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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

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

Organic Chemistry | 8th Edition

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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 2

(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  = 0.6179 mol

there are 0.062 moles in 0.1 L = 0.62M

in HBr, there are 0.62 M  and 0.62 M Br

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

Step 2 of 2

Chapter 1, Problem 13P is Solved
Textbook: Organic Chemistry
Edition: 8
Author: L.G. Wade Jr
ISBN: 9780321768414

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