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)

Part A

What mass of silver chloride can be produced from 1.09 L of a 0.281 M solution of silver nitrate?

Express your answer with the appropriate units.

Part B

The reaction described in Part A required 3.16 L of calcium chloride. What is the concentration of this calcium chloride solution?

Express your answer with the appropriate units.

Answer 1

A)

mol of AgNO3 reacted = M(AgNO3)*V(AgNO3)

= 0.281 M * 1.09 L

= 0.3063 mol

from reaction,

mol of AgCl formed = mol of AgNO3 reacted

= 0.3063 mol

Molar mass of AgCl,

MM = 1*MM(Ag) + 1*MM(Cl)

= 1*107.9 + 1*35.45

= 143.35 g/mol

use:

mass of AgCl,

m = number of mol * molar mass

= 0.3063 mol * 1.434*10^2 g/mol

= 43.91 g

Answer: 43.9 g

B)

from reaction,

mol of CaCl2 reacted = (1/2)*mol of AgNO3 reacted

= (1/2)*0.3063 mol

= 0.1532 mol

Now use:

mol of CaCl2 = M(CaCl2)*V(CaCl2)

0.1532 = M * 3.16 L

M = 0.0485 M

Answer: 0.0485 M