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Unformatted text preview: A student needs to make an aqueous solution with pH = 9.0. Can this be done by simply diluting 1 M HCl? Explain below, showing calculations as necessary. 1. Problems for week 6 discussion Name a) Solid ammonium bromide (NH 4 Br) is added to pure water. Will the resulting solution be acidic, basic, or neutral? (Use a chemical equation to justify your answer) b) If the aqueous ammonium bromide solution made above has a pH of 8.5, what must be the concentration of ammonium ion? (NH 3 p K b = 4.75) 2. If added to 1 L of 0.20 M acetic acid (CH 3 COOH), which of these would form a buffer? a) 0.10 mole NaCH 3 COO b) 0.10 mole NaOH c) 0.10 mole HCl d) 0.30 mole NaOH 3. A buffer consists of 0.20 lactic acid (p K a = 3.85) and 0.30 M sodium lactate. a) Calculate the pH of this buffer b) Calculate the pH of this buffer after addition of 10.0 mL of 0.01 M HCl to 10.0 mL of the buffer 4. Vinegar must be at least 4% acetic acid by weight (0.67 M). If you titrate a 5.00 mL sample of vinegar with 0.100 M NaOH and find that you need 33.5 mL to reach the equivalence point, does your sample meet the 0....
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This note was uploaded on 05/15/2011 for the course CHM 116 taught by Professor Matchett during the Fall '11 term at Grand Valley State University.
- Fall '11