   Chapter 4, Problem 61PS

Chapter
Section
Textbook Problem

What volume of 0.109 M HNO3, in milliliters, is required to react completely with 2.50 g of Ba(OH)2?2 HNO3(aq) + Ba(OH)2(s) → 2 H2O(l) + Ba(NO3)2(aq)

Interpretation Introduction

Interpretation:

It should be determine that the volume of 0.109MHNO3, in milliliters, which is required to react completely with 2.50gofBa(OH)2

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

Volume of 0.109MHNO3, in milliliters, is required to react completely with 2.50gofBa(OH)2

Balanced chemical equation for the given reaction is

2HNO3(aq)+Ba(OH)2(s)2H2O(l)+Ba(NO3)2(aq)

The amount (moles) of Ba(OH)2  available can be calculated by using the equation

Numberofmole=GivenmassofthesubstanceMolarmass

2.50gBa(OH)2×1molBa(OH)2171.34gBa(OH)2=0.0146molBa(OH)2

By using the stoichiometric factor calculating the amount of HNO3 required based on the amount of Ba(OH)2 as follows,

0

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