Kate+Mauschbaugh+&+Kylie+Ashton


 * Title:** Measuring the Concentration of Asorbic Acid in Orange Juice

Which orange juice contains the most asorbic acid? Until you make a connection between Vitamin C and Ascorbic Acid, use the same term. Appears to be no connection between your title and problem. Ms. Miller
 * Problem:**

Vitamin C is essential to life functions. Vitamin C is a carbon-based compound that performs two main functions in the body. First, it absorbs iron which is necessary to transport oxygen through the blood stream. Second, it has the ability to manage collagen. Also, Vitamin C helps the maintenance of capillaries and helps fight off diseases. We are aware that vitamin C is an important vitamin to contain daily. Vitamin C boosts the immune system and protects against cardiovascular diseases. This will help people because it it important to keep healthy and if they are aware of this people are more likely to choose the better choice of orange juice with the most vitamin C. We are interested in finding out which brand of orange juice contains the largest amount of vitamin C. We will observe a variety of types of orange juice in our experiment. These will include frozen, homemade, with pulp, and without pulp orange juices. The amount of vitamin c will be compared between the orange juices. To do this project, titration will be used. " Titration is a way to measure the unknown amount of a chemical in a solution (the titrant) by adding a measured amount of a chemical with a known concentration (the titrating solution)" (2). Vitamin C, or ascorbic acid, and iodine are combined during titration to make a chemical reaction. “Chemists call this type of reaction an oxidation/reduction reaction. The ascorbic acid is oxidized to dehydroascorbic acid, and the iodine is reduced to iodide ions. The molecule that loses electrons is oxidized, and the molecule that accepts the electrons is reduced”(2 ). Start with a known concentration of iodine, measure the amount of the iodine solution, and then calculate ascorbic acid present. “You add an indicator to the solution. In this case, the indicator is soluble starch. When iodine reacts with starch, it turns the solution a blue-black color. If ascorbic acid is present in the solution, iodine will react with it, and not with the starch, so the solution will not change color”(2).
 * Background:**

**Hypothesis**: If homemade orange juice is titrated, then it will contain the most vitamin C. observed?? Ms. Miller

Independent: type of orange juice Dependent: amount of vitamin C Quantitative: amount of vitamin C Qualitative: taste or color
 * Variables: **

Total cost:$185.95
 * Materials: **
 * Juicer for extracting juice from oranges-$17.78
 * Masking tape-$6.92
 * Cheesecloth-$8.42
 * Permanent marker-$1.89
 * Vitamin C tablets; 250-mg-$9.44
 * Goggles-$30.60
 * Lugol's iodine solution (2%); 30g-$10.95
 * Soluble starch; 30g-$16.35
 * Small funnel-$9.35
 * Graduated cylinder; 50mL-$22.40
 * Graduated cylinder; 500mL-$51.85
 * Knife-
 * 4 oranges-
 * Tropicana orange juice with pulp-
 * Tropicana orange juice without pulp-
 * Tropicana orange juice frozen-
 * Plastic pitcher-
 * 8 Cups-
 * 4 Bowls-


 * Methods:**
 * 1) Wear gloves, chemical safety goggles, and a lab coat or apron when using the iodine solutions in this experiment.
 * 2) Dilute the Lugol's solution 1:10 in distilled water to make your iodine titration solution.
 * 3) Pour the 30 mL Lugol's solution into the 500 mL graduated cylinder.
 * 4) Add enough distilled water to bring the total fluid volume to 300 mL and mix.
 * 5) Store the solution in a clean, tightly covered glass jar that is clearly labeled. Store it in a location that is protected from light.
 * 6) Rinse and dry the 500 mL graduated cylinder.


 * 1) Make a starch indicator solution.
 * 2) This can be anywhere from 0.5 to 1.0%. The exact amount of starch is not critical.
 * 3) For a 0.5% solution, add 1 g (which is equivalent to 1/4 teaspoon) of soluble starch to 200 mL of near-boiling distilled water.
 * 4) Stir to dissolve, and allow to cool.
 * 5) When cool, store the starch solution in a clean, tightly covered glass jar that is clearly labeled.
 * 6) Rinse and dry the 500 mL graduated cylinder.


 * 1) Make a fresh vitamin C standard solution (1 mg/mL). Do this on each day that you make vitamin C measurements from orange juice.
 * 2) You will use this solution to "standardize" your iodine titration solution. You will measure how much of your iodine solution it takes to oxidize a known amount of vitamin C. You can then use your iodine titration solution to determine the amount of vitamin C from test samples of juice from oranges.
 * 3) Crush a 250 mg vitamin C tablet, and dissolve it in 100 mL of distilled water.
 * 4) Pour into a graduated cylinder and add distilled water to bring the total volume to 250 mL.


 * 1) Titrate 25 mL of vitamin C standard solution.
 * 2) Use a clean 50 mL graduated cylinder to measure 20 mL of vitamin C standard solution.
 * 3) Pour this into a 50 mL Ehrlenmeyer flask (the shape of this flask allows you to swirl the solution to mix it without spilling).
 * 4) Add 10 drops of starch indicator solution.
 * 5) Set up the 50 mL buret on the the ringstand.
 * 6) Use a funnel to carefully fill the buret with your iodine titration solution. Tip: the fluid level should not be past the graduated markings on the buret.
 * 7) Write down the initial volume of the iodine titration solution in the buret.
 * 8) Place the Ehrlenmeyer flask (containing the vitamin C and starch solutions) under the buret.
 * 9) Carefully release the spring clamp of the buret to add iodine solution drop by drop.
 * 10) Swirl the flask to mix in the iodine solution after each addition.
 * 11) The titration is complete when the iodine creates a blue-back color in the solution that lasts for longer than 20 seconds.
 * 12) Record the final volume of the iodine solution in the buret.
 * 13) The difference between the initial volume and the final volume is the amount of iodine titration solution needed to oxidize the vitamin C.
 * 14) Repeat this step three times. You should get results that agree within about 0.1 mL.


 * 1) Here's how to prepare fresh-squeezed orange for testing.
 * 2) Use a juicer to squeeze orange juice from two (or more) oranges.
 * 3) You need 20 mL of juice per titration, and you should do at least three titrations per storage condition, for a total of 60 mL.
 * 4) Filter the orange juice through cheesecloth to remove any pulp and seeds.


 * 1) Titrating an orange juice sample is quite similar to titrating the vitamin C standard. Here are the steps:
 * 2) Tip: if any of the orange juice samples contain pulp, filter them through clean cheesecloth before doing the titration.
 * 3) Use a clean 50 mL graduated cylinder to measure 20 mL of the fresh-squeezed juice.
 * 4) Pour this into a 50 mL Ehrlenmeyer flask (the shape of this flask allows you to swirl the solution to mix it without spilling).
 * 5) Add 10 drops of starch indicator solution.
 * 6) Set up the 50 mL buret on the the ringstand.
 * 7) Fill the buret nearly full with your iodine titration solution.
 * 8) Write down the initial volume of the iodine titration solution in the buret.
 * 9) Place the Ehrlenmeyer flask (containing the vitamin C and starch solutions) under the buret.
 * 10) Carefully release the spring clamp of the buret to add iodine solution drop by drop.
 * 11) Swirl the flask to mix in the iodine solution after each addition.
 * 12) The titration is complete when the iodine creates a distinct color change in the juice/starch solution. This color change will be harder to see than with the vitamin C solution, since the juice starts out orange. The color will change from orange to grayish brown when the endpoint is reached. If you continue to add iodine, the color will darken further. You want to note the volume of iodine added when the color //first// changes.
 * 13) Record the final volume of the iodine solution in the buret.
 * 14) The difference between the initial volume and the final volume is the amount of iodine titration solution needed to oxidize the vitamin C.
 * 15) Repeat this step three times. You should get results that agree within about 0.1 mL.

>> **X=** **(6.8 mg/ml)*(20 mg)/(8.5ml):** ** 16.0 mg **
 * 1) For each juice (fresh, premium, or from-concentrate), calculate the average amount of iodine needed to titrate a 20 mL sample.
 * 2) You can calculate the amount vitamin C in your samples by setting up a proportion. Here's an example (with made-up numbers) to show you how:
 * 3) Let's say that it took an average of 8.5 mL of iodine solution to titrate 20 mL of 1 mg/mL vitamin C standard solution, which means 20 mg vitamin C total.
 * 4) Let's also say it takes an average of 6.8 mL of iodine solution to titrate a 20 mL test sample of orange juice.
 * 5) We'll call the amount of vitamin C in the orange juice sample //x//. You can find what //x// is with the following equation:

Methods Sources:

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<span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;"> "Which Orange Juice Has the Most Vitamin C?" Which Orange Juice Has the Most Vitamin C? N.p., n.d. Web. 22 Oct. 2013. < [|__http://www.sciencebuddies.org/science-fair-projects/project_ideas/Chem_p044.shtml__] <span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;">>. ======

Overall Sources:

<span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;">1. "Vitamin C." World of Scientific Discovery. Gale, 2007. Student Resources In Context. Web. 22 Oct. 2013 < [|__http://ic.galegroup.com/ic/suic/ReferenceDetailsPage/ReferenceDetailsWindow?failOverType=&query=&prodId=SUIC&windowstate=normal&contentModules=&mode=view&displayGroupName=Reference&limiter=&currPage=&disableHighlighting=false&displayGroups=&sortBy=&source=&search_within_results=&action=e&catId=&activityType=&scanId=&documentId=GALE%7CCV1648500636__] <span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;">>.

<span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;">2. "Vitamin C." World of Sports Science. Ed. K. Lee Lerner and Brenda Wilmoth Lerner. Vol. 2. Detroit: Gale, 2007. 755-756. Gale Virtual Reference Library. Web. 22 Oct. 2013. [|__http://go.galegroup.com/ps/i.do?id=GALE%7CCX3451100567&v=2.1&u=washington_chs&it=r&p=GVRL&sw=w&asid=23370e178551bf18a65b982e4e5bb5a8__]

<span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;">3. "Which Orange Juice Has the Most Vitamin C?" Which Orange Juice Has the Most Vitamin C? N.p., n.d. Web. 22 Oct. 2013. < [|__http://www.sciencebuddies.org/science-fair-projects/project_ideas/Chem_p044.shtml__] <span style="background-color: #ffffff; color: #333333; font-family: 'Times New Roman'; font-size: 19px; vertical-align: baseline;">>.