Answer:
[tex]\boxed{\text{58.0919 u}}[/tex]
Explanation:
1. Atomic mass of K
To get the atomic mass of K, you calculate the weighted average of the isotopic masses.
That is, you multiply the atomic mass of each isotope by a number representing its relative importance (e.g., its percent of the total).
Set up a table for easy calculation:
[tex]\begin{array}{ccrcr}\textbf{Atom} & \textbf{Mass/u} &\textbf{Percent} & \textbf{Calculation}& \textbf{Result/u}\\^{39}\text{K}& 38.9637 & 93.258 & 38.9637 \times 0.932 58 & 36.3368\\^{41}\text{K}& 40.9618 & 6.730 & 40.9618 \times 0.06730& 2.7567\\& & \text{TOTAL } = &\textbf{39.0935}\\\end{array}[/tex]
2. Formula mass of KF
[tex]\begin{array}{rcl}\text{K} & = & \text{39.0935 u}\\\text{F} & = & \text{18.9984 u}\\\text{Total} & = & \textbf{58.0919 u}\\\end{array}\\\text{The formula mass using only the two isotopes of K is $\boxed{\textbf{58.0919 u}}$}[/tex]
Based on data provided, the gormula mass of potassium fluoride, KF = 58.09
The relative atomic mass of potassium is first determined:
Relative atomic mass of potassium = 38.9637 × 93.258% + 40.9618 × 6.730%
Relative atomic mass of potassium = 39.09
Atomic mass of Fluorine = 18.9984
Formula mass of potassium fluoride, KF = 39.09 + 18.9984
Formula mass of potassium fluoride, KF = 58.09
Therefore, based on data provided, the formula mass of potassium fluoride, KF = 58.09
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