Thursday

July 24, 2014

July 24, 2014

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

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 1:03pmThe 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.

**Related Questions**

Math: Law of Vectors (Cross Product) - (au) × v + (bu) × v = [(a + b)u] × v u...

Chemistry - Write equilibrium Constant expressions (k) for the following ...

Chem - Calculate the amount (in moles) of H₂O in 2.00g of Na₂CO&#...

Chemistry - Na₂CO₃ (s) + 2HCL (ag) → 2NaCl (ag) + CO₂ + ...

Chemistry - A propane stove burned 470. grams of propane and produced 625 ...

chemistry - Record and calculate the following masses: (a)mass of empty beaker: ...

Chemistry - I don't understand these two questions. Any help on how to figure ...

11th grade - Base your answers to the following questions using the diagram. The...

Discrete Math - Solve the recurrence relation a_n = -2a_n-1 + 15a_n-2, n ≥...

chemistry - how to solve for a 28.4 L sample of methane gas is heated from 35.0...