weight of the tablet = 1.022 g
it was dissolved in 500 ml and from that 25 ml was taken for analysis
22.6 ml of 0.00500 M I2 solution required
moles of I2 required = 0.0226*0.00500 = 1.13*10^-4 M
so moles of vitamin C present in the 25 ml aliquot = 1.13*10^-4 M
vitamin C present in the stock = 2.26*10^-3 M
Amount of vitamin C in the tablet = 176.12*2.26*10^-3*1000 = 398 mg
An old tablet of vitamin C weighed 1.022 g. It was dissolved in 500. mL water,...
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...
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:
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 4.112-g tablet, containing quinine was dissolved in 0.10 M HCl to give 500 mL. Dilution of a 10.0-mL aliquot to 100 mL yielded a reading for fluorescence intensity (at 347.5 nm) of 320 on an arbitrary scale. A second 10.0-mL aliquot was mixed with 10.0 mL of 100-ppm quinine solution before dilution to 100 mL. The fluorescence intensity of this solution was 433. Calculate the percentage of quinine in the tablet.
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 tablet weighing 2.074 g and containing aluminium salts was dissolved and diluted to 100.0 mL in a volumetric flask. A 25.00 mL aliquot was removed and treated with enough ammonia to precipitate the aluminium (Al) present as aluminium hydroxide (Al(OH)3). After ignition at 800 oC, this precipitate was converted to aluminium oxide (Al2O3) weighed 0.1967 g. Calculate the Al% in the tablet.
A Tums tablet weighed 1.319 g. Using the procedure of this experiment, the tablet was dissolved in, and reacted with, an excess amount of HCl (125.00 mL of 0.101 M HCl). The excess unreacted HCl was titrated with NaOH; 18.75 mL of 0.101 M NaOH was used to reach the endpoint. Calculate the moles of HCl that did not react with the antacid. Calculate the moles of HCl that did react with the antacid. Calculate the mass of HCl that...
A solid weak acid is weighed, dissolved in water and diluted to exactly 50.00 ml. 25.00 ml of the solution is taken out and is titrated to a neutral endpoint with 0.10 M NaOH. The titrated portion is then mixed with the remaining untitrated portion and the pH of the mixture is measured. Mass of acid weighed out (grams) 0.773 Volume of NaOH required to reach endpoint: (ml) 19.0 pH of the mixture Ihalf neutralized solution 3.54 Calculate the following...
A tablet containing some Vit C (ascorbic acid) was dissolved in water then titrated with 24.88 ml of 0.1085 M NaOH. What is the w/w% of Vit C in the tablet if the tablet weighed 0.6672 g? (use Vit C = 176.0 g/mol) NaOH + Vit C rightarrow sodium ascorbate + H_2O