A solution contains 0.018 moles each of I',Br'' and Cl^- When the solution is mixed with 200 mL of 0.24MAgNO_(3), how much AgCl(s) precipitates out? KspAgI=1.5times 10^-16 Ksp AgBr=5.0times 10^-13 Ksp AgCl=1.6times 10^-10 2.6g 3.3 g 0.0 g 1.7 g 5.0 g

1. Calculate moles of added moles 2. Determine precipitation order (lowest first) Order: ( ), then , then 3. Precipitate moles react with moles to form . Remaining moles.4. Precipitate moles react with moles to form . Remaining moles.5. Check if will precipitate , Since , all will react with until one is exhausted.6. Calculate moles of formed moles left, so moles can form.7. Convert moles to grams Molar mass