I have two questions about pH of buffers. It's a general chemistry class, but the questions aren't similar to anything we've had yet. 1. The problem statement, all variables and given/known data A buffer is prepared by adding 0.96 L of 0.96 M HCl to 762 mL of 1.4 M NaHCOO. What is the pH of this buffer? [Ka(HCOOH) = 1.7 × 10-4] 2. Relevant equations pH=pKa+log([A-]/[HA] 3. The attempt at a solution It's the fact that it's HCl that's really throwing me off. I thought a buffer could only be made with a weak acid and it's conjugate base (and vice versa). I can figure out the pH of the HCl and the NaHCOO solutions without a problem, but it's the combining that's throwing me. 1. The problem statement, all variables and given/known data A certain monoprotic weak acid with Ka = 0.37 can be used in various industrial processes. (a) What is the [H+] for a 0.234 M aqueous solution of this acid and (b) what is its pH? 2. Relevant equations Ka=[H+][A-]/[HA] pH=-log[H+] 3. The attempt at a solution I did an ICE table and set up the equation .37=x^2/(.234-x) to get [H+]. Once I had that, -log[H+] gave me the pH. I got [H+]=.1625 and pH=.79, which doesn't make sense at all considering it's supposed to be a weak acid, but I'm not sure what I'm doing wrong.