- Calculate the H
_{3}O^{1+}concentration, OH^{1-}concentration, pH, and pOH of the following solutions. First solve assuming that K_{w}is insignificant. Repeat the calculations and include K_{w}(*you will need to use the quadratic equation to solve these*). When is K_{w}significant?- 1.0 x 10
^{-9}M HNO_{3} - 1.0 x 10
^{-6}M HNO_{3} - 1.0 x 10
^{-3}M HNO_{3} - 1.0 x 10
^{-1}M HNO_{3} - 1.0 M HNO
_{3} - 10.0 M HNO
_{3}

- 1.0 x 10
- Calculate the H
_{3}O^{1+}concentration, OH^{1-}concentration, pH, pOH, nitrate ion concentration and sodium ion concentration for the following experimental steps in a titration. Graph your results.- 6 M HNO
_{3}. - Pure Deionized Water.
- 1.00 mL of the nitric acid is diluted with deionized water to a volume of 100.0 ml.
- 5.2468 g of NaOH is dissolved in deionized water to a volume of 1.000 liter.
- 0.100 mL of the sodium hydroxide solution is added to the nitric acid solution.
- 1.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
- 10.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
- 20.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
- Enough sodium hydroxide solution is added to reach the equivilence point.
- 50.00 mL of the sodium hydroxide solution is added to the nitric acid solution.
- 100.0 mL of the sodium hydroxide solution is added to the nitric acid solution.

- 6 M HNO
- 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).
- 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).
- Calculate the H
_{3}O^{1+}concentration, OH^{1-}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.- 1.00 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.
- 2.2468 g of NaOH is dissolved in deionized water to a volume of 500 mL.
- 0.100 mL of the sodium hydroxide solution is added to the acetic acid solution.
- 1.00 mL of the sodium hydroxide solution is added to the acetic acid solution.
- 10.00 mL of the sodium hydroxide solution is added to the acetic acid solution.
- Enough sodium hydroxide solution is added to reach the equivilence point.
- 160.00 mL of the sodium hydroxide solution is added to the acetic acid solution.
- 200.0 mL of the sodium hydroxide solution is added to the acetic acid 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