A student titrates 25.0 mL of orange juice with 0.0100 mol/L iodine solution…
Contributed by StemPy LabTry it on paper first. A hint, the key idea and the worked solution are here when you need them.
A student titrates of orange juice with iodine solution. The vitamin C in the juice reacts with iodine in a 1 : 1 ratio. The juice needs of the iodine solution. The molar mass of vitamin C is . Find the amount of iodine used, the mass of vitamin C in the sample, and the concentration of vitamin C in the juice in mg for each .
Need a reminder? The key ideaShow
Fat-soluble vitamins (A, D, E, K) are stored in the body. Water-soluble vitamins (B group and C) are not, except B12. Vitamin B12 contains cobalt. Vitamin C reacts with iodine in a 1 : 1 ratio: . The mass fraction of an element in a compound is .
The worked solution
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Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.
Plan. Moles of iodine equal moles of vitamin C. Then use the molar mass.
Step 1. Iodine. .
Step 2. Mass of vitamin C. The same amount of vitamin C: .
Step 3. Per 100 mL. .
Answer: , and in each .
Check. Orange juice usually holds some tens of mg of vitamin C in each 100 mL, so the answer is in the right range.
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