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The pH of a solution containing 0.4 M HC...

The pH of a solution containing 0.4 M `HCO_(3)^(-)` and 0.2 M `CO_(3)^(2-)` is :
`[K_(a1)(H_(2)CO_(3))=4xx10^(-7)` , `K_(a2)(HCO_(3)^(-))=4xx10^(-11)]`

A

`10.4`

B

`10.1`

C

`6.1`

D

`10.7`

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The pH of the a solution containing 0.4 M HCO_(3)^(-) is : [K_(a_(1)) (H_(2)CO_(3)) = 4 xx 10^(-7), K_(a_(2)) (HCO_(3)^(-)) = 4 xx 10^(-11)]

In a solution containing 0.02M CH_(3)COOH and 0.01M C_(6)H_(5)COOH . If K_(CH_(3)COOH) and K_(C_(6)H_(5)COOH) are 1.8xx10^(-5) and 6.4xx10^(-5) respectively, then calculate the pH of solution.

50 ml, 0.1M NaHCO_(3) aqueous solution is mixed with 50 ml, 0.8 M Na_(2)CO_(3) aqueous solution at 25^(@)C . The pH of resulting solution exiists between colour transition range of an indicator which is: (K_(a_(1))=4xx10^(-7), K_(a_(2)) =2xx10^(-11) "for" H_(2)CO_(3))

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