Unit 12 Quiz--Acid and Base Titrations

Multiple Choice (Choose the best answer.)

  1. In the laboratory experiment, Heat of Acid / Base Reactions, you saw that a 2.0 M solution of HNO3 was a great counductor of electrcity. What explains this?

    HNO3 is a strong acid.

    HNO3 ionizes completely in water.

    HNO3 neutralizes bases.

    Both A and B are correct.

    A, B, and C are correct.


  2. The ionic reaction for the neutralization of HCl (a strong acid) with NaOH (a strong base) is:

    HCl (aq) + NaOH (aq) H2O (l) + NaCl (aq)

    H + (aq) + Cl - (aq) + Na + (aq) + OH - (aq) H + (aq) + OH - (aq) + Na + (aq) + Cl - (aq)

    H + (aq) + Cl - (aq) + Na + (aq) + OH - (aq) H2O (l) + Na + (aq) + Cl - (aq)

    H + (aq) + Cl - (aq) + Na + (aq) + OH - (aq) H2O (l) + NaCl (s)

    None of the above are correct.


  3. The end point ( or equivalence point ) your acid / base titration between HCl and NaOH occurred when:

    the acid and the base neutralized each other.

    the phenolphthalein indicator turned a faint pink color.

    the moles of H += the moles of OH -.

    Both A and B are correct.

    A, B, and C are correct.


    The information given at

    Concentration HCl --

    0.35 M
    right will be used in questions

    Volume HCl --

    24.35 mL
    4, 5, and 6.

    Volume NaOH --

    36.44 mL
  4. The data above refers to a titration of NaOH with a known concentration of HCl. Calculate the moles of HCl at the end point.

    8.5 moles HCl

    0.14 moles HCl

    0.0096 moles HCl

    0.0085 moles HCl

    None of the above are correct.


  5. Calculate the moles of NaOH present at the end point of the titration.

    12.8 moles NaOH

    0.013 M NaOH

    0.0096 moles NaOH

    0.0085 moles NaOH

    None of the above are correct.


  6. Calculate the molarity of NaOH.

    0.23 M NaOH

    0.35 M NaOH

    0.53 M NaOH

    1.9 M NaOH

    None of the above are correct.


  7. It required 42.35 mL of H2SO4 to neutralize 21.17 mL of 0.5000 M NaOH. Calculate the concentration of H2SO4. (Hint: Write a balanced reaction to help you perform the calculation.)

    0.2499 M H2SO4

    0.1250 M H2SO4

    0.4998 M H2SO4

    1.000 M H2SO4

    None of the above are correct.


  8. In your acid / base titration lab, you found the molecular weight of a solid acid. Perform the same calculation given that 0.50 g of acid required 20.00 mL of 0.25 M NaOH to titrate it. (Assume that the acid and base react on a one-to-one molar basis.)

    0.0025 g/mol

    0.010 g/mol

    0.10 g/mol

    4.0 x 102 g/mol

    None of these answers are correct.


  9. A 20.0 mL of 0.500 M HCl are mixed with 15.0 mL of 0.500 M NaOH. What is true about the resulting solution?

    The solution will be acidic with a pH > 7.

    The solution will be acidic with a pH < 7.

    The solution will be basic with a pH > 7.

    The solution will be basic with a pH < 7.

    None of the above are true.


  10. Calculate the pH of the mixture in problem 9. You may have to refer to questions 10 and 11 in your supplemental problems.

    pH = 0.3010

    pH = 0.9031

    pH = 1.146

    pH = 2.602

    None of these are correct.


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