   Chapter 4, Problem 62PS

Chapter
Section
Textbook Problem

What mass of Na2CO3, in grams, is required for complete reaction with 50.0 mL of 0.125 M HNO3?Na2CO3(aq) + 2 HNO3(aq)→ 2 NaNO3(aq) + CO2(g) + H2O(l)

Interpretation Introduction

Interpretation:

It should be determine that the mass of Na2CO3, in grams, which is required to react completely with 50.0mlof0.125MHNO3

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.
Explanation

Balanced chemical equation for the given reaction is,

Na2CO3(aq)+2HNO3(aq)2NaNO3(aq)+CO2(g)+H2O(l)

The amount (moles) of HNO3  available can be calculated by as follows,

Before that 50.0mLHNO3 is converted into L.

Thus amount of HNO3 available,

0.05LHNO3×(0.125molHNO31LHNO3)=0.006250molHNO3

By using the stoichiometric factor calculating the amount of Na2CO3  required based on the amount of HNO3 as follows

0

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