A chemist mixes equal volumes of $0\mathrm{.}1$ M HF and $0\mathrm{.}005$ M NaF. What is the reason why this solution will not make an effective buffer solution? Question $5$Answer A$.$The concentrations of HF and NaF are too low for an effective buffer solution B$.$HF is not a weak acid, and NaF is not a salt of a weak acid C$.$The concentrations of weak acid and weak base components differ by more than $10$x in this solution D$.$In an effective buffer solution, the concentration of the weak base component should be higher than the concentration of the weak acid component E$.$The solution does not contain a mixture of a weak acid its conjugate base