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Dimpalk104
 one year ago
Suppose the isotopic ratio of the two boron isotopes 10B (10.013 amu) and 11B (11.009 amu) in a sample has been altered from the ratio found in nature and now contains 18.67% 10B in the sample. Determine the atomic weight of this sample of this new boron element.
Dimpalk104
 one year ago
Suppose the isotopic ratio of the two boron isotopes 10B (10.013 amu) and 11B (11.009 amu) in a sample has been altered from the ratio found in nature and now contains 18.67% 10B in the sample. Determine the atomic weight of this sample of this new boron element.

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zpupster
 one year ago
Best ResponseYou've already chosen the best response.1(0.1876 * 10.013) + ((1  0.1876) * 11.009)) taking the known percent and multiply by 10b subtract from 100 percent(or 1) to get remaining percent and multiply by 11B

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.0Simply when we have 2 types of isotopes the total abundance of both the elements should be equal to 100% If you have 18.67% of 10B then you will have (10018.67%) of 11B So you have 81.33% of 11B. \[a.m.u. = \frac{ (18.67 * 10.013) + (81.33 * 11.009) }{ 100 }= 10.823\]
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