Ask questions and get helpful answers.

A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered and dried and found to have a mass of 258 mg. What mass of baium was in the original solution? (Assume that all of the barium was precipitated out of solution by the reaction)

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
3 answers
  1. 258 mg BaSO4 = 0.258 g.
    mols BaSO4 = 0.258/molar mass BaSO4.
    mols Ba = same as mols BaSO4,
    g Ba = mols x atomic mass Ba

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
  2. Na2SO4(aq) + Ba(aq)-> BaSO4(s) + 2Na(aq)

    .258gr BaSO4 x 1 mol BaSO4/ 233.4 gr BaSO4 x 1 mol Ba/1 mol BaSO4 x 137.33 grams Ba/1 mol Ba = .152 grams of Ba

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
  3. A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered and dried and then found to have a mass of 266 mg.

    Answer: m(Ba+2)=157 mg

    Balanced Chemical Equation: Ba + Na2SO4 --> BaSO4 + 2 Na

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩

Answer this Question

Similar Questions

  1. general chem

    Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Nickel metal is added to a solution of copper (II) nitrate; (b) a solution of zinc nitrate is added to a

  2. ap chem

    A 1.42 g. sample of a pure compound, with formula M2SO4, was dissolved in water and treated with and excess of aqueous barium chloride, resulting in the precipitation of all the sulfate ions as barium sulfate. The precipitate was collected, dried, and

  3. Chemistry

    An unknown nonelectrolyte and nonvolatile compound is dissolved in enough pure water to make 229 ml of solution. The vapour pressure above the solution drops from 233.7 torr to 229.1 torr when 82.3g of the compound is dissolved at constant temperature.

  4. ap chemistry

    what mass of barium sulfate can be produced when 100 ml 0.100 M of solution of barium chloride is mixed with 100.0 ml of a 0.100 M solution of Iron (III) sulfate

  5. chemistry

    Hydrochloric acid(75.0 ml of 0.250 M) is added to 225.0 ml of 0.0550 M Barium hydroxide solution. What is the concentration of the excess H+ or OH- ions left in this solution?

  6. Chemistry

    5.85 g of sodium chloride(NaCl) is dissolved in 250 mL OF solution. Calculate mass percentage of the solute.

  7. Chemistry

    a precipitate is expected when an aqueous solution of potassium iodide is added to an aqueous solution of: sodium sulfate iron(II) chloride calcium perchlorate barium hydroxide lead nitrate

  8. Chemistry PLEASE HELP!!

    Procedure: 1. Calculate the mass of iron(II) ammonium sulfate hexahydrate, Fe(NH©þ)©ü(SO©þ)©ü*6H©üO (MW = 392.14) required to make 100 mL of solution that is 0.2M in Fe©÷⁺ ions. You will be asked to show your calculation in the Assignment. 2.

  9. chemistry

    5.34g of salt of formula M2SO4 (M is a metal)were dissolved in water. The sulfate ion was precipitated by adding excess barium chloride solution when 4.66g of barium sulfate (BaSO4) were obtained. a)How many moles of sulfate ion were precipitated as barium

  10. chemistry

    Given a solution containing 0.242 g of aqueous barium chloride, BaCl2, how many mL of 0.0581 M H2SO4 solution will completely precipitate the barium ions, Ba2+? The molar mass of BaCl2 is 208.3 g/mol.

Still need help?

You can ask a new question or browse existing questions.