Chapter 18, Problem 54E

For the following system, $\text{K}=4.86\times {10}^{-5}$ at $298\text{K}$: $\text{HClO}\left(\text{aq}\right)+{\text{F}}^{-}\left(\text{aq}\right)\rightleftharpoons {\text{ClO}}^{-}\left(\text{aq}\right)+\text{HF}\left(\text{aq}\right)$ Assuming that you start with equal concentrations of $\text{HClO}$ and ${\text{F}}^{-}$, and that no ${\text{ClO}}^{-}$ or $\text{HF}$ is initially present, which of the following best describes the equilibrium system: (a) the forward reaction is favored at equilibrium; (b) the reverse reaction is favored at equilibrium; (c) appreciable quantities of all species are present at equilibrium?