###### Question

Complete this table of values for four aqueous solutions at 25°c

# Solution: Complete this table of values for four aqueous solutions at ...

$pH$ is of a solution is found by: $pH=-log[H^{+}]$

$pOH$ of a solution is found by: $pOH=-log[OH^{-}]$

The relationship between $pH$ and $pOH$ is: $pH + pOH = 14$

$[H^{+}] [OH^{-}] = 1.0 x 10^{^{-14}}$

**For solution A:**

The concentration of $[H^{+}]$ given is $7.6x10^{-12}M$

To find $pH$:

$pH=-log[H^{+}] \rightarrow pH=-log[7.6x10^{-12}] \rightarrow pH = 11.12$

To find $pOH$:

$pH + pOH = 14 \rightarrow pOH = 14 - pH \rightarrow pOH = 14-11.12 \rightarrow pOH=2.88$

To find $[OH^{-}]$:

$pOH=-log[OH^{-}] \rightarrow [OH^{-}]=10^{-pOH} \rightarrow [OH^{-}]=1.3x10^{-3}M$

**For solution B:**

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