(a) Write the mass balance for ${\mathbf{CaCl}}_{\mathbf{2}}$in water if the species are${\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}$ and${\mathbf{CI}}^{\mathbf{-}}$ .

(b) Write the mass balance if the species are${\mathbf{Ca}}^{\mathbf{2}\mathbf{+}}\mathbf{,}{\mathbf{CI}}^{\mathbf{-}}\mathbf{,}{\mathbf{CaCI}}^{\mathbf{+}}$ , and${\mathbf{CaOH}}^{\mathbf{+}}$

(c) Write the charge balance for part (b).

• According to a mass balance, approximately 85 percent of the lead was returned to the smelter, while 15 percent was removed with the calcium arsenate precipitate.
• A mass balance is a method of calculating the total amount of material used in a process.
• A consideration of the input, output, and distribution of a substance amongst streams in a process or stage is known as mass balance.

The mass equilibrium for${\mathrm{CaCI}}_2$It is necessary to provide water..

The mass balances for each species must be provided.

Mass balance:

All species in a solution containing a certain atom (or group of atoms) must be equal to the amount of that atom (or group) given to the solution.

(a)

If you are given information,${\mathrm{CaCI}}_2$ in the water

Species:${\mathrm{Ca}}^{2+},{\mathrm{CI}}^{-}$Mass balance:

The mass balance of the process is given by by definition.

$\left[{\mathrm{CI}}^{-}\right]=2\left[{\mathrm{Ca}}^{2+}\right]$

(b)

If you are given information,

Species:${\mathrm{Ca}}^{2+},{\mathrm{CI}}^{-},{\mathrm{CaCI}}^{+}\mathrm{and}{\mathrm{CaOH}}^{+}$and

By definition, the process's mass balance is determined by

$\underset{\mathrm{species}\mathrm{containie}{\mathrm{CI}}^{-}}{\underbrace{\left[{\mathrm{CI}}^{-}\right]+\left[{\mathrm{CaCI}}^{+}\right]}}\underset{\mathrm{species}\mathrm{containing}{\mathrm{Ca}}^{2+}}{=\underbrace{2\left\{\left[{\mathrm{Ca}}^{2+}\right]+\left[{\mathrm{CaCI}}^{+}\right]+\left[{\mathrm{CaOH}}^{+}\right]\right\}}}$

(c)

It is necessary to provide the charge balance for the species listed in item (b).

Charge balance is achieved when the total positive charges in a solution are equal to the total negative charges in the solution

${\mathrm{n}}_1\left[{\mathrm{C}}_1\right]+{\mathrm{n}}_2\left[{\mathrm{C}}_2\right]+......={\mathrm{m}}_1\left[{\mathrm{A}}_1\right]+{\mathrm{m}}_2\left[{\mathrm{A}}_2\right]+......$

where,[C] -concentration of a cation and n-charge of the cation.

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

Given the facts,Species:${\mathrm{Ca}}^{2+},{\mathrm{CI}}^{-},{\mathrm{CaCI}}^{+}{\mathrm{andCaOH}}^{+}$

On the basis of electroneutrality, charge balance:

$\left[{\mathrm{CI}}^{-}\right]+\left[{\mathrm{OH}}^{-}\right]=2\left[{\mathrm{Ca}}^{2+}\right]+\left[{\mathrm{CaCI}}^{+}\right]+\left[{\mathrm{CaOH}}^{+}\right]+\left[{\mathrm{H}}^{+}\right]$