anonymous
  • anonymous
If 2.891g of Mg Cl2 is dissolved in enough water to make 300.0mL of solution what is the molarity of the magnesium chloride solution? The molecular mass of magnesium chloride 95.3g/mol and the density of the solution is 1.22g/mol.
Chemistry
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jamiebookeater
  • jamiebookeater
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aaronq
  • aaronq
Find the moles of magnesium chloride, divide by volume of solution. \(\sf moles=\dfrac{mass}{Molar~Mass}\) \(\sf Molarity=\dfrac{moles~of~solute}{L~of~solution}\)
anonymous
  • anonymous
Its asking for the molarity of magnesium chloride within the solution.
anonymous
  • anonymous
these are the possible answers to the problem .5505 Mol 5.782 Mol 5.782 x 10^-3 Mol 6.703 x 10^-2 Mol Also just noticed but is supposed to be 500mL not 300 mL.

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aaronq
  • aaronq
what i posted above is how you find the molarity of MgCl2 in the solution.
aaronq
  • aaronq
i got 0.06067 M
aaronq
  • aaronq
it's pretty much D, 0.06067 M = 6.07*10^-2 M that digit is likely an error
anonymous
  • anonymous
what are you dividing? I did 500/1.22 and got 409.83 moles of solution. I did 2.891/95.3 and got 0.303357 moles of MgCl2 I did 500/95.3 and got 5.2465
aaronq
  • aaronq
"density of the solution is 1.22g/mol." this is wrong mol is not a unit of volume, its a typographical error and they mean mL, 1.22 g/mL you dont need the density to solve the question though. i found moles, first \(\sf moles=\dfrac{2.891~ g}{95.3~ g/mol}\) then divided by the volume of solution (in liters) \(\sf Molarity=\dfrac{(\dfrac{2.891~ g}{95.3~ g/mol})} {0.5~L}\)
anonymous
  • anonymous
ok I got it now. thank you for the explaination.

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