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5 October, 07:42

You have 10 ml of ethanol and want to use it all to make a 10-fold dilution with water. How would you do this, including the final volume? Show your calculations and give complete instructions.

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  1. 5 October, 09:53
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    You should add water to the 10 ml ethanol until you have a 100-ml solution. For this, pour the 10 ml ethanol in a 100-ml volumetric flask and add water until the mark that indicates that you have a volume of 100 ml. Don't forget to mix before you reach the mark.

    Explanation:

    You can assume that your ethanol has a concentration of 1X.

    if you have to dilute it ten times, the final concentration will be 1X / 10 = 0.1X

    The number of moles of ethanol present in the solution will remain the same after the dilution because you are not adding nor substracting ethanol, that means:

    mol ethanol before dilution = mol ethanol after dilution

    The number of moles can be expressed in this form:

    mol ethanol = volume of the solution * concentration of ethanol

    then, to find how much water you have to add you have to solve the final volume (Vf) from this equation:

    mol ethanol before dilution = mol ethanol after dilution

    Vi * Ci = Vf * Cf

    where:

    Vi = volume of the solution before dilution.

    Ci = concentration of the solution before dilution

    Vf = volume of the final solution

    Cf = concentration of the final solution

    Replacing with the dа ta:

    10 ml * 1X = Vf * 0.1X

    10 ml * 1X / 0.1X = Vf

    100 ml = Vf
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