   Chapter 4, Problem 25PS

Chapter
Section
Textbook Problem

A mixture of CuSO4 and CuSO4.5 H2O has a mass of 1.245 g. After heating to drive off all the water, the mass is only 0.832 g. What is the mass percent of CuSO4.5H2O in the mixture? (See page 98.)

Interpretation Introduction

Interpretation:

The mass percent of CuSO4.5H2O in the given sample has to be determined.

Concept introduction:

• The relation between the number of moles and mass of the substance is ,

Numberofmole=MassingramMolarmass

Massingramofthesubstance=Numberofmole×Molarmass

• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
• Amountof substance=Concentrationofsubstance×volumeofthesubstance
• Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.
Explanation

Here mixture of CuSO4 and CuSO4.5H2O heating to drive off all the water then the mass of the mixture is reduced from  1.245g to 0.832g

From the amount of water involved in the reaction, amount of CuSO4 can be calculated.

Both of these components in this reaction react in 1:1 stoichiometric ratio.

Mass of water =1.245g0.832g=0.413g

Amount of water = 0.413g18g/mol=0.0229molH2O

Amount of  CuSO4 = 0.0229molH2O×1molofCuSO45molH2O=0.00458molCuSO4

Mass of CuSO40

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