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Nikhil619

What would be the molarity of the solution obtained by mixing 30% by mass concentration of h2so4 and 70% by mass of h2so4. If the resultant solution has a density 1.425 g/ml.Calculate molarity

  • one year ago
  • one year ago

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  1. Nikhil619
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    @Peter14

    • one year ago
  2. shubhamsrg
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    re-check the question -_-

    • one year ago
  3. Nikhil619
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    why?

    • one year ago
  4. shubhamsrg
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    both shouldn't be h2so4

    • one year ago
  5. Peter14
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    that's what I was thinking too

    • one year ago
  6. Nikhil619
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    why not?

    • one year ago
  7. shubhamsrg
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    oh,,well, it can be, okay, let it be..

    • one year ago
  8. Nikhil619
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    there's even a equation for same solute...called Dilutional equation...

    • one year ago
  9. Peter14
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    does it give molarities for the two initial solutions? if not I haven't studied this.

    • one year ago
  10. Nikhil619
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    no...i gave u the whole question..

    • one year ago
  11. Nikhil619
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    i got molarities of both separate..i dont know how to find volume..cuz for the equation i need separate volumes and total volume..

    • one year ago
  12. Nikhil619
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    @shubhamsrg @Peter14 Crap! sry i frgt to give u densities... the 30% one d=1.218 70% one d=1.61..both are g/ml

    • one year ago
  13. shubhamsrg
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    the language of the question confuses me molarity = total moles/toatl volume. @Peter14 please continue! :| I am confused here.

    • one year ago
  14. Peter14
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    i'm confused here too. If I were you I would try to find a table or graph somewhere on how the concentration of h2so4 affects the density of a solution

    • one year ago
  15. Nikhil619
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    Also...molarity equals

    • one year ago
  16. Peter14
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    if you can't find that, I have no clue.

    • one year ago
  17. Peter14
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    and I have to go now, it's 22:37 which is past my bedtime

    • one year ago
  18. Nikhil619
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    (molarity of 1solute*its volume + m of 2nd solute*its volume)/total volume in litres

    • one year ago
  19. Nikhil619
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    @shubhamsrg does that formula help? @Peter14 goodnight...sry to have kept you awake...

    • one year ago
  20. shubhamsrg
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    thats just the formula I wrote -_-

    • one year ago
  21. Nikhil619
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    so? what to do?

    • one year ago
  22. shubhamsrg
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    not too sure, I wouldn't direct you wrong. Not too sure on this one.

    • one year ago
  23. Nikhil619
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    hmm..ok..one sec there's one more..

    • one year ago
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