Upon titration a solution of Ethylene diamine K b 1 = 8 × 10 - 5 ; K b 2 = 2 . 7 × 10 - 8 with HCl solution, pH value of solution at I st equivalence point depends upon:

Initial concentration of weak base solution.

Initial concentration of strong acid solution.

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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Upon titrating a solution of weak monoprotic acid with a weak monoacidic base solution, at equivalence point:

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Important Questions on Equilibrium

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 93

The total number of different kind of buffers obtained during the titration of

H_{3} {PO}_{4}

with

NaOH

are :

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 94

Upon titration a solution of Ethylene diamine

(K_{b_{1}} = 8 \times 10^{- 5}; K_{b_{2}} = 2.7 \times 10^{- 8})

with

HCl

solution,

pH

value of solution at

I^{st}

equivalence point depends upon:

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 95

What can be the maximum concentration of equimolar solutions of ferrous sulphate

({FeSO}_{4})

and sodium sulphide

({Na}_{2} S),

so that when mixed in equal volumes, there is no precipitation of iron sulphide (

FeS

) (For iron sulphide,

K_{sp} = 6.25 \times 10^{- 18}

) Assume no ion to be undergoing hydrolysis.

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 103

Solubility product of silver chloride and silver thiocyanate are

1.2 \times 10^{- 10}

and

7.1 \times 10^{- 13}

respectively. The equilibrium constant for the reaction

AgCl (s) + {CNS}^{- 1} (aq) ⇌ AgCNS (s) + {Cl}^{- 1} (aq)

is:

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Alpha Question Bank for Engineering: Chemistry>Chapter 5 - Equilibrium>Exercise-2>Q 104

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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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

Upon titrating a solution of weak monoprotic acid with a weak monoacidic base solution, at equivalence point:

Important Questions on Equilibrium

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