Calculate the ratio of concentration of `HCOO^(-) & OCN^(-)` ions in a solution containing `0.1MHCOOH (K_(a)=1.8xx10^(-4))` and `0.1MHOCN(K_(a_(1))=4x

Question

Calculate the ratio of concentration of `HCOO^(-) & OCN^(-)` ions in a solution containing `0.1MHCOOH (K_(a)=1.8xx10^(-4))` and `0.1MHOCN(K_(a_(1))=4x

Calculate the ratio of concentration of `HCOO^(-) & OCN^(-)` ions in a solution containing `0.1MHCOOH (K_(a)=1.8xx10^(-4))` and `0.1MHOCN(K_(a_(1))=4xx10^(-4))` .if simplest ratio is `a:b` reprot your answer as `(a+b)`.

Monjur Alahi

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2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Salim Ahmed Kawsar

`[H^(+)]` is the same for equilibria of both acids.
Now ,let `[HCOO^(-)]=aM` and `[OCN^(-)]=b M`
`:.([H^(+)]xxa)/(0.1)=1.8xx10^(-4)&([H^(+)]xxb)/(0.1)=4xx10^(-4)rArr (a)/(b)=(9)/(20)` So `(a+b)=29`

4 views Answered 2023-02-05 15:29