Finding the Molarity of the Reactant

[derwalrus]

Homework Statement

96 grams of Iron(III)Chloride is dissolved in water to give 300ml of solution. What is the Molarity of Iron(III)Chloride? What is the Molarity of just the Chloride?

Homework Equations

FeCl₃ + H₂O → Fe⁺³ + 3Cl^-

The Attempt at a Solution

96g FeCl₃ X (1 mol FeCl₃ / 162.2g FeCl₃) = .59 mol FeCl₃

Then I found the molarity of the solution.
.59 mol FeCl₃ / .3L solution ≈ 2M solution.

I'm just confused as to where I go from here to find the molarity of the FeCl₃ and then the Cl. Any help would be much appreciated, thanks!

Edit: Did some more tinkering.

.59 mol FeCl₃ X (3 mol Cl^- / 1 mol FeCl₃) = 1.77 mol Cl^-

M Cl^-= 1.77 mol Cl^- / .300 L
M Cl^- = 5.9M

 

[Infinitum]

Your working is correct

 

[Borek]

There is one small problem. Iron(III) chloride as a solid is usually present in the form of hexahydrate. Not knowing the context in which the question was asked it is hard to say if your molar mass is right or not.