Home
Class 11
CHEMISTRY
A buffer solution contains 0.20 mole of ...

A buffer solution contains `0.20` mole of `NH _(4)` OH and `0.25` mole of `NH _(4) Cl` per litre. Calculate the pH of the solution . Dissociation constant of `NH _(4) OH at 29^(@) C ` is `1.81 xx 10 ^(-5).`

Text Solution

Verified by Experts

Here, `pK _(b) = - log K _(b) =- log (1. 81 xx 10 ^(-5)) = 4.7423`
`pOH = p K _(b) + log ""(["Salt"])/(["Base"]) implies pHO = 4. 7423 + log "" (0.25)/(0.20) = 4. 839`
`pH = 14 - 4.839= 9.161`
Promotional Banner

Similar Questions

Explore conceptually related problems

50 ml of 0.2 M NH_(4)OH and 50 ml of 0.2 M HCl solutions are Mixed. pH of the resulting solution is (Given Kb of NH_(4)OH=1 times 10^(-5) )

Calcualte the pH of a solution containing 4.9 g of sulphuric acid per litre.

Calulate the pH of the buffer solution formed by mixing 0.2M NH_4Cl and 0.1M NH_3K_b of ammonia is 1.77xx10^(-5)

A solution is prepared by taking 0 . 4 M CH_(3) CO OH and 0.4 M CH_(3) CO ON a per litre of the solution . What is pH of the solution ? (K_(a) = 1. 0 X 10^(-5))

solution contains 1 mole of alcohol and 4 moles of water. The möle fraction of water and alcohol will be

The pKb value of NH_(4)OH at 298 K is 4.75. An aq. Solution of NH_(4)OH is titrated against HCl. The pH of the solution when half of the NH_(4)OH has been neutralized as