Acid-Base and Solubility Homework Problem Set

This problem set was developed by S.E. Van Bramer for Chemistry 146 at Widener University.

  1. Calculate the H3O1+ concentration, OH1- concentration, pH, and pOH of the following solutions. First solve assuming that Kw is insignificant. Repeat the calculations and include Kw (you will need to use the quadratic equation to solve these). When is Kw significant?
    1. 1.0 x 10-9 M HNO3
    2. 1.0 x 10-6 M HNO3
    3. 1.0 x 10-3 M HNO3
    4. 1.0 x 10-1 M HNO3
    5. 1.0 M HNO3
    6. 10.0 M HNO3

  2. Calculate the H3O1+ concentration, OH1- concentration, pH, pOH, nitrate ion concentration and sodium ion concentration for the following experimental steps in a titration. Graph your results.
    1. 6 M HNO3.
    2. Pure Deionized Water.
    3. 1.00 mL of the nitric acid is diluted with deionized water to a volume of 100.0 ml.
    4. 5.2468 g of NaOH is dissolved in deionized water to a volume of 1.000 liter.
    5. 0.100 mL of the sodium hydroxide solution is added to the nitric acid solution.
    6. 1.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
    7. 10.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
    8. 20.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
    9. Enough sodium hydroxide solution is added to reach the equivilence point.
    10. 50.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
    11. 100.0 mL of the sodium hydroxide solution is added to the nitric acid solution.

  3. What is the pH and pOH of a buffer prepared by adding 1.2435 g of sodium acetate to 100 mL of 0.124 M acetic acid. Calculate using the Henderson-Hasselbalch equation (as shown in your textbook) and using the quadratic equation (as shown in class).

  4. Determine the pH and pOH of a buffer prepared by adding 0.0100 g of sodium hydroxide to 100 mL of 0.124 M acetic acid. Calculate using the Henderson-Hasselbalch equation (as shown in your textbook), the method of successive approximations, and using the quadratic equation (as shown in class).

  5. Calculate the H3O1+ concentration, OH1- concentration, pH, pOH, acetic acid concentration, and the acetate ion concentration for the following experimental steps in a titration. Calculate using the Henderson-Hasselbalch equation (as shown in your textbook) and using the quadratic equation (as shown in class). Graph your results.
    1. 1.00 mL of glacial acetic acid (pure acetic acid, density 1.0492 g/mL) is diluted with deionized water to a volume of 100.0 ml.
    2. 2.2468 g of NaOH is dissolved in deionized water to a volume of 500 mL.
    3. 0.100 mL of the sodium hydroxide solution is added to the acetic acid solution.
    4. 1.00 mL of the sodium hydroxide solution is added to the acetic acid solution.
    5. 10.00 mL of the sodium hydroxide solution is added to the acetic acid solution.
    6. Enough sodium hydroxide solution is added to reach the equivilence point.
    7. 160.00 mL of the sodium hydroxide solution is added to the acetic acid solution.
    8. 200.0 mL of the sodium hydroxide solution is added to the acetic acid solution.

  6. Assuming the molar solubility of a salt is x, write the balanced chemical equation for dissolving the solid salt, write the Ksp expression for the reaction, and rearrange the Ksp expression to solve for x.
    1. AB (s)
    2. AB2 (s)
    3. A2B (s)
    4. AB3 (s)
    5. A2B3 (s)

  7. 3.2 x 10-3 g of manganese (II) hydroxide will dissolve in 1 liter of water at 25 oC. What is the pH of a saturated manganese (II) hydroxide solution? What is Ksp for manganese (II) hydroxide?

  8. How many grams of silver chromate can dissolve in 250 mL of 0.25 M sodium chromate?

  9. 0.500 grams of lead nitrate is dissolved in 250.0 mL of water. When 10 mL of 1.0 M NaCl is added to this solution: What is the mass of the precipitate? What is the equilibrium concentration of all the ions in the solution? Repeat these calculatons if 20 mL of 2.0 M Na Cl is added to the original lead nitrate solution.

Please send comments or suggestions to svanbram@science.widener.edu

Scott Van Bramer
Department of Chemistry
Widener University
Chester, PA 19013

© copyright 1996, S.E. Van Bramer
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Last Updated: Saturday, May 18, 1996