Question

When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution according to the equation

2AgNO3(aq)+CaCl2(aq)→2AgCl(s)+Ca(NO3)2(aq)

1. What mass of silver chloride can be produced from 1.97 L of a 0.285 M solution of silver nitrate?

2.The reaction described in Part A required 3.62 L of calcium chloride. What is the concentration of this calcium chloride solution?

Answer 1

Q1.

calculate mol of Silver nitrate, AgNO3

mol = MV = 1.97*0.285 = 0.56145 mol of AgNO3

then..

ratio is 2:2 or 1:1 with reswpect to AgNO3 and AgCl

so

mol of AgCl = 0.56145mol

MW of AgCl = 143.32 g/mol

mass = mol*MW = 0.56145*143.32 = 80.467014 g

Q2.

V = 3.62 L of CaCl2 solution...

relate to mol of CaCl2

2:1 ratio of AgNO3:CaCl2

so

0.56145 mol of AgNO3 --> 1/2*0.56145 = 0.280725 mol of CaCl2

then

molarity was:

M = mol/V = 0.280725 /(3.62) = 0.0775483 M of CaCl2