How do you find the pH of a solution with a known pKa and Molarity?
Do you know the formula:

$$K_\text{a} = \frac{[\ce{H+}][\ce{A-}]}{[\ce{HA}]}$$

?

You will need to find a concentration first, however, on the equation.

$$\ce{HA &lt;=&gt; H+ + A-}$$

And solve for the dissociated hydrogen ion, say $x$.

$$K_\text{a} = \frac{[x][x]}{[\ce{HA}]-x} = \frac{x^2}{[\ce{HA}]-x}$$

The logic is: if $x$ of $\ce{HA}$ dissociated, then we would get $x$ of $\ce{H}$, $x$ of $\ce{A}$ and $[\ce{HA}]-x$ left of $[\ce{HA}]$.

Does this make sense?