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28 September, 07:19

8. 71.67 g of InBr2 was dissolved in water to a final volume of 650 mL. (A) What is the molar concentration of indium in the resulting solution? (B) If 25.0 mL of the solution in part A was diluted to 75.0 mL, what is the molar concentration of the resulting solution?

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  1. 28 September, 09:17
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    A) 0.39 M is the molar solution of the resulting solution.

    B) The resulting solution will have molarity of 0.13M

    Explanation:

    The atomic weight of 2 atoms of bromine = 79.904 gms

    The atomic weight of 1 atom of In = 114.818

    Atomic weight of InBr2 = 274.26 gm

    From the data mass percentage is calculated ie. 58.19% of bromine, 41.80 % of Indium

    so from the mass of the InBr2 the percentage of indium can be calculated as

    41.088/100 * 71.67

    = 29.447 grams

    No of moles of indium = 29.04/114.818

    = 0.256 moles

    In the solution of 650 ml 0.256 moles of Indium are there

    M=n/C

    = 0.256/650ml

    = 0.256/0.65 litre

    = 0.39 M

    B) in 25 ml of the solution the molarity is 0.39 which is diluted to 75 ml ie three fold diluted the molarity decreases.

    from the formula M1V1=M2V2

    = 0.39*25 = M2 * 75

    M2 = O. 39*25/75

    = 0.13 M
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