What is the pH of a solution that results from adding 0.075 mol Ca(OH)2 (s) to 1.71 L of a buffer comprised of 0.37 M CH3COOH and 0.37 M CH3COONa?
Any help is appreciated!
You want to use the Henderson-Hasselbalch equation.
mols OH^- added 0.075*2 = 0.150
mols HAc = 1.71L x 0.37M = 0.633
mols Ac^- = 1.71 x 0.37M = 0.633
..........HAc + OH^- ==> Ac^- + H2O
I.......0.633....0......0.633.......
add............0.150............
C......-0.150..-0.150....+0.150......
E.........?.......0........?
Substitute the E line into the HH equation and solve for pH.