Problem: The arsenic in a 1.26 g sample of a pesticide was converted to AsO43- by suitable chemical treatment. It was then titrated using Ag+ to form Ag3AsO4 as a precipitate.If it took 23.0 mL of 0.106 M Ag+ to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide?

FREE Expert Solution

The reaction is:

3 Ag+(aq) + AsO4(aq) → Ag3AsO4(s) 

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Problem Details

The arsenic in a 1.26 g sample of a pesticide was converted to AsO43- by suitable chemical treatment. It was then titrated using Ag+ to form Ag3AsO4 as a precipitate.

If it took 23.0 mL of 0.106 M Ag+ to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide?

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