(B) According to Le Chatelier's principle,adding $HCl$ increases the concentration of $H^{+}$ ions in the solution.This shift in concentration causes

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Concentration of $CH_3COO^{-}$ will decrease

(B) According to Le Chatelier's principle,adding $HCl$ increases the concentration of $H^{+}$ ions in the solution.This shift in concentration causes the equilibrium to move in the reverse direction to counteract the change.As the reaction proceeds in the reverse direction,the concentration of $CH_3COO^{-}$ ions will decrease.The equilibrium constant $(K_a)$ remains unchanged because the temperature is constant.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Common ion effect

Easy

The following equilibrium exists in aqueous solution: $CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$. If dilute $HCl$ is added without a change in temperature,then the:

A
Concentration of $CH_3COO^{-}$ will increase
B
Concentration of $CH_3COO^{-}$ will decrease
C
Equilibrium constant will increase
D
Equilibrium constant will decrease

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6-2.Equilibrium-II (Ionic Equilibrium)

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Common ion effect

Addition of conc. $HCl$ to saturated $BaCl_2$ solution precipitates $BaCl_2$; because

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Calculate $[S^{2-}]$ and $[HS^{-}]$ of the solution which contains $0.1 \ M \ H_2S$ and $0.3 \ M \ HCl$.
[$K_{a1} = 1.0 \times 10^{-7}$ and $K_{a2} = 1.3 \times 10^{-13}$ for $H_2S$]

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In the absence of the formation of complex ions by the addition of a common ion,the solubility of a given salt is

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Assertion $(A) :-$ When a small amount of strong acid or strong base is added to pure water,its $pH$ undergoes a change.
Reason $(R) :-$ Addition of an acid or base increases the degree of ionisation of water.

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Consider the nitration of benzene using mixed conc. $H_2SO_4$ and $HNO_3$. If a large amount of $KHSO_4$ is added to the mixture,the rate of nitration will be

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The following equilibrium exists in aqueous solution: $CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$. If dilute $HCl$ is added without a change in temperature,then the:

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Addition of conc. $HCl$ to saturated $BaCl_2$ solution precipitates $BaCl_2$; because

Calculate $[S^{2-}]$ and $[HS^{-}]$ of the solution which contains $0.1 \ M \ H_2S$ and $0.3 \ M \ HCl$.[$K_{a1} = 1.0 \times 10^{-7}$ and $K_{a2} = 1.3 \times 10^{-13}$ for $H_2S$]

In the absence of the formation of complex ions by the addition of a common ion,the solubility of a given salt is

Assertion $(A) :-$ When a small amount of strong acid or strong base is added to pure water,its $pH$ undergoes a change.Reason $(R) :-$ Addition of an acid or base increases the degree of ionisation of water.

Consider the nitration of benzene using mixed conc. $H_2SO_4$ and $HNO_3$. If a large amount of $KHSO_4$ is added to the mixture,the rate of nitration will be

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Calculate $[S^{2-}]$ and $[HS^{-}]$ of the solution which contains $0.1 \ M \ H_2S$ and $0.3 \ M \ HCl$.
[$K_{a1} = 1.0 \times 10^{-7}$ and $K_{a2} = 1.3 \times 10^{-13}$ for $H_2S$]

Assertion $(A) :-$ When a small amount of strong acid or strong base is added to pure water,its $pH$ undergoes a change.
Reason $(R) :-$ Addition of an acid or base increases the degree of ionisation of water.