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Silver has two naturally occurring isotopes (Ag-107 and

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

Solution for problem 104P Chapter 4

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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1
Problem 104P

Silver has two naturally occurring isotopes (Ag-107 and Ag-109).

(a) Use the periodic table to find the atomic mass of silver.

(b) If the natural abundance of Ag-107 is 51.84%, what is the natural abundance of Ag-109?

(c) If the mass of Ag-107 is 106.905 amu, what is the mass of Ag-109?

Step-by-Step Solution:
Step 3 of 5

Solution 104P

Here, we are going to calculate the natural abundance and mass of Ag-109.

Step1:

Atomic mass can be defined as the average mass of the isotopes of that element. If an element has no isotopes, then the mass of its atom would be the same as the sum of protons and neutrons in it. But if an element occurs in isotopic forms, then we have to know the percentage of each isotopic form and then the average mass is calculated.

The general formula for calculating the atomic mass of an element having n number of isotopes is given below:

                Atomic mass = (fraction of isotope n) x (mass of isotope n)        ----(1)

Step 2:

From the periodic table, the atomic mass of silver = 107.8682 amu.

Step 3:

b)        Given, natural abundance of Ag-107 = 51.84 %

Therefore, natural abundance of Ag-109 = 100 - 51.84 = 48.16 %

Step 4 of 5

Chapter 4, Problem 104P is Solved
Step 5 of 5

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

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Silver has two naturally occurring isotopes (Ag-107 and

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