Suppose an epa chemist tests a 200.ml sample of groundwater known to be contaminated with iron(ii) chloride, which would react with silver nitrate solution like this: fecl2 (aq) + 2agno3 (aq) → 2agcl (s) + feno32 (aq) the chemist adds 14.0m m silver nitrate solution to the sample until silver chloride stops forming. she then washes, dries, and weighs the precipitate. she finds she has collected 6.9mg 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.

The concentration of iron(II) chloride contaminant in the original groundwater sample is .

Explanation:

Amount of silver chloride recovered = 6.9 mg = 0.0069 g[/tex]

Moles of silver chloride =

According to reaction. 2 moles of silver chloride are obtained from 1 mole of iron(II) chloride.

Then moles of silver chloride will be obtained from:

Moles of iron(II) chloride =

Volume of a sample of ground water = 200 mL = 0.2 L

The concentration of iron(II) chloride contaminant in the original groundwater sample is .

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell