If an aqueous solution of potassium iodide (Kl) was mixed with an aqueous solution of silver nitrate (AgNO3) would the reaction produce a precipitate?

Question

BlackTom AI · Accepted Answer

Consider the reaction between potassium iodide (KI) and silver nitrate (AgNO3) in aqueous solution.

Option: Yes and the precipitate would be AgI.

First, identify the possible ionic species in solution: KI dissociates into K+ and I− ions, while AgNO3 dissociates into Ag+ and NO3− ions. When these solutions are mixed, Ag+ ions meet I− ions.

Silver iodide (AgI) is known to be highly insoluble in water, having a very small solubility product (Ksp). As a result, when Ag+ and I− combine, they exceed the solubility limit and precipitate as solid AgI: Ag+ + I− → AgI(s).

The other product, potassium nitrate (KNO3), remains soluble in water and therefore stays as ions in solution: K+ and NO3− remain in aqueous form.

Why the other options would be incorrect: since only iodide is present to form an insoluble silver salt, there is indeed a precipitate; stating that no precipitate forms would ignoring the known low solubility of AgI. And specifying any other silver salt precipitate (like AgNO3 or AgI2−) is not supported by typical aqueous chemistry of these ions.

In summary, the reaction between KI and AgNO3 yields a precipitate of AgI due to the low solubility of silver iodide in water, with KNO3 remaining dissolved.

AGRI10046_2025_SM2 Week 4 progress quiz

If an aqueous solution of potassium iodide (Kl) was mixed with an aqueous solution of silver nitrate (AgNO3) would the reaction produce a precipitate?

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