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Complete the table. Assume that all concentrations are equilibrium concentrations in

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

Solution for problem 90P 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 90P

Problem 90P

Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.

Compound

[Cation]

[Anion]

Ksp

CdS

3.7 × 10−15

3.7 × 10−15

_____

BaF2

_____

7.2 × 10−3

1.9 × 10−7

Ag2SO4

2.8×10−2

_____

1.1 × 10−5

Step-by-Step Solution:
Step 1 of 3

Solution: Here, we are going to complete the given table.

Step1:

Solubility product of any substance is the product of the concentrations of the dissolved ions raised to the power of their stoichiometric coefficients.

Consider the ionization of a substance AB,

                                AB  A+ + B-

Then, the solubility product, Ksp = [A+][B-]

\Step2:

Compound

[Cation]

[Anion]

Ksp

CdS

3.7 x 10-15

3.7 x 10-15

1.369 x 10-29

BaF2

3.665 x 10-3

7.2 x 10-3

1.9 x 10-7

Ag2SO4

2.8 x 10-2

1.403 x 10-2

1.1 x 10-5

  1. The ionization of CdS takes place in the following manner:

                                CdS  Cd2+ + S2-

Solubility product for the reaction, Ksp = [Cd2+][S2-]

                                          = (3.7 x 10-15)(3.7 x 10-15)

                                          = 1.369 x 10-29

    b)        The ionization of BaF2 takes place in the following manner:

                                BaF2  Ba2+ + 2F-

Solubility product for the reaction, Ksp = [Ba2+][F-]2

                        Therefore, [Ba2+] = Ksp / [F-]2

                                          = (1.9 x 10-7) / (7.2 x 10-3)2

                                          = 0.03665 x 10-1

                                           = 3.665 x 10-3

                                

     c)        The ionization of Ag2SO4  takes place in the following manner:

                                Ag2SO4  2Ag+ + SO42-

Solubility product for the reaction, Ksp = [Ag+]2 [SO42-]

                        Therefore, [SO42-] = Ksp / [Ag+]2

                                          = (1.1 x 10-5) / (2.8 x 10-2)2

                                          = 0.1403 x 10-1

                                          = 1.403 x 10-2

                        

                                        -----------------------

Step 2 of 3

Chapter 15, Problem 90P is Solved
Step 3 of 3

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

The full step-by-step solution to problem: 90P from chapter: 15 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. The answer to “Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.Compound[Cation][Anion]KspCdS3.7 × 10?153.7 × 10?15_____BaF2_____7.2 × 10?31.9 × 10?7Ag2SO42.8×10?2_____1.1 × 10?5” is broken down into a number of easy to follow steps, and 25 words. Since the solution to 90P from 15 chapter was answered, more than 445 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This full solution covers the following key subjects: concentrations, compound, baf, cation, cds. This expansive textbook survival guide covers 19 chapters, and 2046 solutions.

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Complete the table. Assume that all concentrations are equilibrium concentrations in