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 58.73% ¹⁰B in the sample. Determine the atomic weight of this sample of boron. A) 10.511 amu B) 10.013 amu C) 11.009 amu D) 10.424 amu E) 10.498 amu

Question

Quizplus · Accepted Answer

To determine the atomic weight, we first need to calculate the weighted average of the two isotopes based on their abundance:

(0.5873 x 10.013 amu) + (0.4127 x 11.009 amu) = 10.424 amu

Therefore, the atomic weight of the sample is 10.424 amu, which corresponds to choice D.

Suppose the Isotopic Ratio of the Two Boron Isotopes 10B

Suppose the Isotopic Ratio of the Two Boron Isotopes ¹⁰B