Calculate the equilibrium constant, Ka for the acid, HA if, at equilibrium, the pH of a 1.85 M solution of HA is 3.13?
I know that:
Use pH = -log [H+] first and solve for [H+].
Then use Ka = [H+][A-]/[HA] to solve for Ka.
[A-] = [H+]
[HA] is given in the problem.
I keep getting it wrong, any ideas??
Calculate the equilibrium constant, Ka for the acid, HA if, at equilibrium, the pH of a...
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