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10 November, 01:21

Given the reaction:

2 NaOH + H2SO4 Na2SO4 + 2 H2O

How many milliliters of 1 M NaOH are needed to exactly neutralize 100 milliliters of 1 M H2SO4?

a

50 ml

b

100 ml

c

200 ml

d

400 ml

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Answers (1)
  1. 10 November, 02:01
    0
    Option C. 200mL

    Explanation:

    We'll begin by writing the balanced equation for the reaction. This is illustrated below:

    2NaOH + H2SO4 - > Na2SO4 + 2H2O

    From the balanced equation above,

    The mole ratio of the acid (nA) = 1

    The mole ratio of the base (nB) = 2

    The following data were obtained from the question:

    Molarity of the base (Mb) = 1M

    Volume of the base (Vb) = ... ?

    Molarity of the acid (Ma) = 1M

    Volume of the acid (Va) = 100mL

    The volume of the base needed can be obtained as follow:

    MaVa/MbVb = nA/nB

    1 x 100 / 1 xVb = 1/2

    Cross multiply to express in linear form

    Vb = 1 x 100 x 2

    Vb = 200mL

    Therefore, the volume of the base needed for the reaction is 200mL
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