estimation of vitamin c cbse 12 project 2017

Introduction Vitamin C also called ascorbic acid, is an essential nutrient for humans and other animals Vitamin C is needed by the body to form collagen. body also uses vitamin C to make skin, tendons, ligaments and blood vessels. It also uses this vitamin to repair and maintain cartilage, bones and teeth, to heal wounds and to form scar tissue. A person needs at least 40mg vitamin C daily. The lack of vitamin C in the body can cause weak immunity, and even scurvy.

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Thus ,It is important to know how much vitamin C is in the food we eat.

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I would like to express my special thanks of gratitude to my teacher MR Sunderash sir as well as our lab assistant Mrs. Fatima who gave me the golden opportunity to do this wonderful project on the topic (Write the topic name), which also helped me in doing a lot of Research and i came to know about so many new things I am really thankful to them. Secondly i would also like to thank my parents and friends who helped me a lot in finalizing this project within the limited time frame.

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Aim

To determine the amount of vitamin-c (absorbic acid) present in different fruitjuices by titration with iodin solution and compare its value with the mentioned values on on their bottle lables

Theory  It's well known that Iodine reacts with many substances as it is very powerful oxidant. In the mixture of many different substances it first reacts with molecules that easier to break down.  Vitamin C is anti-oxidant and will react with Iodine promptly. If we mix vitamin C and starch and will gradually add iodine into this mixture, iodine will only react with vitamin C, ignoring starch  When mixture ran out of vitamin C Iodine will react with starch. This reaction has very distinctive dark blue color output. As soon as all the vitamin C reacts with iodine next drop of iodine will react with starch and turn the mixture into dark blue.

 Thus we can find out the exact amount of iodine needed to react with vitamin C. Knowing that we can calculate amount of vitamin C in the mixture.

Formula used Amount of vit.c : vol. of iodine used for juice mg/ml samples

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Absorbic value

Titration process at the beginning and almost the end

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Materials required

Measuring cylinder Titration cylinder Beaker Burette Burner Matchbox Titration box Iodine solution Starch solution Vitamin c solution 3 fruit juices

 Preperations Take a one liter beaker and fill it up with 500 ml of water. Crush one (500mg) or two (250 mg) tablet of vitamin C and put it in the jar, stir it well, until vitamin C tablet dissolves. This way you'll get 1 mg/ml solution of vitamin C. Measure 20 ml of that solution, bring it to another glass and add about half glass of water. This glass will contain 20 mg of vitamin C. Starch solution Starch indicator solution: (0.5%). Weigh 0.25 g of soluble starch and add it to 50 mL of near boiling water

in a 100 mL conical flask. Stir to dissolve and cool before using.

Procedure 20 ml of the prepared vitamin c solution is measured using a measuring cylinder and taken on a conical falsk,2 ml of prepared starch solution is added to this 2 well cleaned burette is rinsed with iodine and is filled withit The experimentation set up is made with burette and conical flask in a stand The iodine solution is slowly run into he conical flask,and it is shaken and rotated slowly The endpoint of the titration is identified as the first permanent trace of a dark blue-black colour due to the starch-iodine complex. At this stage burette reading is noted as final burette reading .yhis value indicates

the amount of iodine solution needed to react with 20mg of vitamin c 

Titration of fruit juices 

20 ml of the prepared vitamin c solution is measured using a measuring cylinder and taken on a conical falsk,2 ml of prepared starch solution is added to this 2 well cleaned burette is rinsed with iodine and is filled withit The experimentation set up is made with burette and conical flask in a stand The iodine solution is slowly run into he conical flask,and it is shaken and rotated slowly The endpoint of the titration is identified as the first permanent trace of a dark blue-black colour due to the starch-iodine complex. At this stage burette reading is noted as final burette reading .yhis value indicates the amount of iodine solution needed to react with 20mg of vitamin c

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Calulations For titration 

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