Question

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

Answer 1

The solution of the above question is given below with explanation

sol - vol of vitamin (= loom2 vol. of Vitamin (used - 2 mL = volume of Iodine used = 17.73 m L=b Molarity of Iodine = 5x103 M =M, According to standardisation MVI = M₂ V₂ M = M₂ V₂ M = 5*103 x 17.73 M = 0.0443

Now, we know that molarity = no of moles of solute vol. of solution (L) ..0.0443 = h 1000mL :h= 0.0443 10 no. of moles of Vitamine f = given masse molar mais here mdar mass of Vitamin (= 176.1 g/mo! .: Mass of Vitamin Lust = 0.0443 x 176.1 in tablet = 0.7809 lo Hence 0.780 g is the mass of Vitamin C in the tablet

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