Chemistry Help! A student performed a conductimetric titration for the reaction

Question

Chemistry Help! A student performed a conductimetric titration for the reaction between sulfuric acid and barium hydroxide. The student transferred 15.0 mL Ba(0H)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 H2SO4. From this data determine: a. Write a balanced chemical equation showing phases. Moles of H2SO4 used to reach the equivalence point. Moles of Ba(OH)2 reacted. Molarity of the original Ba[OH]2 solution

Explanation / Answer

a.

   Ba(OH)2 + H2SO4 -------> BaSO4 + H2O

b.

   Molarity = Moles / liter

    mole     = M * V

               = ( 0.1 ) * (7.8*10-3)L

moles of H2SO4 required to reach the equivalence point              = 7.8 * 10-4 moles

c.

   

   Molarity = Moles / liter

    mole     = M * V

               = ( 0.052 ) * (0.015)L

moles of Ba(OH)2 required to reach the equivalence point              = 7.8 * 10-4 moles

d.

7.8 ml of 0.100M H2SO4 = 15ml of ? M Ba(OH)2

                      M1V1          =   M2V2

                 (0.100)(7.8)           = M2 * 15

   Molarity of Ba(OH)2 solution is ,     M2       = 0.052M

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