Question

An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List 1. The variation in conductivity of these reactions is given in List 2. Match List 1 with List 2 and select the correct answer using the code given below the lists:

Answer 1

$\left(A\right)$ $(C_2\underset{X}{H_5}{)}_{3}N+C{H}_3\underset{Y}{CO}OH\to (C_2{H}_5{)}_{3}N{H}^{+}C{H}_{3}CO{O}^{-}$
Initially, conductivity increases due to ion formation after that it becomes practically constant because X alone can not form ions. Hence, (3) is the correct match.
$\left(B\right)$ $KI\left(\underset{X}{0.1}M\right)+AgN{O}_3\underset{Y}{(}0.01M)\to AgI\downarrow +KN{O}_3$
Number of ions in the solution remains constant until all the $AgN{O}_3$ precipitated as $AgI$. Thereafter, conductance increases due to increases in number of ions. Hence, (4) is the correct match.
$\left(C\right)$ Initially, conductance decreases due to the decrease in the number of $O{H}^{-}$ ions thereafter, it slowly increases due to the increases in number of $H^{+}$ ions. Hence, (2) is the correct match.
$\left(D\right)$ Initially it decreases due to decrease in $H^{+}$ ions and then increases due to the increases in $O{H}^{-}$ions. Hence, (1) is the correct match.