Chemistry

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If the Ka of a monoprotic weak acid is 4.5x10^-6 what is the pH of a .10M solution of this acid.

I don't even know how to start this problem, I'm totally lost please help!

  • Chemistry -

    Step 1. Write and balance the equation.
    Step 2. Complete the ICE chart (initial, change. equilibrium).
    Step 3. Write the Ka expression.
    Step 4. Substitute the E line of the ICE chart into Ka expression and solve for the unknown.

    .........HA ==> H^+ + A^-
    I........0.1....0......0
    C........-x.....x......x
    E......0.1-x....x......x

    Ka = (H^+)(A^-)/(HA)

    4.5E-6 = (x)(x)/(0.1-x)
    Solve for x = (H^+), then convert to pH.

  • Chemistry -

    ph=10.3

  • Chemistry -

    The pH is not 10.3

  • Chemistry -

    I got that the pH equals 2.67 is this number correct?

  • Chemistry -

    I don't get 2.67. If you will show your work I will find the error. I agree the answer isn't 10.3.

  • Chemistry -

    The correct pH is 3.17

  • Chemistry -

    3.17 is correct.

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