(assuming that the solution is at 
, under which 
.)![{\rm [H^{+}]}](/tpl/images/1343/6413/ad601.png)
and ![{\rm [OH^{-}]}](/tpl/images/1343/6413/6cc4a.png)
denote the concentration of 
and 
respectively.
denote the self-ionization constant of water. The exact value of 
depends on the temperature of the solution. 
at 
, or moles per liter, as the unit) is supposed to be equal to the ![{\rm [H^{+}]} \cdot {\rm [OH^{-}]} = K_{\rm w}](/tpl/images/1343/6413/10f13.png)
.![{[\rm OH^{-}]}](/tpl/images/1343/6413/e07bd.png)
:![\begin{aligned}{\rm [OH^{-}]} &= \frac{K_{\rm w}}{[\rm H^{+}]}\end{aligned}](/tpl/images/1343/6413/c0cdc.png)
.![\begin{aligned}{\rm [OH^{-}]} &= \frac{K_{\rm w}}{[\rm H^{+}]} \\ &= \frac{10^{-14}}{2.6 \times 10^{-6}}\approx 3.85\times 10^{-9}\; \rm M\end{aligned}](/tpl/images/1343/6413/660c1.png)
.
of this solution would be:![\begin{aligned}\rm pOH &= -\log_{10}{\rm [OH^{-}]} \\&\approx -\log_{10} (3.85 \times 10^{-9}) \approx 8.41 \end{aligned}](/tpl/images/1343/6413/17241.png)
.What is the pOH of a
2.6 x 10-6 M H+ solution?...
Answers: 3
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