A solution has a [H^+] of 1.0times 10^-5M 6. What is its [OH^-] 7. What is its pH? 8. What is its POH?

6. To find the concentration of hydroxide ions $[OH^{-}]$, we can use the ion product constant for water, $K_w$, which is $1.0\times 10^{-14}$ at 25°C. The relationship between $[H^{+}]$ and $[OH^{-}]$ is given by the equation $[H^{+}][OH^{-}] = K_w$. Rearranging the equation, we get $[OH^{-}] = \frac{K_w}{[H^{+}]}$. Substituting the given value of $[H^{+}]$, we have $[OH^{-}] = \frac{1.0\times 10^{-14}}{1.0\times 10^{-5}} = 1.0\times 10^{-9}M$.<br /><br />7. The pH of a solution is defined as the negative logarithm of the hydrogen ion concentration: $pH = -\log[H^{+}]$. Substituting the given value of $[H^{+}]$, we have $pH = -\log(1.0\times 10^{-5}) = 5$.<br /><br />8. The pOH of a solution is defined as the negative logarithm of the hydroxide ion concentration: $pOH = -\log[OH^{-}]$. Substituting the calculated value of $[OH^{-}]$, we have $pOH = -\log(1.0\times 10^{-9}) = 9$.