   Chapter 4, Problem 106GQ

Chapter
Section
Textbook Problem

A noncarbonated soft drink contains an unknown amount of citric acid, H3C6H5O7. lf 100. mL of the soft drink requires 33.51 mL of 0.0102 M NaOH to neutralize the citric add completely, what mass of citric acid does the soft drink contain per 100. mL? The reaction of citric acid and NaOH isH3C6H5O7(aq) + 3 NaOH(aq) → Na3C6H5O7(aq) + 3 H2O(ℓ)

Interpretation Introduction

Interpretation:

The mass of citric acid in 100mL of soft drink 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.

Concentrationofsubstance=Amountof substancevolumeofthesubstance

• Amountof substance=Concentrationofsubstance×volumeofthesubstance
Explanation

Balanced chemical equation for the reaction of citric acid and NaOH is,

H3C6H5O7(aq)+3NaOH(aq)Na3C6H5O7(aq)+3H2O(l)

From the balanced chemical equation it is clear that reactants H3C6H5O7(aq)andNaOH are reacts in a 1:3 ratio

The amount (moles) of NaOH used in the reaction can be calculated from its volume and concentration as follows,

AmountofNaOH =CNaOH×VNaOH =0.0102molL×0.03351L =0

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