A student performed a conductimetric titration for the reaction between sulfuric
ID: 539248 • Letter: A
Question
A student performed a conductimetric titration for the reaction between sulfuric acid and barium hydroxide. The student transferred 15.0 mL Ba(OH)_2 solution to a 250-mL beaker. The student added 50 mL of distilled water to the beaker. The student recorded the equivalence point volume to be 7.8 mL for the 0.100 M H_2SO_4. From this data determine: a. Write a balanced chemical equation showing phases. b. Moles of H_2SO_4 used to reach the equivalence point. c. Moles of Ba(OH)_2 reacted. d. Molarity of the original Ba(OH)_2 solutionExplanation / Answer
a. balanced equation.
Ba(OH)2 (aq) + H2SO4(aq) -----> BaSO4(s) + 2H2O(l)
b. no of mole of H2SO4 used = v*M = 7.8*0.1/1000 = 0.00078 mole
c. from equation ,
no of mole of Ba(OH)2 reacted = no of mole of H2SO4
so that,
no of mole of Ba(OH)2 reacted = 0.00078 mole
d. Molarity of Ba(OH)2 reacted = n/V = 0.00078 / 0.015 = 0.052 M
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