What is the pH of a solution that results from adding 0.054 mol Ca(OH)2 to 1.76 L of a buffer comprised of 0.33 M CH3COOH and 0.33 M CH3COONa?
I'm not sure how to start this. Thanks!
mols CH3COOH (HAc) = M x L = 0.581
mols CH3COONa (NaAc) = 0.581
.......HAc + OH^- ==> Ac^- + H2O
I......0.581..0......0.581........
add.........2*0.054...............
C.....-1.08..-1.08..+1.08
E.....0.499..0.......1.66
Substitute the E line into the Henderson-Hasselbalch equation and solve for pH.