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When the barium chloride test is performed on a known solution of 0.1 M #Na_2SO_4#, what do you expect the observed results to be?

Answer 1

Caleb Adams

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.

The reaction is a double displacement reaction.

The equation for the reaction is

#"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") → "BaSO"_4("s")#

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Answer 2

Ellie Andrews

The barium chloride test on a 0.1 M Na2SO4 solution is expected to result in the formation of a white precipitate of barium sulfate (BaSO4) due to the reaction between barium chloride (BaCl2) and sodium sulfate (Na2SO4), following the precipitation reaction:

BaCl2(aq) + Na2SO4(aq) -> BaSO4(s) + 2NaCl(aq)

The white precipitate of barium sulfate indicates the presence of sulfate ions (SO4^2-) in the solution.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.