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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) +3AgN)3 (aq) =3AgCl (s) Fe(NO3)3 (aq)
The chemist adds a 59.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 4.3 mg of silver chloride.
calculate the concentration of iron chloride containment in the original groundwater

Respuesta :

cristisp93

Iron (III) chloride (FeCl₃) have a concentration of  5 × 10⁻⁵ M in the contaminated groundwater.

Explanation:

We have the following chemical reaction:

FeCl₃ (aq) +3 AgNO₃ (aq) = 3 AgCl (s) + Fe(NO₃)₃ (aq)

where:

(aq) - aqueous

(s) - solid

number of moles = mass / molar weight

number of moles of AgCl = 4.3 / 143 = 0.03 mmoles

Knowing the chemical reaction we devise the following reasoning:

if           1 mmole of FeCl₃ produces 3 mmoles of AgCl

then    X mmoles of FeCl₃ produces 0.03 mmoles of AgCl

X = (1 × 0.03) / 3 = 0.01 mmoles of FeCl₃

And now we can calculate the molar concentration of iron (III) chloride (FeCl₃) in the groundwater sample:

molar concentration = number of moles / volume

molar concentration of FeCl₃ = 0.01 mmoles / 200 mL

molar concentration of FeCl₃ = 5 × 10⁻⁵ M

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molar concentration

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