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Question

A mixture of CaCl2 and KCl weighing 0.75 g was reacted with aqueous AgNO3. The reaction converted all Cl- ions to 1.75 g of AgCl. What percent by mass of the original mixture was KCl?

Answer 1

CaCl2(aq) + 2 AgNO3(aq) ==> 2AgCl(s) + Ca(NO3)2(aq)

KCl(aq) + AgNO3(aq) ==> AgCl(s) + KNO3(aq)

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CaCl2(aq) + KCl(aq) + 3 AgNO3(aq) ==> 3 AgCl(s) + Ca(NO3)2(aq) + KNO3(aq)

moles of AgCl formed = 1.75 g AgCl x 1mole/143.3 g = 0.0122 moles AgCl

grams CaCl2 in original sample = 0.0122 moles AgCl x 1 mol CaCl2/3 mole AgCl x 111 g/mol = 0.45 g

grams KCl in original sample = 0.0122 mol AgCl x 1 mol KCl/3 mol AgCl x 74.55 g/mol 0.30 g

% KCl by mass = 0.30 g/0.75 g (x100) = 40%