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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 13, Problem 43E
Textbook Problem
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Suppose that the stomach contains 0 .200 L of 0 .05-M HCl . What mass of the antacid Mg ( OH ) 2 is required to completely neutralize all of the HCl ?

Interpretation Introduction

Interpretation:

The mass of antacid Mg(OH)2 required to neutralize all the given volume of HCl is to be calculated.

Concept Introduction:

Antacids are the substances that neutralize the acidity of the stomach. They work differently from other acids, by reducing the secretion of stomach acids.

Antacids can be in the form of liquid, tablets, or chewable tablets.

These are used to treat indigestion, heartburn, the burning sensation in the chest, and acid reflux in stomach.

Molar mass is the mass of a substance, in grams, present in one mole of the substance.

Molarity and number of moles are related to each other by the formula:

Number of moles= molarity× volume of solution in litres

Explanation of Solution

Given information: 0.200 L of 0.05 M HCl.

The neutralization reaction of antacid Mg(OH)2 is:

Mg(OH)2+ 2HCl MgCl2+ 2H2O

Number of moles= molarity× volume of solution in litres

Number of moles of H+=0.05 M×0.200 L=1×102 mol 

In the neutralization reaction, number of moles of H+ and OH are equal, therefore,

Number of moles of OH=1×102 mol 

Number 

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Chapter 13 Solutions

Chemistry In Focus
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