Tuesday

July 22, 2014

July 22, 2014

Posted by **Annie** on Saturday, June 7, 2014 at 8:18pm.

when i did it i did -log(1.0) but that is just 0 so what it the procedure to do this question

Calculate the pH of a 1.0 mol/L aqueous solution of sodium benzoate. Note: Only the benzoate ion affects the pH of the solution.

- Chemistry -
**DrBob222**, Saturday, June 7, 2014 at 11:22pmBenzoate ion hydrolyzes in water to form a solution that is not neutral.

If we call the benzoate ion Bz^-, then

.........Bz^- + HOH ==> HBz + OH^-

I........1.0..............0.....0

C........-x..............x.....x

E.......1-x..............x......x

Kb for Bz^- = (Kw/Ka for HBz) = x*x/(1-x) and solve for x = (OH^-),then convert to pH.

HBz is benzoic acid. You can find Ka for HBz in you text/notes I'm sure but it's approx 10^-5.

- Chemistry -
**Annie**, Saturday, June 7, 2014 at 11:38pmthanks

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