ElectrochemistryHard
Question
An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List-I. The variation in conductivity of these reactions is given in List-II. Match List-I with List-II and select the correct answer using the code given below the lists :
Options
A.P → 3, Q → 4, R → 2, S → 1
B.P → 4, Q → 3, R → 2, S → 1
C.P → 2, Q → 3, R → 4, S → 1
D.P → 1, Q → 4, R → 3, S → 2
Solution
(A) For weak base v/s weak acid titration upto equivalence point conductivity increases because weakelectrolyte (W.A.) is converted to strong electrolyte (salt) but after it weak base does not dissociateappreciably
(B) For KI + AgNO3 → AgI(ppt.) + KNO3
upto equivalence point number of ions remain same but after it increases
(C) For weak acid v/s strong base titration upto equivalence point OH- ion is replaced by CH3COO-so conductivity decreases but after it weak acid does not dissociate appreciably.
(D) For strong base v/s strong acid titration upto equivalence point H+ ion is replaced by Na+ so conductivitydecreases but after it increases due to increase in number of ions.
(B) For KI + AgNO3 → AgI(ppt.) + KNO3
upto equivalence point number of ions remain same but after it increases
(C) For weak acid v/s strong base titration upto equivalence point OH- ion is replaced by CH3COO-so conductivity decreases but after it weak acid does not dissociate appreciably.
(D) For strong base v/s strong acid titration upto equivalence point H+ ion is replaced by Na+ so conductivitydecreases but after it increases due to increase in number of ions.
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