general chem
posted by Bri on .
A certain monoprotic weak acid with Ka = 0.49 can be used in various industrial processes. (a) What is the [H+] for a 0.191 M aqueous solution of this acid and (b) what is its pH? Round the [H+] to three significant figures and the pH to two places past the decimal and do NOT use scientific notation
how would i do this?

............HA > H^+ + A^
initial..0.191......0.....0
change......x.......x.....x
equil....0.191x....x......x
Ka = (H^+)(A^)(HA) and solve for (H^+), then convert to pH. I expect you will need to use the quadratic equation but perhaps not.