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17 March, 22:13

How many milliliters of 0.50 M KOH are needed to exactly neutralize 10 milliliters of of 1.5 M

HNO3

A. 5.0 mL

B. 12 mL

C. 25 mL

D. 30 mL

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Answers (1)
  1. 17 March, 22:18
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    Option D. 30 mL.

    Explanation:

    Step 1:

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

    HNO3 + KOH - > KNO3 + H2O

    From the balanced equation above,

    The mole ratio of the acid, nA = 1

    The mole ratio of the base, nB = 1

    Step 2:

    Data obtained from the question. This include the following:

    Volume of base, KOH (Vb) =.?

    Molarity of base, KOH (Mb) = 0.5M

    Volume of acid, HNO3 (Va) = 10mL

    Molarity of acid, HNO3 (Ma) = 1.5M

    Step 3:

    Determination of the volume of the base, KOH needed for the reaction. This can be obtained as follow:

    MaVa / MbVb = nA/nB

    1.5 x 10 / 0.5 x Vb = 1

    Cross multiply

    0.5 x Vb = 1.5 x 10

    Divide both side by 0.5

    Vb = (1.5 x 10) / 0.5

    Vb = 30mL

    Therefore, the volume of the base, KOH needed for the reaction is 30mL.
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