anonymous
  • anonymous
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
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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jamiebookeater
  • jamiebookeater
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anonymous
  • anonymous
@Peter14
shubhamsrg
  • shubhamsrg
re-check the question -_-
anonymous
  • anonymous
why?

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shubhamsrg
  • shubhamsrg
both shouldn't be h2so4
anonymous
  • anonymous
that's what I was thinking too
anonymous
  • anonymous
why not?
shubhamsrg
  • shubhamsrg
oh,,well, it can be, okay, let it be..
anonymous
  • anonymous
there's even a equation for same solute...called Dilutional equation...
anonymous
  • anonymous
does it give molarities for the two initial solutions? if not I haven't studied this.
anonymous
  • anonymous
no...i gave u the whole question..
anonymous
  • anonymous
i got molarities of both separate..i dont know how to find volume..cuz for the equation i need separate volumes and total volume..
anonymous
  • anonymous
@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
shubhamsrg
  • shubhamsrg
the language of the question confuses me molarity = total moles/toatl volume. @Peter14 please continue! :| I am confused here.
anonymous
  • anonymous
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
anonymous
  • anonymous
Also...molarity equals
anonymous
  • anonymous
if you can't find that, I have no clue.
anonymous
  • anonymous
and I have to go now, it's 22:37 which is past my bedtime
anonymous
  • anonymous
(molarity of 1solute*its volume + m of 2nd solute*its volume)/total volume in litres
anonymous
  • anonymous
@shubhamsrg does that formula help? @Peter14 goodnight...sry to have kept you awake...
shubhamsrg
  • shubhamsrg
thats just the formula I wrote -_-
anonymous
  • anonymous
so? what to do?
shubhamsrg
  • shubhamsrg
not too sure, I wouldn't direct you wrong. Not too sure on this one.
anonymous
  • anonymous
hmm..ok..one sec there's one more..

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