Question

# A 25.00 mL sample of an H2SO4 solution of unknown concentration is titrated with a 0.1322...

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.

#### Homework Answers

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 & H2SO4 is : 2KOH + H2SO4 K2SO4 + 2H2O

According to the balanced equation ,

2 moles of KOH reacts with 1 mole of H2SO4

5.45x10-3 mol of KOH reacts with M mole of H2SO4

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

= 2.72x10-3 mol

So the number of moles of H2SO4 reacted with KOH is 2.72x10-3 mol

Given volume of H2SO4 sample is 25.00 mL = 25.00/1000 = 0.025 L

So concentration of H2SO4 , M = number of moles / volume of H2SO4 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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