Question

A 25 mL solution of 0.1 M AgNO3 is mixed with a 50 mL solution of 0.05 M NaCl. What is the mass of AgCl that will be produced if a reaction occurs? (Assume the reaction goes to completion.)

Answer 1

First, we need to determine the limiting reactant. To do this, we will calculate the moles of each reactant.Moles of AgNO3 =  Volume  Molarity Moles of AgNO3 =  0.025 L  0.1 M  = 0.0025 molesMoles of NaCl =  Volume  Molarity Moles of NaCl =  0.050 L  0.05 M  = 0.0025 molesThe balanced chemical equation for the reaction is:AgNO3 + NaCl  AgCl + NaNO3From the balanced equation, we can see that the mole ratio of AgNO3 to NaCl is 1:1. Since both reactants have the same number of moles  0.0025 moles , neither reactant is in excess, and both are limiting reactants.Now, we can calculate the moles of AgCl that will be produced:Moles of AgCl = Moles of limiting reactant = 0.0025 molesNext, we need to convert moles of AgCl to mass. To do this, we will use the molar mass of AgCl  143.32 g/mol :Mass of AgCl =  Moles of AgCl  Molar mass of AgCl Mass of AgCl =  0.0025 moles  143.32 g/mol  = 0.3583 gTherefore, the mass of AgCl that will be produced in the reaction is approximately 0.3583 grams.