CameraIcon

SearchIcon

MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Properties of Water

The pH of 1 M...

Question

The pH of $1 M P O_{4}^{3 -}$ (aq) solution is:
[Given $p K_{b} (P O_{4}^{3 -}) = 1.62]$

A

13.19

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

B

1.62

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

C

8.1

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

D

4.86

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 $p K_{b} (P O_{4}^{3 -}) = 1.62], [P O_{4}^{3 -}] = 1 M$ $P O_{4}^{3 -} + H_{2} O ⇌ H P O_{4}^{2 -} + O H^{-}$
$[O H^{-}] = \sqrt{K_{b} C}$
we know
$p O H = \frac{1}{2} [p K_{b} - l o g C]$
$p O H = \frac{1}{2} [1.62 - l o g 1] = 0.81$
Also,
$p H = 14 - p O H$
$p H = 14 - 0.81 = 13.19$

Suggest Corrections

thumbs-up

1

Similar questions

Q. Calculate pH of

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

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

p H

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

in aqueous solution. Given

p K_{b} o f P O_{4}^{3 -} = 1.62

.

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

(aq) solution is:
[Given

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

p H

of a solution of

N H_{4} C l

is 4.86. calculate the molar concentration of the solution if

K_{b} = 1.0 \times 10^{- 5}

K_{w} = 1.0 \times 10^{- 14}

N a C l (a q)

is electrolysed. The

p H

of solution after electrolysis will

View More

Join BYJU'S Learning Program

explore_more_icon

Explore more

Properties of Water

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon