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

Calculate the pH of the following solutions.(a) 5.00 g of

Organic Chemistry | 8th Edition | ISBN: 9780321768414 | Authors: L.G. Wade Jr ISBN: 9780321768414 33

Solution for problem 13P Chapter 1

Organic Chemistry | 8th Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Organic Chemistry | 8th Edition | ISBN: 9780321768414 | Authors: L.G. Wade Jr

Organic Chemistry | 8th Edition

4 5 1 378 Reviews
13
4
Problem 13P

Calculate the pH of the following solutions.

(a) 5.00 g of HBr in 100 mL of aqueous solution

(b) 1.50 g of NaOH in 50 mL of aqueous solution

Step-by-Step Solution:
Step 1 of 3

Answer :

(a) 5.00 g of HBr in 100 mL of aqueous solution.

Given that

Mass of HBr= 5.00 g.

Volume =100 mL.

5 g HBr = ?

Before going to know the concentration we can calculate the number of moles of solute present in the given solution .

          =mass /molar mass .

          =5.0 g/80.91 g/mol.

          = 0.06179 mol.

Concentration of HBr = number of moles solute present in the 1L solution.

Concentration of HBr=0.06179 mol/0.1L

                                    =0.6179 mol / L(M).

Hence [H3O+]=0.6179 mol L -2

there are 0.062moles in 0.1L = 0.62M

in HBr, there are 0.62 M H+ and 0.62 M Br

pH = -log[H+] = -log [0.62] = .2

(b) 1.50 g of NaOH in...

Step 2 of 3

Chapter 1, Problem 13P is Solved
Step 3 of 3

Textbook: Organic Chemistry
Edition: 8
Author: L.G. Wade Jr
ISBN: 9780321768414

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

Calculate the pH of the following solutions.(a) 5.00 g of

×
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