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anonymous

  • one year ago

What is the molarity of barium chloride, BaCl2, in the final solution prepared by dissolving 2.50 g of barium chloride dihydrate, BaCl2 • 2 H2O , in enough water to make 400. mL of solution?

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  1. Rushwr
    • one year ago
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    \[Molarity = \frac{ Moles of BaCl2 }{ Volume of the solution }\]

  2. Rushwr
    • one year ago
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    First find the no. of moles of BaCl2 Use n= mass / molar mass

  3. cuanchi
    • one year ago
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    1) calculate the molecular mass of the BaCl2 • 2 H2O, look for the atomic mass of the elements in the periodic table and and include the H2O too 2) calculate the number of moles in 2.50g of BaCl2 • 2 H2O 2.50 g BaCl2 • 2 H2O x 1 mol BaCl2 • 2 H2O/ molecular mass BaCl2 • 2 H2O = ??? 3) calculate the molarity M= moles of solute /L solution moles of BaCl2 • 2 H2O / 0.400L =????

  4. anonymous
    • one year ago
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    Oh okay. I didn't think that you would need to add the molar mass of the dihydrate so I just used the molar mass of BaCl2. Thanks!

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