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QUESTION

When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation? AgNO3(aq)+KCl(aq)→AgCl(s)+KNO3(aq)

Since you've got the first part, I'll just answer the second question, so to speak.

So, you've got your balanced chemical equation for this reaction

AgNO_(3(aq)) + KCl_((aq)) -> AgCl_((s)) + KNO_(3(aq))

You know that you have a "1:1" between all the species involved. This means that the number of moles of potassium chloride must be equal to the number of moles of silver nitrate.

Since I assume you've calculated the number of moles of silver nitrate to be

C = n/V => n = C * V

n_(AgNO_3) = "0.162 M" * "1.27 L" = "0.206 moles" AgNO_3

automatically you'll have

"0.206"cancel("moles "AgNO_3) * ("1 mole" KCl)/(cancel("1 mole "AgNO_3)) = "0.206 moles" KCl

Now use the volume of potassium chloride given to figure out what the solution's must be in order to have that many moles of KCl available for the reaction

C = n/V = "0.206 moles KCl"/"3.78 L" = color(red)("0.0545 M")