#38. When solutions of silver nitrate and magnesium chloride are mixed, silver c

Question

#38. 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 1.68 L of a 0.243 M solution of silver nitrate

Express your answer with the appropriate units. Mass of AgCl=

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

Explanation / Answer

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

moles of AgCl= 0.243 x 1.68

= 0.408 moles

from the balenced reaction two moles of AgNO3 is giving 2 moles of AgCl

0.408 moles of AgNO3 will give 0.408 moles of AgCl

mass of AgCl = moles x molar mass

= 0.408 x 143.32

= 58.509 grams AgCl will get

Part B

from part A moles of AgCl = 0.408 moles

volume = 3.43 L

concentration M = 0.408 / 3.43

= 0.1189 M

= 0.12 M

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