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A certain weak acid has a dissociation c...

A certain weak acid has a dissociation constant `1.0xx10^(-4)`. The equilibrium constant for its reaction with a strong base is :

A

`10^(9)`

B

`10^(10)`

C

`10^(11)`

D

`10^(12)`

Text Solution

Verified by Experts

`underset("weak")(HA)+BOH Leftrightarrow BA+ underset("strong")(H_(2)O)`
`or HA+B^(+)+OH^(-) Leftrightarrow B^(+)+A^(-)+H_(2)O or HA+OH^(-) Leftrightarrow A^(-)+H_(2)O` `therefore K=([A^(-)])/([HA][OH^(-)])`
Also for weak acid HA
`HA Leftrightarrow H^(+)+A^(-)`
`K_(a)=([H^(+)][A^(-)])/([HA])`
`K_(a)/K=K_W or K=K_a/K_w =(10^(-4))/(10^(-14))=10^10`
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