   Chapter 4, Problem 113GQ

Chapter
Section
Textbook Problem

You place 2.56 g of CaCO3 in a beaker containing 250. mL of 0.125 M HCl. When the reaction has ceased, does any calcium carbonate remain? What mass of CaCl2 can be produced?CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(ℓ)

Interpretation Introduction

Interpretation:

The mass of CaCl2 produced in the given reaction has to be determined.

Concept introduction:

• 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.
• 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).
• 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
• Massofthesubstance=Amountofthesubstance×molarmassofthesubstance
Explanation

Balanced chemical equation for the given reaction is,

CaCO3(s)+2HCl(aq)CaCl2(aq)+CO2(g)+H2O(l)

Amount of HCl can be calculated from its volume and concentration as follows,

AmountofHCl =CHCl×VHCl =0.125molL×0.25L =0.03125molHCl

Using the stoichiometric factor the amount of CaCO3 required to proceed this reaction can be calculated as follows,

0.03125molHCl×1molCaCO32molHCl=0

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