Write the charge and mass balances for dissolving ${\mathbf{CaF}}_{\mathbf{2}}$ in water if the reactions are

role="math" localid="1654770961556" $$\begin{gathered} {\mathbf{CaF}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ٟ}\mathbf{}\mathbf{}\mathbf{}\mathbf{}{\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{+}\mathbf{2}\mathbf{F} \\ {\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{ٟ}\mathbf{}\mathbf{}\mathbf{}\mathbf{}{\mathbf{CaOH}}^{\mathbf{+}}\mathbf{+}{\mathbf{H}}^{\mathbf{+}} \\ {\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{F}\mathbf{ؚ}\mathbf{}\mathbf{}\mathbf{}\mathbf{}{\mathbf{CaF}}^{\mathbf{+}}{\mathbf{CaF}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{ؚ}\mathbf{}\mathbf{}\mathbf{}{\mathbf{CaF}}_{\mathbf{2}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)} \\ \mathbf{F}\mathbf{+}{\mathbf{H}}^{\mathbf{+}}\mathbf{}\mathbf{ؚ}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{HF}\mathbf{\left(}\mathbf{aq}\mathbf{\right)} \\ \mathbf{HF}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{F}\mathbf{}\mathbf{ؚ}\mathbf{}\mathbf{}\mathbf{}{\mathbf{HF}}_{\mathbf{2}} \end{gathered}$$

• Calcium fluoride (CaF2) is an inorganic compound made up of the elements calcium and fluorine.
• It's an insoluble white solid. Fluorite (also known as fluorspar) is the mineral form, which is often richly coloured due to impurities.

The dissolving charge and mass balances${\mathrm{CaF}}_2$It must be given in water.

Balance of charge: [C] -concentration of a cation and n-charge of the cation.

The [A] -concentration of an anion and the m-magnitude of the anion's charge.

The total number of species in a solution containing a certain atom (or group of atoms) must equal the total amount of that atom (or group) given to the solution (mass balance)..

In the given information,

$$\begin{gathered} {\mathrm{CaF}}_2\left(\mathrm{s}\right)\mathrm{ٟ}{\mathrm{Ca}}^{2+}+2\mathrm{F} \\ {\mathrm{Ca}}^{2+}+{\mathrm{H}}_2\mathrm{O}\mathrm{ٟ}{\mathrm{CaOH}}^{+}+{\mathrm{H}}^{+} \\ {\mathrm{Ca}}^{2+}\mathrm{F}\mathrm{ؚ}{\mathrm{CaF}}^{+}{\mathrm{CaF}}_2\left(\mathrm{s}\right)\mathrm{ؚ}{\mathrm{CaF}}_2\left(\mathrm{aq}\right) \\ \mathrm{F}+{\mathrm{H}}^{+}\mathrm{ؚ}\mathrm{HF}\left(\mathrm{aq}\right) \\ \mathrm{HF}\left(\mathrm{aq}\right)+\mathrm{F}\mathrm{ؚ}{\mathrm{HF}}_2 \end{gathered}$$

On the basis of electroneutrality, charge balance:

role="math" localid="1654771916727" $\left[{\mathrm{F}}^{-}\right]+\left[{\mathrm{HF}}_2^{-}\right]+\left[{\mathrm{OH}}^{-}\right]=2\left[{\mathrm{Ca}}^{2+}\right]+\left[{\mathrm{CaOH}}^{+}\right]+\left[{\mathrm{CaF}}^{+}\right]+\left[{\mathrm{H}}^{+}\right]$

By definition, the process's mass balance is determined by ${\mathrm{CaF}}_2$

gives 2 m ol F for each molCa.

$$\begin{gathered} \underset{\mathrm{species}\mathrm{containing}\mathrm{F}}{\underbrace{\left[{\mathrm{F}}^{-}\right]+\left[{\mathrm{CaF}}^{+}\right]+2\left[{\mathrm{CaF}}_{2\left(\mathrm{aq}\right)}\right]+\left[{\mathrm{HF}}^{-}\right]+2\left[{\mathrm{HF}}_2^{-}\right]}} \\ =\underset{\mathrm{species}\mathrm{containing}{\mathrm{Ca}}^{2+}}{\underbrace{2\left\{\left[{\mathrm{Ca}}^{2+}\right]+\left[{\mathrm{CaOH}}^{+}\right]+\left[{\mathrm{CaF}}^{+}\right]+2\left[{\mathrm{CaF}}_{2\left(\mathrm{aq}\right)}\right]\right\}}} \end{gathered}$$

Charge and mass balances for calcium fluoride dissolution$\left({\mathrm{CaF}}_2\right)$ it was provided in water.