Buffers & Titrations Questions (& such)
1. Calculate the pH of the following solutions:
a) 0.500 M nitric acid
b) 0.00100 M barium hydroxide
c) 1.0 M RbF
d) 1.0 M potassium dihydrogen phosphate
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 HCl. Calculate the pH after 20.0 mL of the HCl 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.