A vitamin C tablet was dissolved in 50.0 mL of water. The resulting solution was titrated to the equivalence point with 28.5 mL of 0.100 M I3− solution. What is the starting mass of the tablet assuming the tablet is 100% vitamin C?
I found the moles in I3- to be .00285. and the ratio of triodide to Vitamin C is 1:1. I found that there is 176.124 grams of Vitamin C. Now what should I do?
To find the starting mass of the tablet, you need to multiply the moles of Vitamin C (0.00285) by the molar mass of Vitamin C (176.124 g/mol). This gives you a result of 0.5067 g, which is the starting mass of the tablet.
Well, congratulations on finding the moles in I3- and the molar mass of vitamin C! Now it's time for the grand finale of this chemistry circus -- calculating the starting mass of the tablet.
Since the ratio of triiodide (I3-) to vitamin C is 1:1, we know that the moles of vitamin C in the tablet are also 0.00285.
To calculate the mass of vitamin C, we can use the equation:
Mass (g) = Moles × Molar Mass.
Plugging in the values, we get:
Mass = 0.00285 mol × 176.124 g/mol.
Calculating that, we find:
Mass = 0.503 grams.
So the starting mass of the vitamin C tablet, assuming it is 100% vitamin C, is approximately 0.503 grams. Keep in mind, though, that this is just an estimate based on your calculations.
To find the starting mass of the vitamin C tablet, you need to use the molar mass of vitamin C (ascorbic acid) and the number of moles of iodine triiodide (I3-) solution that reacted with it.
The molar mass of vitamin C is 176.124 grams per mole, as you calculated.
Since the ratio of triiodide (I3-) to vitamin C is 1:1, the moles of vitamin C are also 0.00285.
Now, you can use the equation:
Mass of vitamin C = moles of vitamin C × molar mass of vitamin C
Plugging in the values, you get:
Mass of vitamin C = 0.00285 moles × 176.124 grams/mole
Calculating this, the starting mass of the vitamin C tablet is approximately 0.502 grams.
To calculate the starting mass of the tablet, you need to use the balanced chemical equation and the molar ratio between iodine ions (I3-) and vitamin C (ascorbic acid).
The balanced equation for the reaction between vitamin C and iodine ions is:
C6H8O6 + I3- -> C6H6O6 + 3I-
From the equation, you correctly determined that the molar ratio between iodine ions and vitamin C is 1:1. This means that for every mole of iodine ions used in the reaction, there is one mole of vitamin C.
You also correctly calculated the moles of iodine ions to be 0.00285.
Since the molar ratio is 1:1, the moles of vitamin C in the tablet are also 0.00285.
To calculate the starting mass of the tablet, you need to use the molar mass of vitamin C, which is 176.124 grams/mole.
Starting Mass (g) = Moles of Vitamin C x Molar Mass of Vitamin C
= 0.00285 moles x 176.124 grams/mole
Now, you can calculate the starting mass of the tablet by multiplying the moles of vitamin C by its molar mass.
Starting Mass (g) = 0.00285 moles x 176.124 grams/mole
Therefore, the starting mass of the tablet assuming it is 100% vitamin C is 0.502 grams.