Question

20.40g Iron(III) oxalate is dissolved in enough water to give 250.0
ml of solution. 25.00 ml of this solution is pipetted into a
100.0ml volumetric flask and diluted to the mark.

A. Calculate the molarity of Iron(III) oxalate in the original
solution.

B. Calculate the molarity of the oxalate ion in the diluted
solution.

Answer #1

**molarmass of Fe2(C2O4)3 = 375.747 g/mol**

**VOLUME OF SOLUTION = 250 ml = 0.25 L**

**Molarity = w/mwt*1/V in L**

w = 40 grams , Mwt = 375.747 g/mol

**V = 0.25 L**

**Molarity = (40/375.747)*(1/0.25)**

**
= 0.426 M**

**A. the molarity of Iron(III) oxalate in the original
solution. = 0.426 M**

**B . molarity of the oxalate ion in the diluted
solution.**

**M1V1 = M2V2**

**M1 = 0.426 M , V1 = 25 ml**

**M2 =
? v2 =
100 ml**

**M2 = M1V1/V2 = 0.426*25/100 = 0.1065 M**

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