# How do we produce a stoichiometrically balanced equation for the formation of BaSO_4?

Jan 29, 2017

You balance it stoichiometrically.

#### Explanation:

And stoichiometry INSISTS that charge be balanced, AND mass be balanced. Experiment tells us that barium sulfate is insoluble in aqueous solution.

And thus:

$B a C {l}_{2} \left(a q\right) + N {a}_{2} S {O}_{4} \left(a q\right) \rightarrow B a S {O}_{4} \left(s\right) \downarrow + 2 N a C l \left(a q\right)$

The water solvate on the barium chloride is along for the ride in aqueous solution.

We could write the net ionic equation as follows:

$B {a}^{2 +} + S {O}_{4}^{2 -} \rightarrow B a S {O}_{4} \left(s\right) \downarrow$

${K}_{\text{sp,}}$ $B a S {O}_{4}$ $=$ 1.0842 xx10^(−10).

If you need further help working out the gram solubility from ${K}_{\text{sp}}$ say the word..........