Problem: Naturally occurring silver consists of two isotopes: 107Ag (51.84%) with an isotopic mass of 106.9051 amu and 109Ag (48.16%) with an isotopic mass of 108.9048 amu.What is the atomic weight of silver?

FREE Expert Solution

We can use the following equation:


Atomic Mass=[mass×f.a.]isotope 1+[mass×f.a.]isotope 2


To get f.a., we simply need to divide the given percent abundance by 100.


82% (291 ratings)
View Complete Written Solution
Problem Details

Naturally occurring silver consists of two isotopes: 107Ag (51.84%) with an isotopic mass of 106.9051 amu and 109Ag (48.16%) with an isotopic mass of 108.9048 amu.

What is the atomic weight of silver?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Atomic Mass concept. You can view video lessons to learn Atomic Mass. Or if you need more Atomic Mass practice, you can also practice Atomic Mass practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Asbury's class at PSU.