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The ionization constant of a certain wea...

The ionization constant of a certain weak acid is `10^(-4)`. What should be the [salt] to [acid] ratio if we have to prepare a buffer with `pH = 5` using this acid and one of the salts

A

`1:10`

B

`10:1`

C

`5:4`

D

`4:5`

Text Solution

Verified by Experts

The correct Answer is:
B
`pH = - log K_(b) + log. (["salt"])/(["acid"])`
` 5 = - log 10^(-4) + log . (["salt"])/(["acid"])`
`log . (["salt"])/(["acid"]) = 1 `
` (["salt"])/(["acid"])="antilog" 1 = 10 : 1 `
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