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The two isotopes of potassium with significant abundance
Chapter 1, Problem 96P(choose chapter or problem)
The two isotopes of potassium with significant abundance in nature are 39K (isotopic mass 38.9637 amu, 93.258%) and 41K (isotopic mass 40.9618 amu, 6.730%). Fluorine has only one naturally occurring isotope, 19F (isotopic mass 18.9984 amu). Calculate the formula mass of potassium fluoride.
Questions & Answers
QUESTION: Problem 96P
The two isotopes of potassium with significant abundance in nature are 39K (isotopic mass 38.9637 amu, 93.258%) and 41K (isotopic mass 40.9618 amu, 6.730%). Fluorine has only one naturally occurring isotope, 19F (isotopic mass 18.9984 amu). Calculate the formula mass of potassium fluoride.
ANSWER:
Solution 96P
Here, we have to calculate the formula mass of potassium fluoride.
Step 1 of 3
The given two isotopes are and
Let’s calculate the proton atomic mass from two isotopes.
For
Given
Isotopic mass = 38.9637 amu
Abundance = 93.258%
Calculate the fraction value = = 0.93258.
Proton of atomic mass from = Isotopic mass x Abundance
= 38.9637 x 0.93258
= 36.337 amu
Therefore, Proton of atomic mass from is 36.337 amu.
For
Given
Isotopic mass = 40.9618 amu
Abundance = 6.730%
Calculate the fraction value = = 0.06730
Poton of atomic from = Isotopic mass x Abundance
= 40.9618 x 0.06730
= 2.757 amu.
Therefore, proton of atomic mass from is 2.757 amu.
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