Show your work neatly on additional sheets of paper. Be sure to use and show mole charts and ICE charts as appropriate. Temperature is 25°C unless otherwise specified. Use the Ka & Ks Tables of this site. Note that these values are experimental values, and they vary slightly depending on the source. In order to check your answers on this site, you need to use the tables of this site. 1. Calculate the pH of the following solutions: (Note, this is review material from Acids-Bases Part 1.) a) 0.500 M nitric acid b) 0.00100 M barium hydroxide c) 1.0 M RbF d) 0.10 M ammonium chloride 2. A buffer solution contains 0.120 mole of propionic acid, and 0.110 mole of potassium propionate. The buffer solution has a total volume of 1.00 L a) Find the pH of this buffer solution. b) Find the pH of this buffer solution after the addition of 10.0 mL of 0.400 M KOH solution. 3. How many grams of potassium hypochlorite should be added to 1.00 L of 0.100 M hypochlorous acid to form a buffer solution of pH 7.70? Assume that no volume change occurs when the potassium hypochlorite is added. 4. In a titration, 60.0 mL of 0.100 M ammonia is titrated with 0.150 M HCI. Calculate the pH after 20.0 mL of the HCI has been added. 5. A 25.0 mL sample of 0.110 M lactic acid (Ka = 0.00014) is titrated with 0.150 M NaOH solution. a) Calculate the pH of the solution after the addition of 5.0 mL of the NaOH. b) Calculate the pH at the equivalence point. 6. A 100.0 mL buffer solution is 0.100M acetic acid and 0.100 M sodium acetate. a) What is the pH of this buffer? b) Calculate the pH of this buffer solution after the addition of 20.0 mL of 0.100 M nitric acid. Assume volumes are additive. What is the pH change? c) For the sake of comparison, 20.0 mL of 0.100 M nitric acid is mixed with 100.0 mL of deionized (pH 7) water. Assume volumes are additive. Calculate the pH of this solution, and the pH change.