×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide
Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide

People take antacids, such as milk of magnesia, to reduce

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 97P Chapter 14

Introductory Chemistry | 5th Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

4 5 0 285 Reviews
28
2
Problem 97P

People take antacids, such as milk of magnesia, to reduce the discomfort of acid stomach or heartburn. The recommended dose of milk of magnesia is 1 teaspoon, which contains 400 mg of Mg(OH)2. What volume of HCl solution with a pH of 1.1 can be neutralized by 1 dose of milk of magnesia? (Assume two significant figures in your calculations.)

Step-by-Step Solution:

Solution 97P:

Here, we are going to calculate the volume HCl required to neutralize 1 dose of milk of magnesia.

Step 1:

We know,

pH = -log [H+]

= 10-pH = 10-1.1

        =  0.0794 M = 0.0794 mol/L

Step 2:

Mass of 1 tablespoon Magnesia Mg(OH)2 = 400 mg = 0.4 g

Molar mass of Mg(OH)2 =58.319 g/mol

Amount of Magnesia =  = 0.00685 mol

Thus the concentration of [OH-] =  0.00685 mol x 2  = 0.0137mol

 

Step 3 of 3

Chapter 14, Problem 97P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

People take antacids, such as milk of magnesia, to reduce

×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide
Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide
×
Reset your password