Predict whether or not a precipitate forms upon mixing 175.0 mLmL of a 0.0055 MKClMKCl solution with 145.0 mLmL of a 0.0015 MM AgNO3AgNO3 solution. Identify the precipitate, if any. Express your answer as a chemical formula. Enter noreaction if no precipitate is formed. nothing

AgCl

Explanation:

The reaction of KCl (In aqueous phase K⁺ + Cl⁻) with AgNO₃ ((In aqueous phase Ag⁺ + NO₃⁻) produce:

Ag⁺ + Cl⁻ ⇄ AgCl(s)

The reaction has a k of 5.56x10¹⁰

That means you will produce 5.56x10¹⁰ molecules of AgCl per molecule of Ag⁺ and Cl⁻ in solution.

As the AgCl is in solid state, this molecules is the precipitate.

I hope it helps!