1. U2 S3 L3 Acid / Base stoichiometry. pages 600-601: Calculations Involving Neutralization Reactions pages 585-586: Calculations That Involve Strong Acids and Bases Questions page 602: items 17, 18, 19 and 20 page 616: items 6 and 7 page 618: item 19 page 586: items 1, 2, 3 and 4

2. Upon completion of this lesson, you should be able to: perform stoichiometric calculations where one of molarity of acid, molarity of base, volume of acid or volume of base is to be determined from knowledge of the others calculating any of [H3O+], [OH-], pH, or pOH in a strong acid-strong base mixture where there is an excess of either the acid or the base (public exam question!!)

3. Sample 1 A series of 20.00 mL samples of sodium hydroxide are titrated with an average of 5.47 mL of 0.100 mol/L sodium hydrogen sulfate. Calculate the molar concentration of the sodium hydroxide solution.

4. Sample 2 Biff and Molly needed standardized hydrochloric acid to carry out a titration. Their teacher provided them with a stock solution labelled 1.0 M HCl. Knowing that stock solutions of HCl can have variable molar concentrations, Biff and Molly decide to standard the stock solution. They titrated three 1.00 g samples of sodium carbonate with an average of 18.97 mL of stock hydrochloric acid. Calculate the molar concentration of the hydrochloric acid stock solution.

5. Sample 3 Three 20.00 mL samples of sulfuric acid are completely neutralized with an average volume of 8.74 mL of standardized 1.16 M sodium hydroxide. Calculate the molar concentration of the sulfuric acid solution.

6. Excess and Limiting reagents A 20.00 mL sample of 0.105 M hydrochloric acid is titrated with 28.55 mL of 0.102 M sodium hydroxide. Calculate the pH of the mixture in the Erlenmeyer flask

7. Calculate the pH, pOH, [H 3 O + ] and [OH - ] of a mixture formed by adding 40.00 mL of 0.221 mol/L sulfuric acid to 91.63 mL of 0.210 mol/L sodium hydroxide.