I can't figure out how to make an equilibrium table when 550 mL of .10 M KF are mixed with 450 mK .10 M HF?

Thank you.

I don't quite understand what you mean by 'equilibrium table'. Perhaps you can post an example of one you know.

The equations are:

HF \rightleftharpoons H^+ + F^-

KF \rightarrow K^+ + F^-

There is a common ion effect of fluoride ions, which makes the equilibrium of the reversible reaction shift to the left. As a result, the HF is less soluble.

Post an example you have done, or the teacher gave you. It'll help me understand what you are asking exactly.