Question

A
25.00 mL sample of an H2SO4 solution of unknown concentration is
titrated with a 0.1322 M KOH solution. A volume of 41.22 mL of KOH
is required to reach the equivalence point. What is the
concentration of the unknown H2SO4 solution? Express your answer in
molarity to four significant figures.

Answer #1

Number of moles of KOH , n = Molarity x volume in L

= 0.1322 M x (41.22/1000) L

= 5.45x10^{-3} mol

The reaction between KOH & H_{2}SO_{4} is :
2KOH + H_{2}SO_{4}
K_{2}SO_{4} + 2H_{2}O

According to the balanced equation ,

2 moles of KOH reacts with 1 mole of
H_{2}SO_{4}

5.45x10^{-3} mol of KOH reacts with M mole of
H_{2}SO_{4}

M = ( 1x= 5.45x10^{-3} ) / 2

= 2.72x10^{-3} mol

So the number of moles of H_{2}SO_{4} reacted
with KOH is 2.72x10^{-3} mol

Given volume of H_{2}SO_{4} sample is 25.00 mL =
25.00/1000 = 0.025 L

So concentration of H_{2}SO_{4} , M = number of
moles / volume of H_{2}SO_{4} in L

= ( 2.72x10^{-3} mol) / 0.025 L

= 0.1089 M

Therefore the molarity of unknown solution is 0.1089 M

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