This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: 4. What is the pH of a 0.10 M solution of acetic acid (CH 3 COOH)? K a = 1.8 x 10-5 HA H+ + A-Initial 0.1 Change-x +x +x Equilibrium 0.1-x x x x = 1.34 x 10-3 = [H + ] Therefore, pH = - log [H + ] = 2.87 5. What is the K a of butanoic acid, CH 3 CH 2 CH 2 COOH, if a 0.025 M solution has a pH of 3.21? HA H+ + A-Initial 0.025 Change-x +x +x Equilibrium 0.025-x x x Since the pH = 3.21, the [H+] concentration can be calculated to be 6.17 x 10-4 . Therefore x = 6.17 x 10-4 ....
View Full Document
- Spring '10
- pH, Acid rain, initial change equilibrium