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Ionic Equilibria

Question
ICSEENICH12028864
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(i)Give Lewis’ definition for acids and bases.    

(ii) The solubility of Ag2CrO4 at 25°C is 8.0 x 10-5 moles /litre. Calculate its solubility product.

Solution

i) Lewis acid: A compound or an ionic species which can accept a pair of electron known as lewis acid.
Lewis base: A compound or an ionic species which can donate a pair of electron known as lewis base.
ii) Ag2CrO4 ⇌ 2Ag+ + CrO42‒ 
     S               2s        s
Ksp = [Ag+ ]2 [CrO42‒] = (2s)2 (s)
     = 4s3 = 4 x (8 x 10‒5 )3 = 2.048 x 10‒12

Question
ICSEENICH12028885
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The [OH-] concentration of a weak base is given by:

  • Ckb

  • square root of straight C k subscript b
  • square root of straight K subscript bevelled straight b over straight c end subscript end root
  • square root of straight K subscript straight b end root

Solution

C.

square root of straight K subscript bevelled straight b over straight c end subscript end root

Question
ICSEENICH12028891
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If the ionization (dissociation) constant of acetic acid is ka, what will be the pH of a solution containing equal concentrations of acetic acid and sodium acetate?

Solution

For the equal concentration of acetic acid and sodium acetate in a solution. its pH will give by

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Question
ICSEENICH12028893
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Match the following:

A. Nernst equation (i) Water
B. Water (ii) Constant volume
C. Amphiprotic solvent (iii) Ammonia
D. Lewis base (iv) Optical Isomers
E. Isochoric process  (v) Electrochemical cells.

Solution

A.

Nernst equation

(i)

Electrochemical cells.

B.

Water

(ii)

Optical Isomers

C.

Amphiprotic solvent

(iii)

Water

D.

Lewis base

(iv)

Ammonia

E.

Isochoric process 

(v)

Constant volume

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