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Enough of a monoprotic acid is dissolved in water to produce a 0.0195 M solution. The pH of the resulting solution is 6.24. Calculate the Ka for the acid.

Also, the answer is not 1.7 * 10 ^ -11

The response is: You treated the initial concentration as 0. In this case, the initial 10^-7 M H+ from water is not negligible. If [H+]initial = 10 ^ -7 and [H+]final = 5.8 * 10^-7, by how much did the concentration change? What does that say about how much A- was produced?

  • Chemistry -

    nevermind, I figured it out

  • Chemistry -

    you figured it out then what was the solution how did you solve it then because others are having the same problems and the same errors

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