Hey guys, I think I've done the better half of this question, but I'm stuck at the end:
Calculate the concentration of the acetate ion (M) in a solution prepared by dissolving 1.00×10-3 mol of HCl(g) in 1.00 L of 1.90 M aqueous acetic acid. Ka = 1.7E-5
. CH3COOH --> CH3COO- + H+
initial: 1.90 M 0 0
change: - x +x +x
equlbm: ~1.9 x x
blah blah blah, calculations ... x = 5.68E-3 . So that would be the acetate concentration before you add the 1E-3 mol H+.
And at that point I'm not sure what to do.