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anonymous
 4 years ago
Naturally occuring boron is 80.20% boron11 (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. :)
anonymous
 4 years ago
Naturally occuring boron is 80.20% boron11 (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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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0The 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.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Okay, thanks for the help, and equation. :)
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