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

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Answer 1 · 2017-01-29T08:59:08

You balance it stoichiometrically.

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

And thus:

#BaCl_2(aq) + Na_2SO_4(aq) rarr BaSO_4(s)darr + 2NaCl(aq)#

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

We could write the net ionic equation as follows:

#Ba^(2+) + SO_4^(2-) rarr BaSO_4(s)darr#

#K_"sp,"# #BaSO_4# #=# #1.0842 xx10^(−10)#.

If you need further help working out the gram solubility from #K_"sp"# say the word..........