This preview shows pages 1–2. Sign up to view the full content.
This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: and the final pH after adding 0.010 mol NaOH. 4. a) 250.0 mL of pure water b) 250.0 mL of a buffer solution that is 0.195 M in HCOOH (formic acid) and 0.275 M in KCOOH (potassium formate). The K a of HCOOH = 1.8 x 10-4 . Determine whether or not the mixing of each of the two solutions indicated below will result in a buffer. Explain why or why not. 5. a) 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b) 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl c) 165.0 mL of 0.10 M HF; 135.0 mL of 0.050 M KOH d) 125.0 mL of 0.15 M CH 3 NH 2 ; 120.0 mL of 0.25 M CH 3 NH 3 Cl e) 105.0 mL of 0.15 M CH 3 NH 2 ; 95.0 mL of 0.10 M HCl The fluids within cells are buffered by H 2 PO 4-and HPO 4 2-. 6. a) Calculate the ratio of H 2 PO 4-and HPO 4 2- required to maintain a pH of 7.1 in a cell. (p K a of H 2 PO 4-is 7.2) b) Could a buffer system employing H 3 PO 4 as the weak acid and H 2 PO 4-as the weak base be used as a buffer system within cells? Explain...
View Full Document
- Fall '11