0.1 M KI (aq) was added to a solution that contains Na2CO3 + AgNO3 + HNO3...

0.1 M KI (aq) was added to a solution that contains Na2CO3 + AgNO3 + HNO3 + HCl + NH3 which was initially colourless.

After 13 drops, a milky solution was produced. What is the precipitate formed and explain the shift of equilibrium of the reaction using Le Chatelier’s principle.

Solutions

Expert Solution

When KI is added to the solution, it completely dissociates into K⁺ and I^-

silver ions react with iodide ions to form silver iodide precipitate which makes the solution milky

AgNO₃ (aq) + KI (aq) AgI (s) + KNO₃ (aq)

The initial equlibrium is assumed as

AgNO₃ (s) Ag⁺ (aq) + NO₃^- (aq)

When silver ions form the silver iodide precipitate, then the above equilibrium is disturbed and according to Le Chatelier's principle, the equilibrium will move in forward direction, producing more Ag⁺ ions to compensate for those lost in forming the precipitate

If there is any other equilibrium process like above, then please specify in comments

queen_honey_blossom answered 1 year ago

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