4. If the vitamin C tablet says that it contains 1000 mg of vitamin C, how much iodine solution would be needed? What is the percent DV for that tablet?
4. If the vitamin C tablet says that it contains 1000 mg of vitamin C, how...
3. A vitamin tablet contains 20 mg of Fe. Calculate the molarity of Fe if the vitamin tablet is dissolved and the solution is diluted to a volume of 100 mL. Would this solution (after being reduced and complexed with o-Phen) be suitable for spectrophotometric analysis?
A niacin vitamin tablet specifies that each tablet contains 100 mg nicotinic acid. A student looking for extra credit in general chemistry lab asks the instructor if it is OK if the vitamin tablet is titrated to determine if the amount the manufacturer claims to be there is correct. Two tablets are crushed and combined, and together weigh 0.3813 g, and require 18.80 mL of 0.1000 M NaOH to titrate to the equivalence point. The ingredients list on the bottle...
. Student dissolves a tablet of Vitamin C in 100.0 mL of water. 2. Using 5.00 mL volumetric pipet, student transfers 5.00 mL of the tablet solution in to an Erlenmeyer flask. 3. After adding starch indicator, student titrated Vitamin C containing solution with standard solution of Iodine (5.00E-3 M). It took 17.73 mL of Iodine solution. MM of vitamin c = 176.1 g/mol Calculate mass of Vitamin C in the tablet.
LABORATORY 10 DETERMINATION OF VITAMIN C CONCENTRATION 3. How many grams of (pure) vitamin C is contained in your unknown stock solution (Part A)? Hint: The solution is made in a 1-L bottle. 4. Consider the following titration: If 21.35 mL of 0.005 M iodine solution is needed to titrate a solution of commercial vitamin C tablet (500 mg) pre- pared in a 100-mL volumetric flask, then what is the mass (%) of vitamin C in the commercial tablet? 5....
Calculate the weight percent of ascorbic acid in a tablet of Vitamin C from the following data: A 100 mg sample of a crushed Vitamin C tablet was dissolved in 40 mL of H2SO4 and 20 mL of water. Two grams of KI and 35 mL of 0.0107 M KIO3 solution was added, and the mixture titrated to a starch endpoint. The titration required 12 mL of 0.0790 M thiosulfate solution.
A multi vitamin supplement contains 200 mg of vitamin C. How many mL of 0.01 M KIO3 solution is required to reach the stioichiometric point? Please provide a detailed explanation.
Question 6 Student dissolves a tablet of Vitamin C in 100.0 mL of water. Student transfers 2.00 mL of the tablet solution into an Erlenmeyer flask After adding starch indicator, student titrated Vitamin C containing solution with standard solution of lodine (5.00E 3 Ml. It took 17.73 ml of iodine solution MM of vitamin c 176.1 g/mol. Calculate mass of Vitamin C in the tablet. A 0.0155 g 8.0.7808 OC 0.3903 0.560
How many molecules of ascorbic acid (vitamin C, C6H8O6) are in a 5.00×102 mg tablet? It states the correct answer shouldn't need be written in scientific notation
A 100 mg vitamin C tablet weighed 1.573 g. A student crushed the tablet and transferred 0.117 g of the crushed powder into a 100 mL volumetric flask, dissolved the powder in ~30 mL DI water, then filled the flask to the calibration line with DI water and mixed well to create Solution 1. The student then transferred 22.1 mL of Solution 1 into a 100 mL volumetric flask and diluted to the calibration line with DI water to create...
please can you answer questions part one Vitamin C can be measured using a technique called titration. Because vitamin C is easily oxidized, we can use this chemical reactivity to detect it in solution. If we react vitamin C with iodine, the vitamin C is oxidized and the iodine is reduced. Iodine (12 molecules) form a purple complex with starch in solution, but reduced iodine, iodide, (I-) is colorless in the presence of starch. CH,OH CH,OH о о снон Η...