Question

# When solutions of silver nitrate and calcium chloride are mixed, silver chloride precipitates out of solution...

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?

Part B

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

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

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

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