Question

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 Iron(II) chloride, which would react with silver nitrate solution like this: FeCl(aq) + 2 AgNO3(aq) + 2 AgCl(s) + Fe(NO), (0) The chemist adds 31.0 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 9.0 mg of silver chloride Calculate the concentration of Iron(II) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits MacBook Air

Answer 1

Moles of AgCl = mass of AgCl / molar mass of AgCl = 9 * 10^-3 / 143.32 = 6.28 * 10^-5 moles

From the equation, moles of FeCl₂ = moles of AgCl / 2 = 6.28 * 10^-5 / 2 = 3.14 * 10^-5 moles

Molarity of FeCl₃ * Volume in liters = moles of FeCl₃

M * 0.25 = 3.14 * 10^-5

SOlving, M = 1.26 * 10^-4 M