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1 April, 04:59

If 0.500 L of a 4.00-M solution of copper nitrate, Cu (NO3) 2, is diluted to a volume of 1.50 L by the addition of water, what is the molarity of the diluted solution?

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  1. 1 April, 05:08
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    1.33 M

    Explanation:

    We'll begin by writing out the data obtained from the question. This includes the following:

    Volume of the stock solution (V1) = 0.5L

    Molarity of the stock solution (M1) = 4M

    Volume of diluted solution (V2) = 1.5L

    Molarity of the diluted solution (M2) =.?

    With the application of the dilution formula, the molarity of the diluted solution can be obtained as follow:

    M1V1 = M2V2

    4 x 0.5 = M2 x 1.5

    Divide both side by 1.5

    M2 = (4 x 0.5) / 1.5

    M2 = 1.33 M

    Therefore the molarity of the diluted solution is 1.33 M
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