## Chemistry: Molecular Approach (4th Edition)

pOH is defined as the negative of the log (base 10) of the hydroxide ion concentration: $$pOH = -log[OH^-]$$ Acidic solution: $pOH \gt 7$ Neutral solution: $pOH = 7$ Basic solution: $pOH \lt 7$
See definition of pOH on the bottom of page 735. Knowing that $pH + pOH = 14$, and acidic solutions have $pH \lt 7$: $$pH = 14 - pOH$$ $$14 - pOH \lt 7$$ $$14 - 7 \lt pOH$$ $$7 \lt pOH$$ $$pOH \gt 7$$ For neutral solutions: pH = 7: $$pH + pOH = 14$$ $$7 + pOH = 14$$ $$pOH = 14 - 7 = 7$$ For basic solutions: pH $\gt$ 7: $$pH + pOH = 14$$ $$pH = 14 - pOH$$ $$14 - pOH \gt 7$$ $$14 - 7 \gt pOH$$ $$7 \gt pOH$$ $$pOH \lt 7$$