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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

  • Chemistry -

    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.

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