chemistry

A 0.25 mol/L solution of benzoic acid, KC7H5O2 and antiseptic also used as a food preservative, has a pH of 2.40. Calculate the Ka of benzoic acid at SATP

My work:

C6H5COOH --> C6H5COO^- + H^+

Ka = (C6H5COO-)(H+)/ C6H5COOH

I know my next steps are to use pH = log(H+) to calculate H+

and then

substitute into Ka expression and determine Ka

How to do this?

Thanks in advance

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asked by Dustin
  1. pH = 2.40
    pH = -log(H+)
    -log(H^+) = 2.40
    log(H^+) = -2.40
    plug -2.40 into your calculator and hit the 10x key to obtain 0.00398. check my work.

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    posted by DrBob222
  2. 0.003898-- this is H+?

    Ka = ( )(0.00398)/( )

    What would be the concentration of C6H5COO- ?

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    posted by Ross
  3. Look at the equation.
    C6H5COOH ==> C6H5COO^- + H^+
    For every 1 mol C6H5COOH that ionizes, you get 1 mol C6H5COO^- and 1 mol H^+. So they are the same.

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    posted by DrBob222
  4. I get 4.0 x 10^-3 but im incorrect

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    posted by Kelsy
  5. No.
    (0.00398)^2/(0.25-0.00398) =
    6.44 x 10^-5

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