Posted by **luke** on Wednesday, January 30, 2013 at 5:26am.

Consider

Ba (NO₃)₂ + K₂SO₄ → BaSO₄ + 2KNO₃

(0.10 M) (0.10 M)

(10.0 mL) (20.0 mL)

Will the K₂SO₄ be sufficient to precipitate all the Ba⁺˛ ions in the Ba (NO₃)₂? Use Stoichiometry to answer this question.

- chemistry -
**Devron**, Wednesday, January 30, 2013 at 1:03pm
The equation shows that 1 mole of K₂SO₄ is needed to react with mole of Ba ions.

Just eyeballing the numbers that you provided, the K₂SO₄ that you provided is in excess compared to Ba ions in the reaction. Therefore, the amount of K₂SO₄ will be sufficient to precipitate Ba.

If you need to know how to do this calculation wise, Molarity*volume in L=moles

convert mL to L by multiplying the volume by 10^-3.

moles of K₂SO₄>Ba (NO₃)₂, Ba will precipitate.

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