Boron naturally occurs in two isotopic forms. the more common isotope is 11b (atomic mass 11.01 amu), which is 80.00% abundant. the average atomic mass of boron is 10.81. what is the mass of the other isotope?

Answer is: mass of the other isotope of boron is 10.01 amu.

Ar₁(B) = 11.01 amu; the average atomic mass of isotope ¹¹B.  

Ar₂(B) =?; the average atomic mass of unknown isotope of boron.  

ω₁(B) = 80.00%; mass percentage of isotope ¹¹B.

ω₂(B) = 100.0% - 80.00%.  

ω₂(B) = 20.00%.; mass percentage of unknown isotope of boron.

ω₂(B) = 20.00% ÷ 100% = 0.20.

Ar(B) = 10.81 amu; average atomic mass of boron.

Ar(B) = Ar₁(B) · ω₁(B) + Ar₂(B) · ω₂(B).  

10.81 amu = 11.01 amu · 0.8 + Ar₂(B) · 0.2.

Ar₂(B) = 2.002 amu ÷ 0.2.

Ar₂(B) = 10.01 amu.

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