Question

When a solution of 0.10 M of AgNO3 is added to 50.0 ml of a CaCl2 solution of unknown concentration, 2.073 g of AgCl precipitates. Assuming 100% yield, what is was the concentration of the CaCl2 solution

Answer 1

Step-by-step explanation:

Equation for the reaction ;

AgNO3 + HCl → AgCl + HNO3

Since AgNO3 is taken in excess, the limiting reactant/agent here is HCl.

Concentration (molarity) of HCl = 0.110 M

Amount of HCl in 1 litre (1000 mL) solution = 0.110 mol

Amount of HCl in 50 mL = (0.110 x 50)/1000 = 0.0055 mol

As per the reaction equation, the consumption of HCl and the formation of AgCl are in the molar ratio 1 : 1.

Moles of AgCl formed = moles of HCl used = 0.0055

Molar mass of AgCl = 107.8 + 35.5 = 143.3 g/mol