A 0.7209-g solid mixture containing MgCl2 is dissolved in water and treated with an excess of AgNO3, resulting in the precipitation of 1.032 g of AgCl. What is the percent of mass of MgCl2in the mixture?
A 0.7209-g solid mixture containing MgCl2 is dissolved in water and treated with an excess of AgNO3, resulting in the precipitation of 1.032 g of AgCl. What is the percent of mass of MgCl2in the mixture?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
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A 0.7209-g solid mixture containing MgCl2 is dissolved in water and treated with an excess of AgNO3, resulting in the precipitation of 1.032 g of AgCl. What is the percent of mass of MgCl2in the mixture?
Expert Solution
Step 1
Given : Mass of MgCl2 sample = 0.7209 g
And mass of AgCl = 1.032 g
Molar mass of AgCl = Atomic mass of Ag + Atomic mass of Cl = 108 + 35.5 = 143.5 g/mol.
Since mass = moles X molar mass
=> 1.032 = moles of AgCl produced X 143.5
=> Moles of AgCl produced = 0.0072 mol approx.
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