We are asked to determine the atomic weight (average molecular mass) of a Boron (B) given 10B (19.9%) with an isotopic mass of 10.0129 amu and 11B (80.1%) with an isotopic mass of 11.00931 amu.
We will solve for Boron's average mass using their abundance.
The formula for average mass is:
Naturally occurring boron consists of two isotopes: 10B (19.9%) with an isotopic mass of 10.0129 amu and 11B (80.1%) with an isotopic mass of 11.00931 amu.
What is the atomic weight of boron? Check your answer by looking at a periodic table.
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