The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)

0.20M

Explanation:

First let us generate a balanced equation for the reaction. This is illustrated below:

H2SO4 + 2LiOH —> Li2SO4 + 2H2O

From the equation above,

nA (mole of the acid) = 1

nB (mole of the base) = 2

Data obtained from the question include:

Ma =?

Va = 25.0mL

Mb = 0.12 M

Vb = 83.6 mL

The concentration of the acid can be obtain as follows:

MaVa/MbVb = nA/nB

Ma x 25/ 0.12 x 83.6 = 1/2

Cross multiply to express in linear form as shown below:

Ma x 25 x 2 = 0.12 x 83.6

Ma x 50 = 10.032

Divide both side by 50

Ma = 10.032/50

Ma = 0.20M

The concentration of the acid is 0.20M

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atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8