Question

Solution Stoichiometry:

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 1.46 L of a 0.218 M solution of silver nitrate?

Part B. The reaction described in Part A required 3.17 L of potassium chloride. What is the concentration of this potassium chloride solution?

Answer 1

moles of AgNO3 ( Silven nitrate) in 1.46L of 0.218M= 1.46*0.218=0.318 moles ( Molairty= moles/ volume of solution in L and moles = molarity* volume of solution in L)

From the reaction, AgNO3+ KCl---> AgCl+ KNO3

one mole of AgNO3 gives 1 mole of AgCl

0.318 moles of AgNO3 gives 0.318 moles of AgCl

Mass of AgCl= moles* Molecular weight of AgCl =0.318*143= 45.474 gms

B) 1 mole of AgNO3 requires 1 mole of KCl

0.318 moles require 0.318 moles of KCl

but its volume is 3.17L Molarity= moles/Liter of solution = 0.318/31.7 M=0.100M