What is the pH of a mixture of $ 1.0 \; L \ NaOH \; 1.0 \; \frac{mol}{L} $ with $ 1.0 \; L \; HCl \; 1.0 \; \frac{mol}{L} $? Write the (nonionic) equation of the reaction!
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$NaOH+HCl \rightarrow NaCl+H_2O$
Completer the following table:
| $NaOH$ | + | $HCl$ |  |
$NaCl$ | + | $H_2O$ | |
| initial nb. of moles | 1.0 | 1.0 | 0 | 0 | |||
| variation of moles nbs | ........ | ........ | ........ | ||||
| final nb. of moles | ........ | ........ | ........ |
| $NaOH$ | + | $HCl$ | |
$NaCl$ | + | $H_2O$ | |
| initial nb. of moles | 1,0 | 1,0 | 0 | ||||
| variation of moles nbs | -1.0 | -1.0 | +1.0 | ||||
| final nb of moles | 0.0 | 0.0 | 1.0 |
Write the substances present at the end with their molarities !
$[NaCl]=\frac{1.0}{2.0}=0.5\frac{mol}{L}$
What is the final pH?
The two ions $ Na^+ $ and $ Cl^- $ formed by dissociation of $ NaCl $ have no influence on the pH, so the pH is that of pure water: $pH=7.0$
