Alright, let's solve the problem step-by-step to determine the mass percentage of fluorine in the compound.
1. Identify Given Values:
- Mass of Hydrogen (H): 5.0 grams
- Mass of Fluorine (F): 95.0 grams
2. Calculate the Total Mass of the Compound:
[tex]\[
\text{Total Mass} = \text{Mass of Hydrogen} + \text{Mass of Fluorine}
\][/tex]
[tex]\[
\text{Total Mass} = 5.0\, \text{grams} + 95.0\, \text{grams} = 100.0\, \text{grams}
\][/tex]
3. Determine the Mass Percentage of Fluorine:
[tex]\[
\text{Mass Percentage of Fluorine} = \left( \frac{\text{Mass of Fluorine}}{\text{Total Mass}} \right) \times 100\%
\][/tex]
[tex]\[
\text{Mass Percentage of Fluorine} = \left( \frac{95.0\, \text{grams}}{100.0\, \text{grams}} \right) \times 100\% = 95.0\%
\][/tex]
Therefore, the mass percentage of fluorine in the compound is [tex]\(95.0\%\)[/tex]. The correct answer is:
[tex]\[
\boxed{95.0\%}
\][/tex]
