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Posted by on Sunday, March 25, 2012 at 8:28pm.

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?

  • general chem - , Sunday, March 25, 2012 at 10:17pm

    ............HA --> H^+ + A^-
    initial..0.191......0.....0
    change......-x.......x.....x
    equil....0.191-x....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.

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