Question

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

Answer 1

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

Answer 2

0.003898-- this is H+?

Ka = ( )(0.00398)/( )

What would be the concentration of C6H5COO- ?

Answer 3

Look at the equation.
C6H5COOH ==> C6H5COO^- + H^+
For every <b>1 mol C6H5COOH</b> that ionizes, you get <b>1 mol C6H5COO^-</b> and <b> 1 mol H^+</b>. So they are the same.

Answer 4

I get 4.0 x 10^-3 but im incorrect

Answer 5

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