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

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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