Given the concentration of a weak base solution and a K _{b} value for the weak base, what is the correct procedure to determine the pH of the solution?

A. Set concentration of weak base equal to [OH ^{-}], convert to [H_{3}O^{+}] and solve for pH

B. Convert K_{b} to K_{a} and use a table to find the equilibrium concentration of [H _{3}O^{+}] and solve for pH

C. Convert K_{b} to K_{a} and use pH = pK_{a} + log(base / acid)

D. Use a table to find the equilibrium concentration of the conjugate acid which is equal to [H _{3}O^{+}] and solve for pH

E. Use a table to find the equilibrium concentration of [OH ^{-}], convert to [H_{3}O^{+}] and solve for pH

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