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Titration of a cola product.

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Dianna Alford Dr. Lund Inorganic Chemistry 12:00 Lab # 8 LAB 8 I. Purpose: Titration of a cola product. II. Objective: To determine the molar concentration of phosphoric acid in a cola product. III. Background: Titration is an analytical technique used to find the concentration of a known volume of acid by adding a known concentration of base. As these substances react, you look for a "tell-tale" indication that the reaction is complete, which allows us to determine the concentration of the base. This is the most common type of titration known as an acid-base titration. The equivalence point is the most crucial point of the titration. It is the point during the titration where the moles of base added will equal the moles of acid added to the solution. Since the volume of base added can be read from the buret at this point, and the concentration of the base and the volume of the acid are also known, the concentration of the acid solution can be determined. One way to determine the equivalence point is by measuring the pH of the solution as you add base to the acid. ...read more.


1. Pour about 75 mL of cola into a clean, dry 250 mL beaker. 2. To prepare the cola for titration, it must first be decarbonated. Cover the beaker containing the cola with a watch glass and gently boil for about 20 minutes using a hot plate. This will remove the CO2 from the cola, which would interfere with the phosphoric acid titration. 3. Let the cola to cool to room temperature before titrating. 4. Using a pipette, add 25.00 mL of room temperature, decarbonated cola into a clean, double-nested styrofoam cup. 5. Using a 250 mL beaker, obtain about 75 mL of 0.01 M NaOH. Note the exact concentration of the NaOH from the container. 6. To prepare the buret for the titration, it should first be rinsed with distilled water and the rinsed with several small portions of the NaOH solution. To begin the titration, the buret should contain between 40 and 50 mL of NaOH. VII. Data: Trial 1-25 mL of decarbonated Pepsi, 0.01 M NaOH used for the titration, and only 8 mL of NaOH used to the first equivalence point. ...read more.


IX. Conclusions: For the titration of the Pepsi, we came to the conclusion that it had 0.00008 to 0.000085 moles per liter of acid in Pepsi and had a Molarity of 0.0032 to 0.0034 of acid. For the Coke, it had 0.000148 to 0.00016 moles per liter of acid and had a Molarity of 0.00592 to 0.0064 of acid. From this statement, you can see that the Pepsi has more acid (H3PO4) than the Coke product does. Thus the Coke will erode other substances quicker, like the enamel on your teeth, than would Pepsi. As you can tell by the graphs, our calculations may be off a bit. When titrating these substances, we ran the base right underneath the pH probe which made our graphs a little difficult to read. X. Real World Applications: In order for things to stay fresh on the shelves, we can things in highly acidic juices to keep them from spoiling. It takes much longer for things to spoil in such acidic environments. Also, chemists use this type of titration at the Cola plant when making cola products. They are like the ingredients to making cookies. Instead of 3 cups of flour, it calls for 1 cup of H3PO4. ...read more.

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