You are given sodium acetate, 1M HCl, NaHCO3 and Na2CO3. Determine which of these four you would need and then show calculations to make buffer pH = 4.7 by method 2. Assume making 100 mls of a 0.1 M buffer.

Neutralization of a portion of the weak base with sufficient strong acid to give the desired ratio, [A- ]/[HA]: Na+ + A- + HCl → HA + Na+ + Cl-

I've been having a lot of trouble going step by step with this one. If you could really explain the logic behind each step it would be very much appreciated!! I'm also confused about the ka value. Am I just supposed to look that up? Thank you so much for your time!