# Problem: Silver is composed of two naturally occurring isotopes: Ag-107 (51.839%) and Ag-109. The ratio of the masses of the two isotopes is 1.0187.What is the mass of Ag-107?

###### FREE Expert Solution
92% (268 ratings)
###### FREE Expert Solution

We’re being asked to calculate the mass of silver-107 (Ag-107). We can use the following equation:

where atomic mass = average atomic mass of the element and f.a. = fractional abundance of the isotope. To get f.a., we simply need to divide the given percent abundance by 100.

92% (268 ratings)
###### Problem Details

Silver is composed of two naturally occurring isotopes: Ag-107 (51.839%) and Ag-109. The ratio of the masses of the two isotopes is 1.0187.

What is the mass of Ag-107?

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 .

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Our expert Chemistry tutor, Jules took 3 minutes to solve this problem. You can follow their steps in the video explanation above.

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

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