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A basic buffer contains 0.8 mole of NH(4...

A basic buffer contains `0.8` mole of `NH_(4)Cl` and `0.2` mole of `NH_(4)OH` for litre of a solution the `K_(b)` of base is `1.8 xx 10^(-5)`. Then the `P^(H)` of the buffer solution is `(log 1.8 = 0.2553)`

A

`8.6532`

B

`6.345`

C

`2.301`

D

`7.635`

Text Solution

Verified by Experts

The correct Answer is:
A
`P^(H) = 14 - P^(k_(b)) - "log" (["salt"])/(["Base"])`
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