Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 98

MEDIUM

11th CBSE

IMPORTANT

Earn 100

At $25 ° C$ , the solubility product of ${Hg}_{2} {Cl}_{2}$ in water is $3.2 \times 10^{- 17} {mol}^{3} {dm}^{- 9}$ . What is the solubility of ${Hg}_{2} {Cl}_{2}$ in water at $25 ° C$ ?

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Important Questions on Ionic Equilibrium in Solution

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 99

What is the minimum volume of water required to dissolve

1 g

of calcium sulphate at

298 K . K_{sp}

for

{CaSO}_{4}

is

9.0 \times 10^{- 6}

.

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 100

If the salt

M_{2} X, {QY}_{2} and {PZ}_{3}

have the same solubilities, their

K_{sp}

values are related as

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 101

H_{2} S

gas is passed into one

{dm}^{3}

of a solution containing

0.1

mole of

{Zn}^{2 +}

and

0.01

mole of

{Cu}^{2 +}

till the sulphide ion concentration reaches

8.1 \times 10^{- 19}

moles. Which one of the following statements is true ?

(K_{sp}

of

ZnS and CuS

are

3 \times 10^{- 22}

and

8 \times 10^{- 36}

respectively)

HARD

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 102

Passing

H_{2} S

gas into a mixture of

{Mn}^{2 +}, {Ni}^{2 +}, {Cu}^{2 +} and {Hg}^{2 +}

ions in an acidified aqueous solution precipitates

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11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 103

In presence of

HCl, H_{2} S

results the precipitation of group-2 radicals but not group-4 radicals during qualitative analysis. It is due to

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11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 104

In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains

{Ag}^{+} and {Pb}^{2 +}

at a concentration of

0.10 M

. Aqueous

HCl

is added to this solution until the

{Cl}^{-}

concentration is

0.10 M

. What will be the concentrations of

{Ag}^{+} and {Pb}^{2 +}

at equilibrium ?

(K_{sp}

for

AgCl = 1.8 \times 10^{- 10}

,

K_{sp}

for

{PbCl}_{2} = 1.7 \times 10^{- 5}

)

MEDIUM

11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 105

The

K_{sp}

of

{Ag}_{2} {CrO}_{4}

is

1.1 \times 10^{- 12}

at

298 K

. The solubility (in

mol / L

) of

{Ag}_{2} {CrO}_{4}

in

0.1 M {AgNO}_{3}

solution is

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11th CBSE

IMPORTANT

Pradeep's Chemistry Vol 1>Chapter 9 - Ionic Equilibrium in Solution>Competition Focus>Q 106

Concentration of the

{Ag}^{+}

ions in a saturated solution of

{Ag}_{2} C_{2} O_{4}

is

2.2 \times 10^{- 4} mol L^{- 1}

. Solubility product of

{Ag}_{2} C_{2} O_{4}

is