(B) According to Le Chatelier's principle,when a product $(CN_{(aq)}^{-})$ is added to a system at equilibrium,the reaction shifts in the backward dir

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Decrease the $H_{(aq)}^{+}$ ion concentration

(B) According to Le Chatelier's principle,when a product $(CN_{(aq)}^{-})$ is added to a system at equilibrium,the reaction shifts in the backward direction to counteract the change.This shift consumes $H_{(aq)}^{+}$ ions and $CN_{(aq)}^{-}$ ions to form more $HCN_{(aq)}$.Therefore,the concentration of $H_{(aq)}^{+}$ ions decreases.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Le-Chaterlier principle and It’s application

Easy

Consider the reaction $HCN_{(aq)} \Leftrightarrow H_{(aq)}^{+} + CN_{(aq)}^{-}$. At equilibrium,the addition of $CN_{(aq)}^{-}$ would

A
Reduce $HCN_{(aq)}$ concentration
B
Decrease the $H_{(aq)}^{+}$ ion concentration
C
Increase the equilibrium constant
D
Decrease the equilibrium constant

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

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Consider the reaction $HCN_{(aq)} \Leftrightarrow H_{(aq)}^{+} + CN_{(aq)}^{-}$. At equilibrium,the addition of $CN_{(aq)}^{-}$ would

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In a lime kiln,to get a higher yield of $CO_2$,the measure that can be taken is:

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Some inert gas is added at constant volume to the following reaction at equilibrium:
$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
Predict the effect of adding the inert gas.