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A saturated solution of PbCl2 has [Cl?] = 2.86 × 10?2 M.

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

Solution for problem 84P Chapter 15

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 84P

A saturated solution of PbCl2 has [Cl−] = 2.86 × 10−2 M. What is the concentration of Pb2+?

Step-by-Step Solution:
Step 1 of 3

Step-1

The concentration of [Cl-] in a saturated solution of PbCl2 = 2.86 × 10−2 M.

We have to calculate the concentration of Pb2+

Step-2

Explanation:

PbCl2 dissociate to give,

PbCl2 = Pb2+ + 2 Cl- 

the ratio between Pb2+ and Cl- is 1 : 2

So...

Step 2 of 3

Chapter 15, Problem 84P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This full solution covers the following key subjects: concentration, pbcl, saturated, solution. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The answer to “A saturated solution of PbCl2 has [Cl?] = 2.86 × 10?2 M. What is the concentration of Pb2+?” is broken down into a number of easy to follow steps, and 18 words. The full step-by-step solution to problem: 84P from chapter: 15 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 84P from 15 chapter was answered, more than 739 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5.

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A saturated solution of PbCl2 has [Cl?] = 2.86 × 10?2 M.

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