Joanna Park Mrs. Carrillo CP chemistry
5 September 17, 2012
i. Beverage Density Lab Report
ii. Purpose: The purpose of this experiment is to determine the percentage of sugar content in beverages.
iii. Materials: Distilled water, beverages (juice, soda, sport drinks), Sugar reference solutions (0, 5, 15, ad 20%) 25ml each, Balance, centigram(0. 01g precision), Beaker (100-mL), Erlenmeyer flask (125-mL to collect rinse solutions), Pipet(10-mL), Pipet bulb or pipet filler
iv. Procedure: Part A
1. Place an empty 100-mL beaker on the balance and hit the “rezero” button and check if the scale reads 0. 00 g
2. Suck up 10. 00mL of 0% sugar (distilled water) into a pipet and move the liquid to an empty beaker.
3. In data table A record the mass of 0% sugar water sample.
4. Make sure you rezero the balance using the ‘’rezero” button
5. Clean out ant residual solution in the pipet by gently blotting the tip with a paper towel.
6. For the other four sugars reference solutions repeat steps 2-5; start in order from the least concentrated to the most concentrated
- Before using the pipet to move the new solution to a beaker, rinse the pipet once with each new solution.
- Drain the rinse solutions into an Erlenmeyer flask. Don’t forget to rezero the balance prior to each new mass measurement.
7. Calculate the density and record the value in Data Table one Part B
8. Use the procedure in part A to determine the density of two beverages. Record all mass and volume data in Data table B and use clean glassware. Between successive beverage measurements rinse the pipet with the second beverage.
v. Pre-Lab Questions
1. If the following mass and volume data are used to calculate the density of solution, how many significant figures are allowed in the calculated density? Mass of solution = 12. 53g; volume of solution = 8. 27mL. 12. 53= 4 sig figs 8. 27= 3 sig figs In the calculated density, three significant figures are allowed
2. Calculate the density of the solution described in Question #1. * 12. 53g/8. 27mL = 1. 52g/mL Density= 1. 52g/mL The density of the solution in question #1 is 1. 52 g/mL
3. According to its nutrition label, orange soda contains 49g of sugar per 3550mL serving. If the density of the beverage is 1. 043 g/mL, what is the percentage sugar concentration in orange soda?
* X g= 355mL(1. 043g/1mL) = 370g, 49g/370g
* 100%= 13%
The percent sugar concentration in the orange soda is 13%
vi. Data Table
Table A. Solution| Mass, g| Sample Volume, mL| Density, g/mL| 0% Sugar| 10. 00 g| 10. 00| 1. 00 g/mL| 5% Sugar| 10. 10 g| 10. 00| 1. 01 g/mL| 10% Sugar| 10. 30 g| 10. 00| 1. 03 g/mL| 15% Sugar| 10. 60 g| 10. 00| 1. 06 g/mL| 20% Sugar| 10. 80 g| 10. 00| 1. 08 g/mL| Table B Beverage| Mass, g| Sample Volume, mL| Density g/mL| Powerade| 10. 27 g| 10. 00 mL| 1. 027 g/mL| Cola| 10. 38g| 10. 00 mL| 1. 038 g/mL|
vii. Results Table
Beverage| Measured density| Percent sugar(from graph)| Amount of sugar ()| Percent sugar| Percent error| Powerade| 1. 27g /mL| 8. 3%| 15g /240| 6. 1%| 22%| Cola| 1. 038g /mL| 11. 1%| 42g /355| 11%| 0. 9%|
2. Use the graph to estimate the unknown sugar concentration in the first beverage. To do this, locate the point on the y-axis that corresponds to the density value of the beverage. Follow that point on the the y-axis across horizontally to where it meets the “best-fit” line through this data. Now read down vertically from this point where this vertical “line” meets the x-axis equals this percent concentration of sugar in the beverage solution. Construct a Results table and record the density of the beverage and the estimated percent sugar concentration. Powerade has the sugar concentration of 10. 27%
3. Repeat step 2 to determine the percent sugar concentration if the second beverage. Record all information in your results table. Cola has the sugar concentration of 11. 1%
4. Calculate the actual or accepted value of the sugar concentration in weight percent for each beverage using the nutrition label information and the measured density value. Hint: See Pre-Lab Questions #3 for how to do this calculation. Record both the nutrition label information and the actual percent sugar concentration in your results table. Answer: Cola X g= 355mL (1. 038g/1mL) = 388g (42g / 368g) x 100% = 11% Cola’s actual sugar concentration is 11% Powerade X g= 240mL (1. 027g / 1mL)= 246mL (15/240) x 100% = 6. 25% Powerade’s actual sugar concentration is 6. 25%
5. Use the following equation to calculate the percent error in your experimental determination of the sugar content I each beverage. Enter the percent error in the results table. Powerade % Error = l 8. 3 – 6. 1 / 8. l * 100% = 22% The percent error for Powerade is 22% Cola % Error = l 11. 1 – 11 / 11. 1l * 100 = 0. 9% The percent error for Cola is 0. 9%
6. What was your measured density for pure water (0% sugar solution)? The density of water is usually quoted as 1. 00 g/mL, but this precise value is for 4? C. Comment on why your measured density might be higher or lower than 1. 00 g/mL. The measured density for pure water I got 1. 00g/ mL, because my water was exactly 4? C.
7. This lab looks at the relationship between the density of a beverage and its sugar content. What assumption is made concerning the other ingredients in the beverage and their effect on the density of the solution? Do you think this is a valid assumption? Explain. Despite this lab looks just at the relationship between the density of a beverage and its sugar content, other ingredients are also shown in the solution, like sodium. These other ingredients throw off the estimated percentage since they make the solution denser.
8. When plotting the data such as that obtained in this experiment, why is it not appropriate to “connect the dots”?
If you were to repeat the lab, do you think you would get the exact same result? Comment of the sources of error in this experiment and their likely effect on the results.
1) It is not appropriate to “connect the dots” when you plot the data such as that in this experiment. It is because the measurements are imperfect. This means that the dots are not in a straight line, but a best fit lie helps approximate reality by using a straight line.
2) The results would not be exact, if I were doing the lab again. It probably would be more accurate, since I know the where I made errors.
I would also consider about the unconsidered ingredients like sodium to get a more accurate result. ix. Conclusion Through the Beverage Density Lab, I learned that the density of any material is determined by measuring its mass and volume and then dividing the mass by the volume. The mass of a substance can be measured directly using a balance for accuracy. I also learned how unconsidered ingredients, cleaning lab materials are a crucial part of the lab that can affect the results of the experiments. Now I know how to reduce my errors and get a more accurate result.