   Chapter 4, Problem 69PS

Chapter
Section
Textbook Problem

What volume of 0.812 M HCI, in milliliters, is required to titrate 1.45 g of NaOH to the equivalence point?NaOH(aq) + HCl(aq) → H2O(l) + NaCI(aq)

Interpretation Introduction

Interpretation:

The volume of 0.812MHCl in milliliters, required to titrate 1.45g of NaOH to the equivalence point has to be determined.

Concept introduction:

Numberofmole=GivenmassofthesubstanceMolarmass

• 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.
• Concentrationofsubstance=Amountof substancevolumeofthesubstance
• Amountof substance=Concentrationofsubstance×volumeofthesubstance
• Volumeofthesubstance=Amountof substanceConcentrationofsubstance
Explanation

Balanced chemical equation for the given reaction is,

NaOH(aq)+HCl(aq)NaCl(aq)+H2O(l)

The amount (moles) of NaOH available can be calculated as follows,

1.45gNaOH×1molNaOH40g=0.03625molNaOH

The balanced equation for the reaction shows that 1mol of NaOH  requires 1mol of HCl

This is the required stoichiometric factor to obtain the amount of HCl present.

Thus the amount of HCl can be calculated as follows,

0.03625molNaOH×1molHCl1molNaOH=0

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