Homework Help: Chemistry

Posted by sh on Thursday, June 3, 2010 at 1:49pm.

Consider the following buffer equilibrium:
HF (high concentration) + H2O <--> H3O+ (low concentration) + F- ( high concentration)
Using Le Chatelier's Principle, explain what happens to the pH of the buffer solution when a small amount of NaOH is added.

Wouldn't OH- react with HF to form water? But they're both on the reactants side.

Chemistry - DrBob222, Thursday, June 3, 2010 at 5:32pm
I'm not sure of what your symbols mean. HF by itself is not a buffer; however, HF in combination with its salt (NaF) is a buffer and your designation of high concn and low concn may be intended to show that. If NaOH is added, it reacts with the H3O^+, and removing H3O^+ shifts the equilibrium to the right to create more H3O^+ to replace that which was removed. The pH will not change much.

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