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TITLE: THE AMOUNT OF VITAMI C IN THE FRIT JUICE IN DIFFERENT
CONDITION.
1
ABSTRACT
Vitamin C also known as ascorbic acid, is a water-soluble vitamin needed by the body for
hundreds of vital metabolic reactions. Vitamin C is not produced in the human body, yet it is
essential for the formation of collagen, connective tissue, and immune system factors. This
experiment was conducted by putting each of the same amount of fresh pineapple juice in 5
different conditions for 10 minutes and the amount of vitamin C left was tested by using Iodine
Titration. The percentage of vitamin C loses is calculated and the vitamin C losses the most is
exposed to microwave while stored in refrigerator losses the least.
2
TITLE………………………………………………………………………………….…..1
ABSTRACT………………………………………………………………………………2
CONTENT…………………………………………………………… ………………….3
1.0 INTRODUCTION
1.1 Problem Statement…………………...................................……………………...4
1.2 Objective………........…………………………………………………………….4
1.3 Literature Review
1.3.1 Previous Research………………......……………………...………………5
2.0 METHODOLOGY
2.1 Theory…………………………………………………………………….……...6
2.2 Procedure..........................…………………………………………………….…7
3.0 OBSERVATION, RESULT AND DISCUSSION
3.1 Data Presenation............…………………………………………………………8
3.2 Discussion.....................................……………………………………………….9
4.0 CONCLUSION………………………………………………………………............13
REFERENCES…………………………………………………………………………...14
3
1.0 INTRODUCTION
Vitamin C or ascorbic acid is important to the body for prevention of scurvy. Scurvy is
caused by lack of vitamin C in the body which can affect muscles weakness, swollen and
bleeding of gums, loss of teeth and bleeding under the skin as well as tiredness and
depression. Good sources of vitamin C are fresh fruits and vegetables, especially citrus fruits.
Benefits of vitamin C (ascorbic acid) may include protection against immune system
deficiencies, cardiovascular disease, prenatal health problems, eye disease, and
even skin wrinkling. It also functions as an antioxidant and is necessary for the treatment and
prevention of scurvy. However, Vitamin c is a type of water soluble vitamin.Water-soluble
vitamins are less stable and can be destroyed by microwave, water, heat, air and light
1.1 Problem Statement
Which condition cause the lost of vitamin C content in fresh juices the most and the
least?
1.2 Objective
To determine the amount and percentage of vitamin C losses after exposed to heating,
sun light, refrigerator, normal room condition and microwave.
4
1.3 Literature Review
1.3.1 Previous research
Vitamin C is a potent reducing agent, meaning that it readily donates electrons to
recipient molecules. Related to this oxidation-reduction (redox) potential, two
major functions of vitamin C are as an antioxidant and as an enzyme cofactor [1].
Vitamin C also participates in redox recycling of other important antioxidants; for
example, vitamin C is known to regenerate vitamin E from its oxidized form[2].
And due to vitamin C is so important for mankind, there are a lot of research has
been done by scientist. For example, diseases cause by vitamin C deficiency [3],
different fruits and vegetables vary in their vitamin C content[4], diseases cause
by vitamin C overdose [5] and preservation of vitamin C [6] Vitamin C is very
unstable in aqueous solutions. Tests showed ascorbic acid to be a weak,
monobasic acid and a strong reducing agent.Therefore, it oxidizes and the product
of such oxidation involving the loss of two hydrogens (C6H6O6), was named
dehydroascorbic acid.[7]Besides that, the factors that affecting the vitamin C is
also been discovered. Factor such as UV light that degrade the vitamin C via
wavelength[8], high temperature that decomposes the vitamin C due to increase of
enzymatic destruction[9] and microwave that hit the vitamin C with high energy
wavelength that directly causing the decomposition of the vitamin C.[10]
5
2.0 METHODOLOGY
2.1 Theory
Vitamin C can be determined by acid-base reaction or oxidation-reduction reaction.
Vitamin C is a weak acid and a good reducing agent. Iodine is a weak oxidizing agent, so
that it will not oxidize substances other than the ascorbic acid in the sample of fruit juice.
As a strong reducing agent, vitamin C will reduce I2 to I- very easily. The excess of iodine
react the starch as indicator to perform the amount of vitamin C is finishing in redox
reaction. In this reaction, the ascorbic acid molecule gains oxygen (in the form of -OH
groups). Each iodine atom in the I2 molecule accepts an electron and become a negatively
charge to form iodide ion. Thus that, the ascorbic acid molecule was oxidized and the
iodine molecule was reduced.
C6H8O6 + I2 + 2H2O → C6H10O8 + 2I - + 2H+ …….equation 1
Excess iodine (I2) reacts with iodide ions (I-) to form triiodide ion (I3-) which forms a
very intense blue color when it reacts starch. This colour is due to incorporation of the
ions within the molecular structure of the starch.
I2 + I-→ I3- ………equation 2
To detect the end point, starch must be added at the beginning of the titration in the
conical flask. When all ascorbic acids have finished, the excess of iodine solution will
react the starch to form blue-black colour in the solution.
I3-+ starch → starch (I3
-) complex …….equation 3
6
2.2 Procedure
350ml of fresh fruit juice were squized from the pineapple fruit. 50 ml of fresh fruit juice
A, B, C, D and E by using a measuring cylinder and poured saperately into 5 beakers.The
5 beakers were then placed under 5 different condition in the order of A-Hot water bath,
B-Under the sun, C-Refrigerator, D-Microwave and E-Room temperature for 10 minutes
measured by using stop watches. 1.27 g of iodine and 2.54 g potassium iodide (KI) were
dissolved in 200 ml of distilled water and added with 30 ml of 3 M sulfuric acid. The
solution was poured into a 1000 ml volumetric flask and diluted to a final volume of 1000
ml with distilled water. The solution was transferred to a 600 ml beaker labeled as iodine
solution. 0.50 g soluble starch was added to 50ml near-boiling distilled water and mixed
well and allows cooling before use. 15.00 ml of fresh squeezed pineapple juice standard
solution to a 125 ml conical flask.2 drops of 1% starch solution were added. Burette was
rinsed with a small volume of the iodine solution and then filled it. The initial volume was
recorded. The solution is titrated until the endpoint is reached which is the first sign of
blue color that persists after 20 seconds of swirling the solution is observed. The final
volume of iodine solution was recorded. The experiment is repeated by using fresh fruit
juice A, B, C, D and E .
7
3.0 OBSERVATION, RESULTS AND DISUSSION
3.1 Data presentation
The chemical equation of the reaction:
I2 + C6H8O6 ---> C6H6O6 + 2 H+ + 2 I-
8
Original Titration First Second Average
Final Reading/cm3 7.85 15.60
Initial Reading/ cm3 0.00 7.85
Volume of iodine solution used/ cm3 7.85 7.75 7.80
A Titration First Second Average
Hot Final Reading/ cm3 6.50 12.90
Water Initial Reading/ cm3 0.00 6.50
Bath Volume of iodine solution used/ cm3 6.50 6.40 6.45
B Titration First Second Average
Under Final Reading/ cm3 6.35 12.60
The Initial Reading/ cm3 0.00 6.35
Sun Volume of iodine solution used/ cm3 6.35 6.25 6.30
C Titration First Second Average
Refri- Final Reading/ cm3 7.05 14.20
gerator Initial Reading/ cm3 0.00 7.05
Volume of iodine solution used/ cm3 7.05 7.15 7.10
D Titration First Second Average
Micro- Final Reading/ cm3 6.85 13.60
wave Initial Reading/ cm3 0.00 6.85
Volume of iodine solution used/ cm3 6.85 6.75 6.80
E Titration First Second Average
Room Final Reading/ cm3 5.50 10.90
Tempe- Initial Reading/ cm3 0.00 5.50
rature Volume of iodine solution used/ cm3 5.50 5.40 5.45
Iodine Ascorbic acid (vit C) dehydroascorbic acid hydrogen ioniodide ion
1 mole of I2 react with 1 mole of Ascorbic acid
Number of mole of iodine = 1.27/126.90
used in the iodine solution = 0.01mole
0.01 mole of I2 react with 0.01 mole of Ascorbic acid
Mass of ascorbic acid reacted= mole x molar mass of ascorbic acid
=0.01 x 176.12
= 1.7612g
Concentration of = 0.01mol/1000cm3
iodine solution = 0.01mol/dm-3
Original: 15 cm3 of pineapple juice required 7.80 cm3 of iodine solution to react completely
Mole of ascorbic acid in = MV/1000
15 cm3 of pineapple juice = 0.01x 7.80/1000
= 7.80 x 10-5mol
Concentration of ascorbic acid in = 7.80 x 10-5mol x 1000/15
pineapple juice = 5.20 x 10-3mol/dm-3
Condition A: 15 cm3 of pineapple juice required 6.45 cm3 of iodine solution to react completely
Mole of ascorbic acid in = MV/1000
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15 cm3 of pineapple juice = 0.01x 6.45/1000
= 6.45 x 10-5mol
Concentration of ascorbic acid in = 6.45 x 10-5mol x 1000/15
pineapple juice = 4.30 x 10-3mol/dm-3
Condition B: 15 cm3 of pineapple juice required 6.30 cm3 of iodine solution to react completely
Mole of ascorbic acid in = MV/1000
15 cm3 of pineapple juice = 0.01x 6.30/1000
= 6.30 x 10-5mol
Concentration of ascorbic acid in = 6.30 x 10-5mol x 1000/15
pineapple juice = 4.20 x 10-3mol/dm-3
Condition C: 15 cm3 of pineapple juice required 7.10 cm3 of iodine solution to react completely
Mole of ascorbic acid in = MV/1000
15 cm3 of pineapple juice = 0.01x 7.10/1000
= 7.10 x 10-5mol
Concentration of ascorbic acid in = 7.10 x 10-5mol x 1000/15
pineapple juice = 4.73 x 10-3mol/dm-3
Condition D: 15 cm3 of pineapple juice required 6.80cm3 of iodine solution to react completely
Mole of ascorbic acid in = MV/1000
15 cm3 of pineapple juice = 0.01x 6.80/1000
= 6.80 x 10-5mol
Concentration of ascorbic acid in = 6.80 x 10-5mol x 1000/15
pineapple juice = 4.53 x 10-3mol/dm-3
10
Condition E: 15 cm3 of pineapple juice required 5.45 cm3 of iodine solution to react completely
Mole of ascorbic acid in = MV/1000
15 cm3 of pineapple juice = 0.01x 5.45/1000
= 5.45 x 10-5mol
Concentration of ascorbic acid in = 5.45 x 10-5mol x 1000/15
pineapple juice = 3.63 x 10-3mol/dm-3
Condition Concentration of ascorbic acid (moldm-3)
Original 5.20 x 10-3
Hot Water Bath 4.30 x 10-3
Under The Sun 4.20 x 10-3
Refrigerator 4.73 x 10-3
Microwave 4.53 x 10-3
Room Temperature 3.63 x 10-3
Table above shows the concentration of the ascorbic acid at different conditions.
The original pineapple juice (Initial) is the fresh juice of the same pineapple without go thought
any condition. Thus, the concentration of the ascorbic acid in the original pineapple juice is
assumed to be 100%.
11
The formula:
[(Initial concentration – Final concentration)/Initial concentration] x 100%
is used to determine the percentage of vitamin C loss in the 5 condition after 10 minutes.
The pineapple juice in A is placed in hot water bath and the Vitamin C loss after 10 minutes is
[(5.20x10-3- 4.30x10-3)/ 5.20x10-3 ] x 100% = 17.31%.
The pineapple juice in B is placed under the sun and the Vitamin C loss after 10 minutes is
[(5.20x10-3- 4.20x10-3)/ 5.20x10-3 ] x 100% = 19.23%.
The pineapple juice in C is placed in refrigerator and the Vitamin C loss after 10 minutes is
[(5.20x10-3- 4.73x10-3)/ 5.20x10-3 ] x 100% = 9.04%.
The pineapple juice in D is placed in microwave and the Vitamin C loss after 10 minutes is
[(5.20x10-3- 4.53x10-3)/ 5.20x10-3 ] x 100% = 12.88%.
The pineapple juice in E is placed at room temperature and the Vitamin C loss after 10 minutes is
[(5.20x10-3- 3.63x10-3)/ 5.20x10-3 ] x 100% = 30.19%.
The table above shows the percentage of vitamin C loss in 5 different conditions.
4.0..CONCLUSION
The effect of cold, heat, oxygen, UV light and microwave on vitamin C is significant .The loss of
vitamin C is arranged in ascending order :
12
Condition Percentage of Vitamin C loss (%)
Hot Water Bath 17.31
Under The Sun 19.23
Refrigerator 9.04
Microwave 12.88
Room Temperature 30.19
Refrigerator > Microwave > Hot Water Bath > Under The Sun > Room Temperature.
The vitamin C in pineapple juice which placed in refrigerator losses the least and the vitamin C
in pineapple juice which placed at room temperature losses the most. The vitamin C in pineapple
juice which treated with hot water bath can also shows the effect of vitamin C losses during
cooking process. The vitamin C in pineapple juice shows that placing the fruit juice under the hot
sun will lead to a great loss of vitamin C. The best way to preserve the vitamin C in the fruit
juice is keep it in an airtight container to prevent oxidation by the air in surrounding and store in
a cold condition to reduce the reactivity vitamin C. Lastly, my recommendation for future study
is to study the effect on enzyme present in the organism to the vitamin C in the organism.
REFERENCE
1. Combs J, Gerald F. The Vitamins. 4 ed. Burlington: Elsevier Science; 2012.
2. Bruno RS, Leonard SW, Free Radic Biol Med. 2006;40(4):689-697.
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3. Sauberlich, HE. A history of scurvy and vitamin C. New York: Marcel Decker Inc. 1997:
pages 1-24 USDA National Nutrient Database for Standard Reference, Release 22. 2009.
4. Sargeant LA, Wareham NJ Diabetes Care. 2000;23(6)
5. Gregory JF, 3rd. Ascorbic acid bioavailability in foods and supplements. Nutr Rev.
1993;51(10):301-303.
6. Burdurlu, Hande S.; Koca, Nuray and Karadeniz, Feryal. (2006): Degradation of Vitamin
C in Citrus
7. Juice Concentrates during Storage, Found in Journal of Food Engineering, volume 74,
Issue 2, May 2006 (p. 211–216)
8. boul-Enein HY, Al-Duraibi IA, Stefan RI, Radoi C, Avramescu A (1999). "Analysis of
L- and D-ascorbic acid in fruits and fruit drinks by HPLC". Seminars in Food
Analysis 4 (1): 31–37. Archived from the original on December 15, 2013
9. Galiano Ramos, Álvaro, VITAMINA C, IQB: MEDCICLOPEDIA, (in Spanish) Web, 03
Jan, 2012. <http://www.iqb.es/nutricion/vitaminac/vitaminac.htm>.
10. Levine M, Dhariwal KR, Washko P, Welch R, Wang YH, Cantilena CC, Yu R (1992).
"Ascorbic acid and reaction kinetics in situ: a new approach to vitamin requirements". J.
Nutr. Sci. Vitaminol. Spec No: 169–72
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