   Chapter 4, Problem 68PS

Chapter
Section
Textbook Problem

What volume of 0.125 M oxalic acid, H2C2O4, is required to react with 35.2 mL of 0.546 M NaOH?H2C2O4(aq) + 2 NaOH(aq) → Na2C2O4(aq) + 2H2O(l)

Interpretation Introduction

Interpretation:

The volume of 0.125M oxalic acid H2C2O4 required to react with 35.2mLof 0.546MNaOH 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).

Molarity=Amountofsolute(mol)Volumeofsolution(L)

• 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.
Explanation

Balanced chemical equation for the given reaction is,

H2C2O4(aq)+2NaOH(aq)Na2C2O4(aq)+2H2O(l)

Amount of NaOH in 35.2 mL of 0.546 M NaOH = 0.0352L×0.546M = 0.0192moles

By using the stoichiometric factor calculating the amount of H2C2O4 required based on the amount of NaOH as follows,

0.0192molNaOH×1molH2C2O42molNaOH=0

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