One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.   Suppose an EPA chemist tests a 200.mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl3(aq)+3AgNO3(aq)→3AgCl(s)+FeNO33(aq) The chemist adds 56.0mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 5.0mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with tin(IT) chloride, which would react with silver nitrate solution like this: SnC12(aq) + 2AgNO3(aq) -> 2 AgCI(s) + Sn(NO3)2(aq) The chemist adds 69.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 6.2 mg of silver chloride. Calculate the concentration of tin(I) chloride contaminant in the original groundwater sample, Round your answer to 2 significant digits.

3. Give the net ionic equation for the reaction (if any). that occurs when aqueous solutions of K2S and Fe(NO;)2 are mixed. A) K*(aq) + NO;(aq) – KNO;(s) B) No reaction occurs. C) Fe"(aq) + S³(aq) + 2 K^(aq) + 2 NO;(aq) → FeS(s) + 2 K“(aq) +2 NO;(aq) D) Fe"(aq) + S²(aq) + 2 K*(aq) + 2 NO;(aq) → Fe²"(aq) + s²(aq) + 2 KNO3(s) E) Fe2(aq) + S²-(aq) FeS(s)

The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding silver nitrate, it is possible effectively to remove all chloride ion from the sample. Ag+(aq) + Cl-(aq) → AgCl(s) Suppose a 1.515 g sample is known to contain 27.5% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample?