When solutions of silver nitrate and magnesium chloride are mixed, silver chlori

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 1.00 L of a 0.294 M solution of silver nitrate?

Express your answer with the appropriate units.

Part B

The reaction described in Part A required 3.22 L of magnesium chloride. What is the concentration of this magnesium chloride solution?

Express your answer with the appropriate units.

Explanation / Answer

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

part A

from equation

2 mole AgNo3 = 1 mole MgCl2

NO of mole of AgNO3 = M*V = 0.294*1 = 0.294 mole

NO of mole of AgCl produced = 0.294 mole

mass of AgCl produced = n*Mwt = 0.294*143.32 = 42.14 g

part B

NO of mole of MgCl2 required = 2*nAgCl = 2*0.294 = 0.588 mole

concentration of this magnesium chloride solution = n/V

              = 0.588/3.22 = 0.183 M

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