Solution Stoichiometry

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)

Part A

What mass of silver chloride can be produced from 1.16  of a 0.233  solution of silver nitrate?

Part B

The reaction described in Part A required 3.35  of potassium chloride. What is the concentration of this potassium chloride solution?

Answer 1

AgNO3(aq) + KCl(aq) ==> AgCl(s) + KNO3(aq) ... balanced equation

Part A (I'm assuming the units are mls and the concentration is M)

What mass of silver chloride can be produced from 1.16 mls of a 0.233 M  solution of silver nitrate?

Part B

The reaction described in Part A required 3.35 mls  of potassium chloride. What is the concentration of this potassium chloride solution?

Part A:

1.16 mls x 1 L / 1000 mls x 0.233 mol / L = 0.000270 mols AgNO₃ present

0.000270 mls AgNO3 x 1 mol AgCl / mol AgNO3 = 0.000270 mols AgCl formed

mass of AgCl = 0.000270 mols AgCl x 143 g AgCl/mol = 0.0387 g AgCl

Part B:

mols KCl reacting = 0.000270 mols AgNO3 x 1 mol KCl / mol AgNO3 = 0.000270 mols KCl

Molarity of the KCl = 0.000270 mols / 0.00335 L = 0.0806 M KCl