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I'm totally confused about this question....I don't know what kind of an answer the teacher is looking for. The worksheet has the header "Preparation of solutions for Beer's Law Lab."
That's the question: Describe the preparation of 250.0mL of a 0.10 M sucrose (C12H22O11) stock solution from solid Kool-Aid powder. One serving is 17g, which contains 16 g of sucrose. Use distilled water when actually making the solution.

  • chemisty - ,

    Weigh out 17 g Kool-Aid accurately (I would use an analytical balance). That contains 16 g sucrose. How many moles is that? moles = grams/molar mass
    Add the powder to a 250 mL volumetric flask, add a little water, swirl until all of the powder is dissolved, then add water to the mark. That will give you M = moles/L soln for the stock solution.

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