Question

A titration analysis was done to determine the arsenic acid (H3AsO4) content of an impure sample. The titrant used is a 0.454 M NaOH solution. A. What mass of solid NaOH is needed to prepare a 500.0 mL solution of 0.454 M NaOH? B. Give the balanced equation of the reaction. (Hint: Consider the following half-reaction of the full dissociation of arsenic acid; H3AsO4 ? 3H+ + AsO43-) To prepare the analyte for titration, a 0.3000 g impure arsenic acid sample was dissolved in 25.00 mL water. This solution was then titrated with the NaOH standard. C. Calculate the molarity of the 25.00 mL arsenic acid solution if the initial volume of the titrant in the burette is 44.32 mL, and the final volume at endpoint is 32.74 mL. D. From the molarity of the arsenic acid, calculate the grams of pure arsenic acid present in the solution. E. What is the percent purity of the arsenic acid sample?

          A titration analysis was done to determine the arsenic acid (H3AsO4) content of an impure sample. The titrant used is a 0.454 M NaOH solution.
A. What mass of solid NaOH is needed to prepare a 500.0 mL solution of 0.454 M NaOH?
B. Give the balanced equation of the reaction.
(Hint: Consider the following half-reaction of the full dissociation of arsenic acid; H3AsO4 ? 3H+ + AsO43-)
To prepare the analyte for titration, a 0.3000 g impure arsenic acid sample was dissolved in 25.00 mL water. This solution was then titrated with the NaOH standard.
C. Calculate the molarity of the 25.00 mL arsenic acid solution if the initial volume of the titrant in the burette is 44.32 mL, and the final volume at endpoint is 32.74 mL.
D. From the molarity of the arsenic acid, calculate the grams of pure arsenic acid present in the solution.
E. What is the percent purity of the arsenic acid sample?

Added by Jacky J.

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