Use P = MRT to calculate the osmotic pressure of 34.2 g sucrose. You will need to assume a volume.
Then P = iMRT for KBr.
OR you can do it the easy way and realize that there is one particle in sucrose, two in KBr. Determine mols sucrose, then calculate g KBr required for half the mols sucrose. I suspect this is the way the prof/book/notes/ whatever intended for the problem to be worked since no volume was given. Check my thinking.
What mass of the ionic substance KBr would result in the same osmotic pressure as 34.2 g of nonionic sucrose (C12H22O11)?
A little step by step walk through would help me. Thanks
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