Question

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

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?

Part B:

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

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

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