Calculate $p H$ of $1.0 M P O_{4}^{3 -}$ in aqueous solution. Given $p K_{b} o f P O_{4}^{3 -} = 1.62$ .

13.19

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

No worries! We‘ve got your back. Try BYJU‘S free classes today!

6.5

No worries! We‘ve got your back. Try BYJU‘S free classes today!

11.5

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A 13.19
Given, $[P O_{4}^{3 -}] = 1 M$
$p K_{b} (P O_{4}^{3 -}) = 1.62$
$P O_{4}^{3 -}$ in aqueous solution gives $O H^{-}$ ion, hence from ostwald's dilution law
$[O H^{-}] = \sqrt{K_{b} . C}$
the relation between $P O H$ and $P k_{b}$ is given by
$P O H = \frac{1}{2} [P k_{b} - log C]$
putting the value of $P k_{b}$ and C we get,
$\Rightarrow P O H = \frac{1}{2} [1.62 - log 1] = 0.81$
Also,
$p H = 14 - p O H = 14 - 0.81 = 13.19$
Hence, pH of $P O_{4}^{3 -}$ in aqueous solution is 13.19

Suggest Corrections

Similar questions

Q. The pH of

1 M P O_{4}^{3 -}

(aq) solution is:
[Given

p K_{b} (P O_{4}^{3 -}) = 1.62]

Q. What is the pH of a 0.5 M aqueous NaCN solution ?

{pK}_{b} of {CN}^{-}

is 4.70.

Q. Calculate pH of an aqueous solution of 1M

H C O O N H_{4}

assuming complete dissociation.

p K_{a} (H C O O H) = 3.8 a n d p K_{b} = 4.8

Calculate the pH of an aqueous solution of $1.0 M$ ammonium formate assuming complete dissociation. ( $p_{K a}$ of formic acid = 3.8 and $p_{K b}$ of ammonia = 4.8)

Q. Calculate the pH of an aqueous solution of

1 M

ammonium formate, assuming complete dissociation.

(p K_{a} = 3.8, p K_{b} = 4.8)

Join BYJU'S Learning Program

Explore more

Ostwald Dilution Law

Standard XII Chemistry

Join BYJU'S Learning Program

Calculate pH of 1.0 M PO3−4 in aqueous solution. Given pKb of PO3−4=1.62.

Calculate $p H$ of $1.0 M P O_{4}^{3 -}$ in aqueous solution. Given $p K_{b} o f P O_{4}^{3 -} = 1.62$ .