To a solution formed by adding n mole of sparingly soluble salt MX in 1 L water, NaY solid (a readily soluble salt) is added until x % of MX is converted to MY ( s ) (another sparingly soluble salt). Then: (Assume no hydrolysis of any ion).

Resulting solution can be called saturated with respect to both MX and MY .

Y - = K sp ( MY ) K sp ( MX ) × nx 100

The exothermic formation of ClF 3 is represented by the following equation: Cl 2 g + 3 F 2 g ⇌ 2 ClF 3 g ; ΔH = - 329 kJ Which of the following will increase the quantity of ClF 3 in the equilibrium mixture of Cl 2 , F 2 and ClF 3 ?

Increasing the volume of the container.

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IMPORTANT

Earn 100

The solubility of ${CaCO}_{3}$ is $7 mg / litre$ . Calculate the solubility of ${BaCO}_{3}$ (in $mol / L$ ) from this information and from the fact that when ${Na}_{2} {CO}_{3}$ is added slowly to a solution containing equimolar concentration of ${Ca}^{+ 2}$ and ${Ba}^{+ 2},$ no precipitate of ${CaCO}_{3}$ is formed until $90 %$ of ${Ba}^{+ 2}$ has been precipitated as ${BaCO}_{3} .$ (Assume no hydrolysis of ${CO}_{3}^{2 -}$ ion)

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Important Questions on Equilibrium

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 114

To a solution formed by adding

n

mole of sparingly soluble salt

MX

1 L

water,

NaY

solid (a readily soluble salt) is added until

x %

MX

is converted to

MY (s)

(another sparingly soluble salt). Then: (Assume no hydrolysis of any ion).

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 118

What maximum $pH$ must be maintained in a saturated $H_{2} S$ solution $(0.1 M)$ to avoid precipitation of both ${Mn}^{2 +} and {Fe}^{2 +}$ from a solution, in which each ion is present at a concentration of $0.01 M ?$

$(K_{a}$ of $H_{2} S = 9.6 \times 10^{- 21}; K_{sp}$ of $MnS = 2.5 \times 10^{- 13}; K_{sp}$ of $FeS = 6.4 \times 10^{- 18})$

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 119

What minimum $pH$ must be maintained in a saturated $H_{2} S$ solution $(0.1 M)$ to avoid precipitation of both ${Mn}^{2 +} and {Fe}^{2 +}$ from a solution, in which each ion is present at a concentration of $0.01 M ?$

$(K_{a}$ of $H_{2} S = 9.6 \times 10^{- 21}; K_{sp}$ of $MnS = 2.5 \times 10^{- 13}; K_{sp}$ of $FeS = 6.4 \times 10^{- 18})$

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 120

A decimolar solution of

HCl

is saturated with

H_{2} S

gas. Calculate the minimum

[{Cu}^{2 +}]

ion that will saturate the above solution with

CuS

. Given

K_{sp}

CuS = 6.4 \times 10^{- 36}, K_{a}

for

H_{2} S = 9.6 \times 10^{- 21}

and solubility of

H_{2} S = 0.1 mole {litre}^{- 1}

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 131

0.98 g H_{3} {PO}_{4}

is dissolved in

100 mL

a buffer solution

(pH = 5) .

If the equilibrium concentrations of

H_{2} {PO}_{4}^{-}, {HPO}_{4}^{2 -}, {PO}_{4}^{3 -}

and

H_{3} {PO}_{4}

are

C_{1}, C_{2}, C_{3}

and

C_{4}

respectively. Find

{pC}_{1} + {pC}_{2} + {pC}_{3} + {pC}_{4} ({pC}_{i} = - {logC}_{i};

where

i = 1, 2, 3, 4)

Given: For

H_{3} {PO}_{4}, K_{a_{1}} = 10^{- 3}, K_{a_{2}} = 10^{- 8}, K_{a_{9}} = 10^{- 12}

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 134

On addition to

V mL

volume of

0.1 M KOH

, buffer capacity is found maximum at

{pH}_{solution} = x (> 7)

when it is titrated against

50 mL, 0.2 M H_{2} {CO}_{3} .

For

(H_{2} {CO}_{3} : K_{a_{1}} = 4.3 \times 10^{- 6}, K_{a_{2}} = 5.6 \times 10^{- 11})

Report your answer as

(V + x) \times 0.4,

rounding it off to the nearest whole number.

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 135

The solubility product of ${Ag}_{2} C_{2} O_{4}$ at $25 ° C$ is $1.29 \times 10^{- 11} {mol}^{3} L^{- 3} .$ A solution of $K_{2} C_{2} O_{4}$ containing
$0.152$ mole in $500 mL$ water.is shaken with an excess of ${Ag}_{2} {CO}_{3}$ till the following equilibrium is reached:

${Ag}_{2} {CO}_{3} (s) + K_{2} C_{2} O_{4} (aq) ⇌ {Ag}_{2} C_{2} O_{4} (s) + K_{2} {CO}_{3} (aq)$ .

At equilibrium, the solution contains $0.0358$ mole of $K_{2} {CO}_{3}$ . Assuming the degree of dissociation of $K_{2} C_{2} O_{4}$ and $K_{2} {CO}_{3}$ to be equal, if the solubility product of ${Ag}_{2} {CO}_{3}$ is $3.794 \times 10^{- x} {mol}^{3} L^{- 3}$ , find $x .$

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IMPORTANT

Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 137

0.1

millimole of

{CdSO}_{4}

are present in

10 mL

acid solution of

0.08 M HCI

. Now

H_{2} S

is passed to precipitate all the

{Cd}^{2 +}

ions. Find the

pOH

of the solution after filtering off precipitate, boiling off

H_{2} S

and making the solution

100 mL

by adding

H_{2} O .

Important Questions on Equilibrium

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