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13/14 Acid–Base and Solubility Equilibria Quiz Online Quiz Questions

Use this free practice quiz with 20 questions to review 13/14 Acid–Base and Solubility Equilibria, test your knowledge, and prepare for your next test or exam.

20 questions
01
Choose one
1 point

In the reaction NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, how is NH₃ classified according to Brønsted–Lowry theory?

  1. A

    Arrhenius acid

  2. B

    Brønsted–Lowry base

  3. C

    Lewis acid

  4. D

    Brønsted–Lowry acid

02
True or false
1 point

True or false: Water is amphiprotic because it can act as either a Brønsted–Lowry acid or a Brønsted–Lowry base.

  1. A

    True

  2. B

    False

03
Fill in the blank
1 point

Complete the statements: A Brønsted–Lowry proton donor is an , and a Brønsted–Lowry proton acceptor is a .

04
Choose one
1 point

At 25 °C, a solution has pH = 9.20. What is its pOH?

  1. A

    2.80

  2. B

    4.20

  3. C

    4.80

  4. D

    5.80

05
Choose all
1 point

Select all statements that correctly describe an acid–base buffer.

  1. A

    It contains a weak acid and its conjugate base.

  2. B

    It always maintains exactly pH 7.00.

  3. C

    It resists large pH changes when small amounts of strong acid or base are added.

  4. D

    Its capacity is limited if a large amount of strong acid or base is added.

06
True or false
1 point

True or false: The equivalence point and the endpoint are defined identically; both refer to the observed indicator color change.

  1. A

    True

  2. B

    False

07
Written response
1 point

What is the name of the equation pH = pKa + log([A⁻]/[HA]) used to calculate the pH of an acidic buffer?

08
Fill in the blank
1 point

For the dissolution equilibrium AgCl(s) ⇌ Ag⁺(aq) + Cl⁻(aq), complete the expression: Ksp = .

09
Choose one
1 point

A mixture has [Ag⁺] = 1.0 × 10⁻⁴ M and [Cl⁻] = 1.0 × 10⁻⁴ M. Given Ksp(AgCl) = 1.6 × 10⁻¹⁰, what is the expected result?

  1. A

    The solution is unsaturated and precipitation cannot occur.

  2. B

    The solution is exactly at saturation equilibrium.

  3. C

    AgCl precipitation is thermodynamically favored.

  4. D

    The AgCl solid must dissolve until Qsp increases.

10
Choose all
1 point

Select all statements that correctly describe a weak-acid–strong-base titration.

  1. A

    Before equivalence, the solution can contain both HA and A⁻ and behave as a buffer.

  2. B

    At the half-equivalence point, pH equals pKa.

  3. C

    At the equivalence point, the pH is always exactly 7.00 at 25 °C.

  4. D

    At the equivalence point of a weak-acid–strong-base titration, the solution is basic.

11
Written response
1 point

Acetic acid has Kₐ = 1.8 × 10⁻⁵. Using the weak-acid approximation, calculate the pH of a 0.100 M acetic acid solution. Enter the pH to two decimal places.

12
Open ended
1 point

A buffer contains 0.20 mol acetic acid, 0.30 mol acetate ion, and has pKa = 4.76. Calculate its initial pH. Then calculate the pH after 0.010 mol HCl is added, and explain why the pH changes only slightly.

13
Choose one
1 point

For a strong Ba(OH)₂ solution with formal concentration CBa(OH)₂, which approximation gives the hydroxide concentration?

  1. A

    [OH⁻] ≈ CBa(OH)₂

  2. B

    [OH⁻] ≈ 2CBa(OH)₂

  3. C

    [OH⁻] ≈ 1/2CBa(OH)₂

  4. D

    [OH⁻] ≈ CBa(OH)₂ + 1

14
Choose one
1 point

In the reaction BF3 + NH3 → F3B←NH3, what role does BF3 play?

  1. A

    A Lewis base

  2. B

    A Brønsted–Lowry acid

  3. C

    An Arrhenius base

  4. D

    A Lewis acid

15
Choose one
1 point

A solution has pH = 9.20 at 25 °C. Which pair gives its pOH and hydroxide-ion concentration?

  1. A

    pOH = 5.20 and [OH−] = 6.3 × 10^−6 M

  2. B

    pOH = 4.80 and [OH−] = 1.6 × 10^−5 M

  3. C

    pOH = 9.20 and [OH−] = 1.0 × 10^−9.20 M

  4. D

    pOH = 14.00 and [OH−] = 1.0 × 10^−14 M

16
True or false
1 point

True or false: At the equivalence point of a weak-acid–strong-base titration, the pH is approximately 7.00 at 25 °C.

  1. A

    True

  2. B

    False

17
Choose one
1 point

What is the pH at 25 °C of a 0.010 M Ba(OH)2 solution, assuming complete dissociation?

  1. A

    10.30

  2. B

    11.70

  3. C

    12.30

  4. D

    13.70

18
Written response
1 point

What is the conjugate acid of NH3 in the Brønsted–Lowry sense?

19
Choose one
1 point

A buffer contains 0.20 mol of acetic acid and 0.30 mol of acetate ion. Given pKa = 4.76, what is the approximate pH?

  1. A

    4.58

  2. B

    4.94

  3. C

    5.06

  4. D

    9.52

20
Written response
1 point

At the half-equivalence point in a weak-acid–strong-base titration, the weak acid has pKa = 4.76. What is the pH?