Calculating Osmotic Pressure: Ammonium Sulfate & Sucrose

Thread starter moil60
Start date Nov 14, 2009
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Pressure

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When calculating the osmotic pressure of a solution containing 0.03M ammonium sulfate and 0.04M sucrose, the ammonium sulfate dissociates into three particles: two ammonium ions and one sulfate ion, resulting in an effective concentration of 0.09M. The sucrose, being a non-ionic solute, does not dissociate and should be added directly to the total concentration. Therefore, the total concentration for osmotic pressure calculation would be 0.09M from ammonium sulfate plus 0.04M from sucrose, leading to a final concentration of 0.13M.

Nov 14, 2009

moil60

when calculating the osmotic pressure of a solution with 0.03M ammonium sulfate and 0.04M sucrose...do i need to add the concentration for sucrose?

2 ions of ammonium
1 ion of sulphate

3 x 0.03M = 0.09M

do i need to add the 0.04M ?

thanks

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Nov 15, 2009

sameeralord

I'm no expert but I think you should add it. As it is not ionized you can just add it. I might be wrong!

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