Naturally occuring boron is 80.20% boron-11 (atomic mass 11.01 amu) and 19.80% of some other isotope. What must the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass of boron? ***NOTE: I will be more than happy if somebody just clarifies the question, I'm not specifically looking for the answer. :)

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Naturally occuring boron is 80.20% boron-11 (atomic mass 11.01 amu) and 19.80% of some other isotope. What must the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass of boron? ***NOTE: I will be more than happy if somebody just clarifies the question, I'm not specifically looking for the answer. :)

Chemistry
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The average atomic mass of an element is found by taking the weighted average of all naturally occurring isotopes. The algorithm will be something like this:\[Avg=(Percent_{} Occurrence)*(Atomic_{}Weight)+(PercentOccurrence)*(AtomicWeight)+...\]Do this for each isotope of the element.
Okay, thanks for the help, and equation. :)

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