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 1.65 L of a 0.282 M solution of silver nitrate?

Express your answer with the appropriate units.

Part B

The reaction described in Part A required 3.91 L of magnesium chloride. What is the concentration of this magnesium chloride solution?

Express your answer with the appropriate units.

Answer 1

2 moles of AgCl is produced from 2 moles of AgNO3.

Moles of AgNO3 used =1.65 L * 0.282 M = 0.4653 moles

So, moles of AgCl produced = 0.4653 moles*143.32 gm/mole = 66.69 gm

Mass of silver chloride produced = 66.69 gm

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1 mole of MgCl2 reacts with 2 moles of AgNO3.

So moles of MgCl2 usd in this reaction =0.4653/2 = 0.2327 moles

Concentration of MgCl2 =0.2327moles/3.91 L =0.059 moles/L = 0.059 M