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Dilution Question

  1. Oct 4, 2007 #1
    1. Concentrated h2so4 solution is 98% by weight and has a density of 1.84% g/mL . A volume of 21.75 mL of this solution was diluted to 500 mL and has a density of 1.09 g/mol. What is the molarity of the resulting solution?



    2. M1V1 = M2V2
    molarity = moles/litres which is also = grams of solutes / MM x litres of solution




    3. Well basically this is my approach but i know im missing something because I dont even use all the values in the question given

    98g/100g x 1.84 g/mL x 1000mL/1L x 1mol/98.03g = M1 = 18.39 M

    v1 = 21.75 mL = 0.02175 L

    v2 = 500 mL = .5 L

    So now i just calculate M2

    M1V1=M2V2
    but then why is the denisty of the diluted solution given ???
     
    Last edited: Oct 4, 2007
  2. jcsd
  3. Oct 4, 2007 #2

    Gokul43201

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    It is unnecessary. But if you wish, you can also find the final density and see how it compares with the number they gave you. Hopefully, it'll be pretty close.
     
  4. Oct 4, 2007 #3
    so what i did was correct?

    thats how to find MOLARITY of the resulting solution.
     
  5. Oct 4, 2007 #4

    Gokul43201

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    Yes, your calculation will give the correct answer (for final molarity).
     
  6. Oct 5, 2007 #5
    Thanks:)
     
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