugate base.

A strong base is a good proton donor and has a weak conjugate acid.

A student adds 0.3 g of magnesium metal to equal volumes of hydrochloric acid and ethanoic acid of the same concentrations in separate flasks. Which statement is correct?

The same total volume of H 2 gas is produced with both hydrochloric acid and ethanoic acid.

Hydrochloric acid reacts more rapidly as it has a higher pH than ethanoic acid.

A greater total volume of H 2 gas is produced with hydrochloric acid than with ethanoic acid.

Ethanoic acid reacts more slowly because it has a lower pH than hydrochloric acid.

Topic 8 Acids and Bases

Quiz

•

Science

•

11th - 12th Grade

•

Practice Problem

•

Medium

Used 56+ times

FREE Resource

67 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

What is the difference between a conjugate Brønsted–Lowry acid–base pair?

Electron pair

Positive charge

Proton

Hydrogen atom

2.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which is an example of an amphiprotic species?

Al₂O₃

CO₃²⁻

P₄O₁₀

HPO₄²⁻

3.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

Which two species act as Brønsted–Lowry acids in the reaction?

H₂PO₄⁻ (aq) + OH⁻ (aq) ⇌
HPO₄²⁻ (aq) + H₂O (l)

HPO₄²⁻ (aq) and OH⁻ (aq)

H₂PO₄⁻ (aq) and HPO₄²⁻ (aq)

HPO₄²⁻ (aq) and H₂O (l)

H₂PO₄⁻ (aq) and H₂O (l)

4.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

Which classification is correct for the reaction?
H₂PO₄⁻(aq) + H₂O(l) → HPO₄²⁻(aq) + H₃O⁺(aq)

A

B

C

D

5.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

What describes HPO₄²⁻?

Amphiprotic but not amphoteric

Amphoteric but not amphiprotic

Amphiprotic and amphoteric

Neither amphiprotic nor amphoteric

6.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

Which is an acid-base conjugate pair?

H₃O⁺ / OH^–

H₂SO₄ / SO₄^2–

CH₃COOH / H₃O⁺

CH₃NH₃⁺ / CH₃NH₂

7.

MULTIPLE CHOICE QUESTION

3 mins • 1 pt

Which of the following is correct?

A weak acid is a proton donor and its aqueous solution shows good conductivity.

A weak acid is a proton donor and its aqueous solution shows poor conductivity.

A weak acid is a proton acceptor and its aqueous solution shows good conductivity.

A weak acid is a proton acceptor and its aqueous solution shows poor conductivity.

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Topic 8 Acids and Bases

67 questions

What is the difference between a conjugate Brønsted–Lowry acid–base pair?

Which is an example of an amphiprotic species?

Which two species act as Brønsted–Lowry acids in the reaction?

H₂PO₄⁻ (aq) + OH⁻ (aq) ⇌
HPO₄²⁻ (aq) + H₂O (l)