A solution is made by adding 23.1 mL of concentrated nitric acid ( 70.4 wt% , density 1.42 g/mL ) to some water in a volumetric flask, and t

Question

A solution is made by adding 23.1 mL of concentrated nitric acid ( 70.4 wt% , density 1.42 g/mL ) to some water in a volumetric flask, and then adding water to the mark to make exactly 200 mL of solution. Calculate the concentration of this solution in molarity.

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Nick 1 year 2021-08-01T22:58:04+00:00 1 Answers 24 views 0

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    2021-08-01T22:59:08+00:00

    Answer:

    The correct solution is “3.6975 M“.

    Explanation:

    The given values are:

    Volume of solution,

    V = 23.2 mL

    Density,

    D = 1.42 g/mL

    Final volume,

    = 200 mL

    or,

    = 0.2 L

    Now,

    The mass will be:

    = [tex]D\times V[/tex]

    = [tex]1.42\times 23.1[/tex]

    = [tex]32.802 \ g[/tex]

    Mass of HNO₃ will be:

    = [tex]\frac{32.802}{0.704}[/tex]

    = [tex]46.59375 \ g[/tex]

    Mol of HNO₃ will be:

    = [tex]\frac{mass}{MW}[/tex]

    = [tex]\frac{46.59375}{63}[/tex]

    = [tex]0.7395 \ mol[/tex]

    hence,

    The concentration will be:

    = [tex]\frac{mol \ of \ HNO_3}{final \ V}[/tex]

    = [tex]\frac{0.7395}{0.2}[/tex]

    = [tex]3.6975 \ M[/tex]

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