Question

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.
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.

Related Questions

At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4×103. The ini... The reaction below is at dynamic equilibrium. N₂(g) + 3H₂(g) <——>2NH3(g) Which statement is true f... write this in a short sentence Diffusion is the process by which molecules move from an area of h... write this in a short sentence Diffusion is the process by which molecules move from an area of h...