When the barium chloride test is performed on a known solution of 0.1 M $N a_{2} S O_{4}$ $Na_2SO_4$ , what do you expect the observed results to be?

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Answer 1 · 2016-03-04T21:32:23

I expect to see a white precipitate.

If you add a solution of barium chloride to a solution of sodium sulfate, barium sulfate forms.

Barium sulfate is insoluble in water. It appears as a white precipitate.

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The equation for the reaction is

${BaCl}_{2} (aq) + {Na}_{2} {SO}_{4} (aq) \to {BaSO}_{4} (s) + 2NaCl(s)$ $"BaCl"_2("aq") + "Na"_2"SO"_4("aq") → "BaSO"_4("s") + "2NaCl(s)"$

The net ionic reaction is

${Ba}^{2 +} (aq) + {SO}_{4}^{2-} (aq) \to {BaSO}_{4} (s)$ $"Ba"^(2+)("aq") + "SO"_4^"2-"("aq") → "BaSO"_4("s")$

When the barium chloride test is performed on a known solution of 0.1 M Na2SO4Na_2SO_4, what do you expect the observed results to be?