×
Log in to StudySoup
Get Full Access to Principles Of General Chemistry - 2 Edition - Chapter 2 - Problem 96p
Join StudySoup for FREE
Get Full Access to Principles Of General Chemistry - 2 Edition - Chapter 2 - Problem 96p

Already have an account? Login here
×
Reset your password

The two isotopes of potassium with significant abundance

Principles of General Chemistry | 2nd Edition | ISBN: 9780073511085 | Authors: Martin S. Silberberg ISBN: 9780073511085 71

Solution for problem 96P Chapter 2

Principles of General Chemistry | 2nd Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Principles of General Chemistry | 2nd Edition | ISBN: 9780073511085 | Authors: Martin S. Silberberg

Principles of General Chemistry | 2nd Edition

4 5 1 347 Reviews
12
1
Problem 96P Problem 96P

The two isotopes of potassium with significant abundance in nature are 39K (isotopic mass 38.9637 amu, 93.258%) and 41K (isotopic mass 40.9618 amu, 6.730%). Fluorine has only one naturally occurring isotope, 19F (isotopic mass 18.9984 amu). Calculate the formula mass of potassium fluoride.

Step-by-Step Solution:

Solution 96P

Here, we have to calculate the formula mass of potassium fluoride.

Step 1 of 3

The given two isotopes are and  

Let’s calculate the proton atomic mass from two isotopes.

For  

Given

Isotopic mass = 38.9637 amu

Abundance = 93.258%

Calculate the fraction value =  = 0.93258.

Proton of atomic mass from   = Isotopic mass x Abundance

                                                      =  38.9637 x  0.93258

                                                      =  36.337 amu

Therefore, Proton of atomic mass from  is 36.337 amu.

For  

Given

Isotopic mass = 40.9618 amu

Abundance = 6.730%

Calculate the fraction value =  = 0.06730

Poton of atomic from  =  Isotopic mass x Abundance

                                           = 40.9618 x 0.06730

                                           = 2.757 amu.

Therefore, proton of atomic mass from   is 2.757 amu.

______________________________________________________________________________

Step 2 of 3

Chapter 2, Problem 96P is Solved
Step 3 of 3

Textbook: Principles of General Chemistry
Edition: 2
Author: Martin S. Silberberg
ISBN: 9780073511085

This full solution covers the following key subjects: mass, AMU, isotopic, potassium, Isotopes. This expansive textbook survival guide covers 23 chapters, and 1878 solutions. Since the solution to 96P from 2 chapter was answered, more than 505 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 96P from chapter: 2 was answered by , our top Chemistry solution expert on 08/31/17, 03:54AM. This textbook survival guide was created for the textbook: Principles of General Chemistry, edition: 2. The answer to “The two isotopes of potassium with significant abundance in nature are 39K (isotopic mass 38.9637 amu, 93.258%) and 41K (isotopic mass 40.9618 amu, 6.730%). Fluorine has only one naturally occurring isotope, 19F (isotopic mass 18.9984 amu). Calculate the formula mass of potassium fluoride.” is broken down into a number of easy to follow steps, and 43 words. Principles of General Chemistry was written by and is associated to the ISBN: 9780073511085.

Other solutions

People also purchased

Related chapters

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

The two isotopes of potassium with significant abundance