Naked Science Forum
Non Life Sciences => Chemistry => Topic started by: danica_aku on 16/05/2006 11:59:15
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What is the pH of 0.100 M sodium phenolate, C6H5ONa, the sodium salt of phenol?[xx(][xx(][xx(]
Please help me...
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Henderson Hasselbach Equation-
pH = pKa - log ([HA] / [A-])
HA would be the OH form
and A- would be the O- form
0.100 mols/ liter of phenolate anion (O- form) from dissolving the salt
look up Pka of phenol
pH = -log [H+]
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tnx a lot![:)]
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H-H doesn't work for this problem. You need to be near the buffer region, where the phenoxide and phenol concentrations are within a couple orders of magnitude.
For this problem, you first need to calculate pKb of phenoxide, then Kb, then make an ICE table for the reaction:
NaC6H5O + H2O <==> HC6H5O + NaOH
I 0.100 0 0
C -x +x +x
-------------------------------------
E 0.100-x x x
~0.100
Kb = [HC6H5O][NaOH]/[NaC6H5O] = x^2/0.1
x = [OH-]
Once you find [OH-], you should be able to find pH pretty easily.
DrDick