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

Byju's Answer

Standard XI

Mathematics

Harmonic Progression

What is the m...

Question

What is the minimum $p H$ required to prevent the precipitation of $Z n S$ in a solution that is $0.01$ $M Z n C l_{2}$ and saturated with $0.10 M H_{2} S$ ?
[Given : $K_{s p} = 10^{- 21}, K_{a_{1}} \times K_{a_{2}} = 10^{- 20}]$

0.0

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

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!

Open in App

Solution

The correct option is B 1
$K_{s p} = [Z n^{2 +}] [S^{2 -}]$
$[S^{2 -}] = \frac{10^{- 21}}{0.01} = 10^{- 19}$
for $K_{a_{2}} \times K_{a_{2}} = \frac{[H^{+}]^{2} [S^{2 -}]}{[H_{2} S]}$
$10^{- 20} = \frac{[H^{+}]^{2} \times 10^{- 19}}{0.1} \Rightarrow [H^{+}] = 0.1$
Or $p H = 1$

Suggest Corrections

Similar questions

Q. What is the minimum

p H

required to prevent the precipitation of

Z n S

in a solution that is

0.01 M Z n C l_{2}

and saturated with

0.10 M H_{2} S

(K_{s p} o f Z n S = 10^{- 21}, K_{a_{1}} \times K_{a_{2}} o f H_{2} S = 10^{- 20})

The minimum pH required to prevent the precipitation of ZnS in a solution containing 0.01 M $Z n C l_{2}$ and saturated with 0.10 $M H_{2} S$ is

(Given $K s p (Z n S) = 10^{- 21}, K a_{1} \times K a_{2} o f H_{2} S = 10^{- 20}$ )

Q. An acidified solution of

0.05 M Z n^{2 +}

is saturated with

0.1 M H_{2} S

. What is the minimum molar concentration

(M)

H^{+}

required to prevent the precipitation of

Z n S

?
Use

K_{S P} (Z n S) = 1.25 \times 10^{- 22}

and overall dissociation constant of

H_{2} S

K_{N E T} = K_{1} K_{2} = 1 \times 10^{- 21}

Q. Calculate the potential of a half cell having reaction:

A g_{2} S (s) + 2 e^{-} ⇌ 2 A g (s) + S^{2 -} (a q)

in a solution buffered at

p H = 3

and which is also saturated with

0.1 M H_{2} S (a q) :

[Given:

K_{s p} (A g_{2} S) = 10^{- 49}, K_{a_{1}} . K_{a_{2}} = 10^{- 21}

]

An aqueous solution of a metal bromide $M B r_{2}$ of $0.05 M$ is saturated with $H_{2} S$ . What is the minimum $p H$ at which $M S$ will precipitate? Given $K_{s p}$ of $M S$ = $6.0 \times 10^{- 21}$ . Concentration of saturated $H_{2} S$ = $0.1 M$ ( $K_{1}$ of $H_{2} S$ = $10^{- 7}$ and $K_{2}$ = $1.3 \times 10^{- 1} C$ )

Join BYJU'S Learning Program

What is the minimum pH required to prevent the precipitation of ZnS in a solution that is 0.01 M ZnCl2 and saturated with 0.10M H2S? [Given : Ksp=10−21,Ka1×Ka2=10−20]

The correct option is B 1Ksp=[Zn2+][S2−] [S2−]=10−210.01=10−19 for Ka2×Ka2=[H+]2[S2−][H2S] 10−20=[H+]2×10−190.1⇒[H+]=0.1 Or pH=1

What is the minimum $p H$ required to prevent the precipitation of $Z n S$ in a solution that is $0.01$ $M Z n C l_{2}$ and saturated with $0.10 M H_{2} S$ ?
[Given : $K_{s p} = 10^{- 21}, K_{a_{1}} \times K_{a_{2}} = 10^{- 20}]$

The correct option is B 1
$K_{s p} = [Z n^{2 +}] [S^{2 -}]$
$[S^{2 -}] = \frac{10^{- 21}}{0.01} = 10^{- 19}$
for $K_{a_{2}} \times K_{a_{2}} = \frac{[H^{+}]^{2} [S^{2 -}]}{[H_{2} S]}$
$10^{- 20} = \frac{[H^{+}]^{2} \times 10^{- 19}}{0.1} \Rightarrow [H^{+}] = 0.1$
Or $p H = 1$