Equal volumes of following solutions are mixed. In which case the pH of resulting solution will be average value of pH of two solutions?
Equal volumes of following solutions are mixed. In which case the pH of resulting solution will be average value of pH of two solutions?
A. Aqueous `HCl` of `pH=2` aqueous `NaOH` of `pH=12`
B. Aqueous `HCl` of `pH=2`, aqueous `HCl` of `pH=4`.
C. Aqueous `HCl` of `pH=2` aqueous `NaOH` of `pH=10`
D. Aqueous `CH_(3)COOH` of `pH=5` aqueous `NH_(3)` of `pH=9.[K_(a)(CH_(3)COOH)=K_(b)(NH_(3))]`
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(A) `[H^(+)]=10^(-2)` and `[OH^(-)]=10^(-2)`
`H^(+)+OH^(-)rArr H_(2)O`
This leads complete neutraltisation.
so `pH=7=(2+12)/(2)`
(D) `[H^(+)]=10^(-5)` and `[OH^(-)]=10^(-5)`
`[H^(+)]+[OH^(-)]=H_(2)O`
This leads complete neutralisation.
so `pH=7=(5+9)/(2)`
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