For the Following Elementary Reaction: HF + NH₃ → F^-

For the following elementary reaction: HF + NH₃ → F^- + NH₄⁺. The rate of consumption of the reactants and rate of formation of products is given by which set of expressions?

A)
$\frac{\mathrm{d}[\mathrm{HF}]}{\mathrm{d} t}=\frac{\mathrm{d}\left[\mathrm{NH}_{s}\right]}{\mathrm{d} t}=\frac{\mathrm{d}\left[\mathrm{F}^{-}\right]}{\mathrm{d} t}=\frac{\mathrm{d}\left[\mathrm{NH}_{a}^{*}\right]}{\mathrm{d} t}$
B) $\frac{\mathrm{d}[\mathrm{HF}]}{\mathrm{d} f}=\frac{3 \mathrm{~d}\left[\mathrm{NH}_{g}\right]}{\mathrm{d} t}=\frac{\mathrm{d}\left[\mathrm{F}^{-}\right]}{\mathrm{d} t}=\frac{4 \mathrm{~d}\left[\mathrm{NH}_{\mathrm{a}}^{\cdot}\right]}{\mathrm{d} t}$
C) $-\frac{d[\mathrm{HF}]}{d t}=-\frac{d\left[\mathrm{NH}_{3}\right]}{d t}=\frac{d\left[\mathrm{~F}^{-}\right]}{d t}=\frac{d\left[\mathrm{NH}_{\mathrm{a}}^{*}\right]}{d f}$
D) $\frac{d[\mathrm{HF}]}{d t}=\frac{d\left[\mathrm{NH}_{0}\right]^{0}}{d f}=\frac{d\left[\mathrm{~F}^{-}\right]}{d f}=\frac{d\left[\mathrm{NH}_{\mathrm{a}}\right]^{a}}{d f}$