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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If a weak base has the dissociation constant, $K_{b}$ , then the value of the dissociation constant, $K_{a}$ , of its conjugate acid is given by:

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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 105

A water sample from a municipal water supply was found to have a

pH = 7.0

. On evaporating

2 L

of this water,

2.016 g

of white solid was left behind in the evaporation vessel, i.e., the total dissolved solid

(TDS)

content of this water was

1008 mg

L^{- 1}

. However, addition of soap to a bucket of this water did not produce any visible scum. Based on these findings, one can conclude that:

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 106

50 m l

solution of

p H = 1

is mixed with a

50 m l

solution of

p H = 2

. The

p H

of the mixture will be nearly -

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 107

The solubility products

(K_{sp})

of three salts

MX, {MY}_{2}

and

{MZ}_{3}

are

2 \times 10^{- 8}, 8 \times 10^{- 9}

and

54 \times 10^{- 8}

respectively. The correct order for solubilities of these salts is

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 108

If the solubility product of iron

(III)

hydroxide is

1.8 \times 10^{- 37}

, the

pH

of a saturated solution of iron

(III)

hydroxide in distilled water is close to:

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 110

The colour changes of an indicator $Hln$ in acid base titrations is given below,

$HIn (aq) ⇌ H^{+} (aq) + \ln^{-} (aq)$

colour $X$ colour $Y$

Which of the following statements is correct?

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 112

One mole of a sparingly soluble salt

MX

are added in

1 L

saturated solution of another sparingly soluble salt

NX

. If

K_{sp} (MX) > > K_{sp} (NX),

then: (Assume no chemical reaction to be taking place).

HARD

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 113

The solubility of

{CaCO}_{3}

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 %

{Ba}^{+ 2}

has been precipitated as

{BaCO}_{3} .

(Assume no hydrolysis of

{CO}_{3}^{2 -}

ion)

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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).

If a weak base has the dissociation constant, Kb, then the value of the dissociation constant, Ka, of its conjugate acid is given by:

Important Questions on Equilibrium

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If a weak base has the dissociation constant, $K_{b}$ , then the value of the dissociation constant, $K_{a}$ , of its conjugate acid is given by: