1. The problem statement, all variables and given/known data The arsenic in a 1.42 g sample of pesticide was converted to AsO43- by suitable chemical treatment. It was then titrated using Ag+ to form Ag3AsO4 as a precipitate. If it took 33.7 mL of 0.113 M Ag+ to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide? 2. Relevant equations im not sure 3. The attempt at a solution I just need a way to get the ball rolling, this is a questions for my AP Chemistry summer review and i havent taken chemistry since sophomore year (im going to be a senior when school starts in two days) and i forgot the equations i need to solve this kind of stuff.