To assay silver content in an alloy, a 13.38 g sample of alloy was dissolved in nitric acid. The addition of 0.53 molar sodium chloride resulted in the precipitation of silver chloride. If the alloy were pure silver, what volume of sodium chloride is needed to precipitate the silver?
Chemistry - GK, Tuesday, September 30, 2008 at 10:01pm
Convert 13.38 g Of Ag to moles by dividing by the gram-atomic mass of Ag.
1 mole of Ag produces 1 mole of AgNO3
1 mole of AgNO3 + 1 mole NaCl ---> 1 mole AgCl
Moles of Ag = Moles of AgNO3 = moles of NaCl
(Moles of NaCl) / (molarity of NaCl) = liters NaCl
Chemistry - DrBob222, Tuesday, September 30, 2008 at 11:14pm
Just a quick note here to have you realize that this is a ridiculous problem. An alloy is at least two somethings together so it can't be pure silver as the problem states.