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 1.94 L of a 0.126 M solution of silver nitrate? Part B The reaction described in Part A required 3.49 L of calcium chloride. What is the concentration of this calcium chloride solution?

a)

moles of AgNO3 = M(AgNO3)*V(AgNO3)

= 0.126 M * 1.94 L

=0.244 mol

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

From balanced reaction above,

moles of AgCl formed = moles of AgNO3 reacted

= 0.244 mol

Molar mass of AgCl,

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

= 1*107.9 + 1*35.45

= 143.35 g/mol

mass of AgCl,

m = number of mol * molar mass

= 0.244 mol * 143.35 g/mol

= 35.0 g

b)

From balanced reaction,

moles of CaCl2 formed = (1/2)*moles of AgNO3

M(CaCl2)*V(CaCl2) = (1/2)*0.244 mol

M(CaCl2)*V(CaCl2) = 0.122

M * 3.49 L = 0.122

M = 0.0350 M

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