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\begin{equation*}  \textup{\% Atom economy}=\frac{\textup{Relative formula mass of desired products}}{\textup{Relative formula mass of all reactants}}\times100  \end{equation*}  \subsection{Production of hydrochloric acid as a co-product}  A large proportion of the hydrochloric acid that is produced is a co-product from the chlorination of organic compounds. Hydrogen chloride can be converted to hydrochloric acid easily in water, due to its high solubility. The gas is made up of covalent molecules, and dissolves in water to form the hydrated ions $H^+$ and $Cl^-$.   \section*{Hydrogen Halides}  \subsection{Preparing Hydrogen Halides}  Fluorine is the strongest oxidising agent in group 7, so has the greatest tendency to be reduced:  \begin{equation*}  F_2+2e^-\Rightarrow 2F^-  \end{equation*}  Fluoride ions have a low tendency to lose electrons and turn back to atoms, so are poor reducing agents as they are difficult to oxidise.   \begin{equation*}  2F^-\Rightarrow F_2 +2e^-  \end{equation*}  \[ \xrightarrow{\hspace*{3cm}} \]