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A solution contains 0.133 g of dissolved lead. How many

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

Solution for problem 111P Chapter 7

Introductory Chemistry | 5th Edition

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

Introductory Chemistry | 5th Edition

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Problem 111P

PROBLEM 111P

A solution contains 0.133 g of dissolved lead. How many moles of sodium chloride must be added to the solution to completely precipitate all of the dissolved lead? What mass of sodium chloride must be added?

Step-by-Step Solution:

Solution 111P

Here, we have to determine the moles of NaCl and mass of NaCl.

Step 1:  

Calculation of the mass of lead which is dissolved into the solution.

Molar mass of Lead =207.2 g/mol

Mass of lead dissolved in the solution = 0.133 g

Therefore, mole required for Lead is = = 0.000642 mol

Step 2:

Calculation for the mole of NaCl required to dissolve the precipitation.

Pb (s) + 2 NaCl(aq)-------> PbCl2(aq)

Therefore, 2 mole of NaCl required to dissolve the ppt = 2x 0.000642 mol =0.00128 mol

Thus, NaCl required to dissolve the lead precipitation = 0.00128 mol =1.28 x 10-3 mol

Step 3 of 3

Chapter 7, Problem 111P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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