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An aqueous solution of hydrogen sulphide...

An aqueous solution of hydrogen sulphide shows the equilibrium: `H_(2) S hArr H^(o+)+HS^(ɵ)`
If dilute hydrochloric acid is added to an aqueous solution of `H_(2)S`, without any change in temperature, the
a. The equilibrium constant will change.
b. The concentration `HS^(ɵ)` will increase.
c. The concentration of un-dissociated hydogen sulphide will decrease.
d. The concentration of `HS^(ɵ)` will decrease.

Text Solution

AI Generated Solution

To solve the problem, we need to analyze the equilibrium reaction of hydrogen sulfide (H₂S) in an aqueous solution: **Equilibrium Reaction:** \[ H_2S \rightleftharpoons H^+ + HS^- \] When dilute hydrochloric acid (HCl) is added to this solution, it dissociates completely to provide additional \( H^+ \) ions: \[ HCl \rightarrow H^+ + Cl^- \] ...
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