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8 August, 18:15

What is the concentration of an unknown Mg (OH) 2 solution if it took an average of 15.4mL of

0.100M HCl solution to neutralize 10.0mL of the Mg (OH) 2 solution?

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  1. 8 August, 21:20
    0
    0.077M

    Explanation:

    Step 1:

    The balanced equation for the reaction. This is given below:

    2HCl + Mg (OH) 2 - > MgCl2 + 2H2O

    From the balanced equation above,

    The mole ratio of the acid (nA) = 2

    The mole ratio of the base (nB) = 1

    Step 2:

    Data obtained from the question.

    Concentration of base Cb = ... ?

    Volume of base (Vb) = 10mL

    Concentration of acid (Ca) = 0.1M

    Volume of acid (Va) = 15.4mL

    Step 3:

    Determination of the concentration of the base, Mg (OH) 2.

    The concentration of the base can be obtained as follow:

    CaVa/CbVb = nA/nB

    0.1 x 15.4 / Cb x 10 = 2/1

    Cross multiply to express in linear form

    Cb x 10 x 2 = 0.1 x 15.4

    Divide both side by 10 x 2

    Cb = (0.1 x 15.4) / (10 x 2)

    Cb = 0.077M

    Therefore, the concentration of the base, Mg (OH) 2 is 0.077M
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