Question

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

2AgNO3(aq)+MgCl2(aq)→2AgCl(s)+Mg(NO3)2(aq)

Part A: What mass of silver chloride can be produced from 1.31 L of a 0.156 M solution of silver nitrate?

Express your answer with the appropriate units.

Part B:

The reaction described in Part A required 3.43 L of magnesium chloride. What is the concentration of this magnesium chloride solution?

Express your answer with the appropriate units.

Answer 1

Part A

what mass of silver chloride can be produced from 1.31L of a .156 M solution of silver nitrate?

2AgNO3(aq) +MgCl2(aq) -> 2AgCl(s) + Mg(NO3)2(aq)

moles of siver nitrate=1.31 L*0.156 moles/L=0.2044 moles

moles of siver chloride=moles of AgNO3=0.2044 moles

mass of silver chloride=moles*mol wt=0.2044*143.32g/mole=29.3 g

Part B

The reaction described in Part A required 3.43L of magnesium chloride. What is the concentration of this magnesium chloride solution?

moles of MgCl2=0.5moles of AgNO3=0.50*0.2044moles=0.1022 moles

Concentration of MgCl2=moes/Volume=0.1022/3.43L=0.0298 M