a) 4.71 mg
we dissolve 0.0471 g (47.1 mg) vitamin C in water to form 100 ml solution.
(since, 1 g = 1000 mg)
ie. 100 ml solution contain 47.1 mg Vitamin C
now we take 10 ml of this vitamin C solution in beaker.
since, 100 ml solution = 47.1 mg vitamin C.
therefore,
10 ml solution = vitamun C.
Therefore, 4.71 mg vitamin C are present in beaker.
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b) 0.2056 mg
22.9 ml of DCP required to end point of the titration.
i.e. 22.9 ml DCP = 4.71 mg vitamin C
therefore,
1 ml of DCP = vitamin C.
Therefore, 0.2057 mg of vitamin C react with each ml of DCP.
i.e. 0.2057 mg/ml
A student needs to prepare 100.0 mL of vitamin C solution according to the directions in...
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
. 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.
A student adds 50 mL of his potassium iodate solution to the vitamin C suspension. However, he does not see the expected color change. Supply at least three reasons for this observation. This is a question in my Ascorbic Acid Content in Vitamin C Tablets via Iodometric Titration Lab and I want to be sure i'm correct.
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.
In the table below is represented the data for a similar titration for Vitamin C analysis. Use the data below to calculate the concentration of Vitamin C in mg/mL of juice. Given that the lodine Solution used for the titration has been standardized against a known Vitamin C solution and its was determined that 1 mL of lodine - 1.50 mg Vitamin C. Buret Reading Trial 1 Trial 2 Initial Buret Reading 0.0 mL 4.8 mL Final Buret Reading 4.8...
A student weighs a sample of potassium hydrogen phthalate (KHP) to prepare a primary standard for a titration. She later discovers that the KHP was contaminated with sugar. To determine the amount of KHP in the mixture, she takes 5.942 g of the mixture and make a 100.0 mL solution. The student then titrates 10.00 mL of this solution with a 0.1491 M sodium hydroxide solution. She finds that 13.12 mL of the NaOH solution is needed to reach the...
Vitamin C Project Lab: Part B: Data analysis Calculate the grams of Vitamin C in your Erlenmeyer. (as in titration #1 ) Calculate the grams of Vitamin C per tablet. Calculate a percent error by comparing your result to the tablet dose above. Determine the % composition of vitamin C in the tablet Build a data table similar to the one you used for titration # 1 to calculate the following: 1. 2 3. 4. Show all your work Trial...
A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and titrated with the standardized NAOH solution. From the results of this titration, the mg of ascorbic acid in the tablet was calculated. Molecular formula of ascorbic acid: C6H806 Volume of NaOH required to neutralize ascorbic acid in Vitamin C tablet (mL) 14.47 Concentration of NaOH in mol/L, 0.1964 Calculate the amount of ascorbic acid in the Vitamin C tablet in (mg). Answer:
An old tablet of vitamin C weighed 1.022 g. It was dissolved in 500. mL water, and a 25.0 mL aliquot of this solution required 22.6 mL of .00500 MI2 solution to oxidize it. Calculate the mg vitamin C in the tablet. 6.
A student dissolved 4.00 g of Co(NO_3)_2 in enough water to make 100.0 mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275 mL of a final solution. How many grams of NO^-_3 ion are there in the final solution?