Acids and Bases Test


True/False

  1. Acids react with metals to produce hydrogen gas.

  2. Bases turn blue litmus paper red.

  3. Aqueous acids and bases usually react to produce water and a salt.

  4. The equivalence point is reached when the moles of acid equal the moles of base.

  5. A solution that has [H+] = 2 x 10 -8 is considered acidic.

  6. A solution that has [H+] = 2 x 10 -8 M has a [OH-] = 5 x 10 -7 M.

  7. A solution with [H+] = 2 x 10 -8 has a pOH = 6.3.

  8. The weak acid, HF, has a KA = [H+] [F-] / [HF].

  9. It would take the same number of moles of base to titrate equal volumes of 1 M HCl (a strong acid) and 1 M HF (a weak acid) to their respective equivalence points.

  10. HCN (KA = 4.0 x 10 -4 ) is a stronger acid than CH3COOH (KA = 1.8 x 10 -5 ).

Multiple Choice (Choose the best answer.)

  1. Which of the following could be part of a conceptual definition of an acid?

    I. Acids taste sour.

    II. Acids donate H+ ions.

    III. Acids react with CaCO3 (limestone) to make carbon dioxide gas.

    I only

    II only

    III only

    I and III only

    I, II, and III

  2. 50.0 mL of 2.0 M HCl is mixed with 50.0 mL of 2.0 M KOH in a calorimeter. After mixing the temperature of the solution increased 15.0 oC. Assuming the specific heat of the solution is 1.00 cal / (g oC), find the heat per mole of H+.

    15.0 oC

    1.5 Kcal

    15 Kcal

    More information is needed.

    None of these is correct.

  3. A concentrated strong acid solution is expected to:

    ionize completely

    be a good conductor

    liberate lots of heat when neutralized by a concentrated strong base

    have a low pH

    All of the above are correct.

  4. 36 mL of a 0.20 M solution of H2SO4 is neutralized by 18 mL of NaOH. What is the concentration of the NaOH?

    0.10 M

    0.20 M

    0.40 M

    0.80 M

    None of these is correct.

  5. 25 mL of 0.10 M HCl is reacted with 26 mL of 0.10 M NaOH. What is the [H+] in the solution?

    0.0020 M

    0.0001 M

    1.0 x 10 -10 M

    5.1 x 10 -12 M

    None of these are correct.

  6. Which of the following is true about a basic solution?

    [OH-] > 10 -7 and pOH > 7

    [OH-] > 10 -7 and pOH < 7

    [OH-] < 10 -7 and pOH > 7

    [H+] > 10 -7 and pH > 7

    [H+] < 10 -7 and pH < 7

  7. The pH of a 0.10 M acid (HA) is 4. What is the KA of the acid?

    1 x 10 8

    1 x 10 7

    1 x 10 -4

    1 x 10 -7

    1 x 10 -8

  8. What is the concentration of H+ in a 0.75 M of acetic acid (CH3COOH). The KA of acetic acid is 1.8 x 10 -5 .

    3.7 x 10 -3

    2.4 x 10 -5

    1.35 x 10 -5

    1.0 x 10 -5

    6.75 x 10 -6

  9. Which of the statements concerning the reaction below is true?

    CN- + CH3COOH HCN + CH3COO-

    CN- and CH3COOH is a conjugate acid/base pair

    HCN and CH3COO- is a conjugate acid/base pair

    CN- and CH3COO- is a conjugate acid/base pair

    CN- and HCN is a conjugate acid/base pair

    Both A and B are correct.

  10. Given that the KA of HCN = 4.0 x 10 -4 and the KA of CH3COOH = 1.8 x 10 -5, the reaction in problem 9 would

    make mostly products at equilibrium

    remain mostly reactants at equilibrium

    have about the same concentrations of reactants and products at equilbrium

    achieve equilibrium quickly

    take a long time to achieve equilibrium

Problem Solving (Respond in complete sentences. Use correct spelling and grammar.)

1) The weak acid, HF is neutralized by the strong base NaOH.

a) Write the reaction in molecular form.


b) Write the reaction in ionic form.


c) If it required 35 mL of 0.21 M NaOH to neutralize 45 mL of HF, calculate the concentration of HF.



2) Given that HNO3 is a strong acid. Find the following for a 0.025 M solution of HNO3.

a) [H+]


b) [OH-]


c) pH


d) pOH

3) A weak acid (HA) has a KA = 1.0 x 10 -5. If you test in with pH paper and find the [H+] = 0.001, what is the concentration of the acid?

Back to Acids, Bases, and Neutralization main page

Back to Chemweb main page