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1 March, 15:09

A chemist must dilute of aqueous barium chloride solution until the concentration falls to. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

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  1. 1 March, 18:30
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    Your question was incomplete so I am writing the down the complete question below for convenience

    Q) A chemist must dilute 17.8 mL of 961. mM aqueous barium chloride BaCl 2 solution until the concentration falls to 267. mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

    Answer:

    V2 = 64.0666 mL

    Explanation

    Let us first write down the data

    The Initial condition of Bacl2 solution is:-

    M1 = 961 mM

    V1 = 17.8 mL

    The chemist wants to dilute the solution to reach the concentration of 267 mM hence the final conditions will be:-

    M2 = 267 mM

    V2 = ?

    here we are going to use the simple formula to calculate V2,

    M1 * V1 = M2 * V2

    V2 = (M1 * V1) / M2

    V2 = (961*17.8) / 267

    V2 = 64.0666 mL
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