If 38.17 mL of 0.1072 M NaOH is required to titrate a 15.00 mL sample of sulfuric acid, what is the molarity of the acid?
The balanced equation is
2NaOH + H2SO4 ----- > Na2SO4 + 2H2O
Number of moles of NaOH = molarity * volume of solution in L
Number of moles of NaOH = 0.1072 * 0.03817 = 0.00409 mole
From the balanced equation we can say that
2 mole of NaOH requires 1 mole of H2SO4 so
0.00409 mole of NaOH will require 0.00205 mole of H2SO4
molarity of H2SO4 = number of moles of H2SO4 / volume of solution in L
molarity of H2SO4 = 0.00205 / 0.015 = 0.137 M
Therefore, the molarity is 0.137 M
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