The titration of a 20.0 ml sample of an h2so4 solution of unknown concentration requires 22.87 ml of a 0.158 m koh solution to reach the equivalence point. what is the concentration of the unknown h2so4 solution?

The concentration of 20.0 mL H2SO4 solution that requires 22.87 mL of a 0.158 M KOH solution to reach equivalence point is 0.0904 M. or 0.0904 moles/L

In the question given;

The equation for the reaction is:

H2SO4 + 2KOH = K2SO4 + 2H2O

Number of moles = Molarity x Volume  

Molarity of KOH is 0.158 M  

Volume of KOH is 22.87 mL or 0.02287 L

Therefore;

Number of moles = 0.158 M x 0.02287 mL

                            = 0.003613 Moles of KOH  

Mole ratio; from the equation, 1 mole of H2SO4 requires 2 moles of KOH

Therefore;

0.003613 moles of KOH requires  

   = 0.003613/2  

   = 0.001807 Moles  

Molarity = Number of moles / Volume  

Number of moles = 0.001807 moles  

Volume = 20 mL or 0.020 L  

Therefore;

Concentration = 0.001807/ 0.020  

                       = 0.0904 M

Hence, the concentration of the acid, H2SO4 was 0.0904 M or 0.0904 moles/L

Keywords: Molarity, Moles, Volume

Level: High School

Subject: Chemistry

Chapter: Mole and stoichiometry equations

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