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Sonja [21]
3 years ago
11

Iron in the 2 oxidation state reacts with potassium dichromate to produce Fe3 and Cr3 according to the equation: 6 Fe2 (aq) Cr2O

72-(aq) 14 H (aq) <----> 6 Fe3 (aq) 2 Cr3 (aq) 7 H2O(l) How many milliliters of 0.2937 M K2Cr2O7 are required to titrate 132.0 mL of 0.1782 M Fe2 solution
Chemistry
1 answer:
allsm [11]3 years ago
6 0

Given :

Volume of Fe^{2+} , V = 132 mL .

Molarity of Fe^{2+}, M = 0.1782 M .

To Find :

How many milliliters of 0.2937 M K_2Cr_2O_7 are required to titrate 132.0 mL of 0.1782 M Fe^{2+} solution .

Solution :

Moles of  Fe_2 :

n=0.1782\times \dfrac{132}{1000}\ mol\\\\n=0.264\ mol

Now , 1 mole of K_2Cr_2O_7 reacts with 6 mole of Fe^{2+} .

So , moles of K_2Cr_2O_7 required is :

N=\dfrac{0.264}{6}=0.044\ mol

Volume required is :

V=\dfrac{N}{M}\\\\V=\dfrac{0.044}{0.2937}\ L\\\\V=0.15\ L=150\ mL

Hence , this is the required solution .

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