anonymous
  • anonymous
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?
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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katieb
  • katieb
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Rushwr
  • Rushwr
\[Molarity = \frac{ Moles of BaCl2 }{ Volume of the solution }\]
Rushwr
  • Rushwr
First find the no. of moles of BaCl2 Use n= mass / molar mass
Cuanchi
  • Cuanchi
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 =????

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anonymous
  • anonymous
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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