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A solution contains an unknown mass of dissolved silver

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

Solution for problem 80P Chapter 8

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 80P

PROBLEM 80P

A solution contains an unknown mass of dissolved silver ions. When potassium chloride is added to the solution, a white precipitate forms. The precipitate is filtered and dried and found to have a mass of 212 mg. What mass of silver was in the original solution? (Assume that all of the silver was precipitated out of solution by the reaction.)

Step-by-Step Solution:

Solution 80P

Step 1:

Amount of precipitate formed = 212 mg

The chemical equation for the reaction happening here is :

Ag2+ (aq) + KCl (aq)  → AgCl (s) + K+

Let’s find out the number of moles of AgCl formed :

                Number of moles (n) =

Molar mass of AgCl = 143.32 g/mol.

Barium precipitate formed is in mg, let’s convert to g :

                1 g = 1000 mg

Therefore, 0.212 mg in gram is :

                212 mg= 0.212 g

Now, let’s find the number of moles :

                         n =

                        n = 0.0014 moles

Therefore, the number of moles of Ag+ in the original solution is 0.0014 moles.  

Step 2 of 2

Chapter 8, Problem 80P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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