Buffer problems?.....?
Sodium benzoate, C6H5COONa, is the salt of the weak acid,benzoic acid,C6H5COOH.A .10 molar solution of sodium benzoate has a pH of 8.6 at room temp.
1. Calculate the [OH-] in the sodium benzoate solution
2.calculate the value for the equilibrium constant for the reaction:C6H5COO- +H2O <-----> C6H5COOH +OH-
3. Calculate the value of Ka,the acid dissociation constant for benzonic acid.
Thanks for your help
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Verified answer
Use an ICE table.
You know you initially have 0.10M C6H5COO-, and [C6H5COOH] = [OH-] 0.
Treat the pH value of 8.6 as your "change" (Δ) part of the (R)ICE table. From that change, you should be able to reflect the "change" value to your C6H5COOH and OH-, and calculate the final equilibrium concentrations for all three compounds. From there, just complete your other questions.
For #1, just remember pH = 14 - pOH and [OH-] = 10^(-pOH)
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