Experiment: Determined the amount of FeSO4.7H2O per 100 ml of the given solution.You are provided with 0.02M solution of kMnO4. (rai amad ud din)

good method for the determining

1. Represented by: Rai amad ud din Chemical engineening Roll No. 27 Pratical (Fundamental and analytical chemistry ) Sharif college of Engineering and techonolgy Thank you

2. Experiment No. 6 Determined the amount of FeSO 4. 7H 2 O per 100 ml of the given solution.You are provided with 0.02M solution of kMnO 4 .

3. Main points which you have to clear before doing the experiment. How to prepared the 0.02M solution of KMnO 4. Second we have to clear that we can not used indicator in this experiment, WHY?

4. Preparation of 0.02M kMnO 4 solution As a standard,we take 1.0g 0.1M kMnO4 1/0.1g 1M kMnO4 1*0.02/0.1g 0.02M kMnO4 so,we can weight the 0.2g of kMnO4 crystals in a water to prepared the 0.02M solution of kMnO4 .

5. Why indicator is not used? The indicator is not used because KMnO 4 is a strong oxidizing agent.permagnate MnO 4 is an intense dark purple colour. The reduction of per magnate ion to colourless Mn+ ion. As you see the colour of potassium permagnate is intense dark purple colour.

6. CHEMICAL EQUATION 2 KMnO4 + 10FeSO4 +8H 2 SO 4 5Fe 2 (SO 4 ) 3 +k 2 SO 4+ 2MnSO 4 +8H 2 O

7. Indicator and apparatus Apparatus ♥ Fe solution. ♥ solution of KMnO 4 ♥ Buret clamp ♥ 250 ml Erlenmyer Flask ♥ 25 ml Pipet,Ring Stand Indicator KMnO 4 is itself indicator

8. ❶ Take the 250 ml erlemneyer flask.Add 25ml Fe solution,12ml H2SO4 of 6N and ass 50ml distilled water in this flask. ❷Now, fill the burette with 0.02M solution of KMnO4. ❸Set the apparatus as shown in the figure, the erlemeyer flask under the burette. ❹Titrate the flask solution against the KMnO4. ❺Titrate the solution until the solution taken in the flask becomes light pink. ❻Carefully, note the initial reading and note the reading at which the solution becomes light pink.this is the final reading. ❼Repeat, the experiment three times to ensure the correct reading P rocedure

9. Observations and Calculations No. of Obs. Initial readind Final reading Volume used(ml) 1 0.0 6.5 6.5 2 6.5 13.5 7 3 13.5 19.5 7

10. Average volume =7 ml Now,we find the molarity of FeSO4 FeSO4.7H2O KMnO4 M1=? M2=o.o2M V1=87 ml V2=7ml n1=10 n2=2 As, we know that M1V1/n1=M2V2/n2 M1=0.008M

11. Amount of FeSO4 Amount of FeSO4 = Molarity * molar mass =0.008*278 =2.24g/L Amount of FeSO4 in 100ml of the solution =2.224/100m RESULT In this experiment,we can determined the percentage of FeSO4.7H20