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Estimation of Ferrous Sulphate - Volumetric Analysis | Chemistry Practical Laboratory Experiment | Study Material, Lecturing Notes, Assignment, Reference, Wiki description explanation, brief detail |

Chapter: 12th Chemistry : Practicals

Estimation of Ferrous Sulphate

To estimate the amount of ferrous sulphate dissolved in 750 ml of the given unknown solution volumetrically.

VOLUMETRIC ANALYSIS


Estimation of Ferrous Sulphate (Fe2+)

 

Aim :

To estimate the amount of ferrous sulphate dissolved in 750 ml of the given unknown solution volumetrically. For this you are given with a standard solution of ferrous ammonium sulphate (FAS) of normality 0.1102 N and potassium permanganate solution as link solution.

 

Principle:

During these titrations, Fe2+ ions (from ferrous salts) are oxidised to MnO4- ions and MnO4- ion (from Mn2+) is reduced to Mn2+ ion.

Oxidation   :        5 Fe2+          5 Fe3+ + 5e

Reduction   : 

Overall reaction:

5Fe2+ + MnO4- + 8H 5Fe3+ + Mn2+ + 4H2O

Short procedure :


 

Procedure :

Titration–I

(Link KMnO4)Vs (Standard FAS)

Burette is washed with water, rinsed with KMnO4 solution and filled with same KMnO4 solution up to the zero mark. Exactly 20 ml of standard FAS solution is pipetted out into the clean, washed conical flask. To this FAS solution, approximately 20ml of 2N sulphuric acid is added. This mixture is titrated against KMnO4 Link solution from the burette. KMnO 4 is added drop wise till the appearance of permanent pale pink colour. Burette reading is noted, and the same procedure is repeated to get concordant values.

Titration –I

(Link KMnO4 )Vs (Standard FAS)


 

Calculation :

Volume of KMnO4 (link) solution (V1) = ----------ml

Normality KMnO4 (link) solution (N1) =-----------N

Volume of standard FAS solution (V2) = 20 ml

Normality of standard FAS solution (N2) = 0.1102 N

According to normality equation: V1× N1 = V2 × N2

N1 = V2 × N2 /  V1


Normality of KMnO4 (link) solution (N1) = ----------------- X N

Titration–II

(Unknown FeSO4 ) Vs (Link KMnO4)

Burette is washed with water, rinsed with KMnO4 solution and filled with same KMnO4 solution up to the zero mark. Exactly 20 ml of unknown FeSO4 solution is pipetted out into the clean, washed conical flask. To this FeSO4 solution approximately 20ml of 2N sulphuric acid is added. This mixture is titrated against KMnO4 Link solution from the burette. KMnO4 is added drop wise till the appearance of permanent pale pink colour. Burette reading is noted and the same procedure is repeated to get concordant values.

Titration –II

(Link FeSO4 )Vs (Unknown FeSO4 solution)


Calculation :

Volume of Unknown FeSO4  solution V1 = 20 ml

Normality of Unknown FeSO4 solution N1 = ? N

Volume of KMnO4 (link) solution V2 = ml

Normality KMnO4  (link) solution N2 = X N

According to normality equation: V1× N1 = V2 × N2

 N1 = V2 × N2  / V1


N1= --------Y--------- N

The normality of unknown FeSO4  solution = ________________ N

Weight calculation:

The amount of FeSO4 dissolved in 1 lit of the solution = (Normality) x (equivalent weight)

The amount of FeSO4 dissolved in 750 ml of the solution  = Normality x equivalentweight x 750 / 1000



Report :

The amount of FeSO4 dissolved in 750 ml of the solution  =  ---g

 

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