What is the titer of the iodine solution of the .1000g sample of pure ascorbic acid 25.32 ml I2
By definition, titer is (normality x equivalent weight). I don't know how you are using it so I'll leave it at that. I rarely used this when I was in school years ago. I looked in several of the newer quant books and it wasn't listed in the index. I did find one reference in a book from the 1960s. Another note: one rarely finds normality used in modern texts, either. I'm sorry to see normality go. In my opinion that isn't progress.
To determine the titer of the iodine solution using the information provided, we need to use a titration calculation. Here's how you can do it step by step:
1. Convert the volume of iodine solution from milliliters to liters:
25.32 mL = 0.02532 L
2. The equation for the reaction between ascorbic acid (C6H8O6) and iodine (I2) is:
C6H8O6 + I2 -> C6H6O6 + 2HI
From the balanced equation, we see that the molar ratio between ascorbic acid and iodine is 1:1.
3. Calculate the number of moles of iodine used in the reaction:
Number of moles of I2 = Volume of I2 solution (in liters) × Titer of I2 solution
Let's assume the titer of the iodine solution is 'x' moles per liter:
Number of moles of I2 = 0.02532 L × x mol/L
4. Since the molar ratio between ascorbic acid and iodine is 1:1, the number of moles of ascorbic acid (C6H8O6) is equal to the number of moles of iodine used in the reaction.
5. Calculate the molar mass of ascorbic acid (C6H8O6):
C = 6 × 12.01 g/mol = 72.06 g/mol
H = 8 × 1.01 g/mol = 8.08 g/mol
O = 6 × 16.00 g/mol = 96.00 g/mol
Total molar mass = 72.06 g/mol + 8.08 g/mol + 96.00 g/mol = 176.14 g/mol
6. Calculate the mass of ascorbic acid used in the reaction:
Mass of ascorbic acid = 0.1000 g
7. Convert the mass of ascorbic acid to moles using its molar mass:
Number of moles of ascorbic acid = Mass of ascorbic acid / Molar mass of ascorbic acid
Number of moles of ascorbic acid = 0.1000 g / 176.14 g/mol
8. Equate the number of moles of iodine to the number of moles of ascorbic acid:
0.02532 L × x mol/L = 0.1000 g / 176.14 g/mol
9. Solve for the titer of the iodine solution (x):
x = (0.1000 g / 176.14 g/mol) / 0.02532 L
By plugging in the values and performing the calculation, you will get the titer of the iodine solution.
To determine the titer of the iodine solution, we need to use the equation:
Ascorbic acid + I2 → Dehydroascorbic acid + 2I-
Based on the balanced equation, we know that 1 mole of ascorbic acid reacts with 1 mole of iodine (I2). Therefore, we can calculate the number of moles of iodine that reacted with the ascorbic acid.
First, let's convert the volume of iodine solution used from milliliters to liters:
25.32 ml = 0.02532 L
Now, since we know that the reaction is a 1:1 ratio with iodine, the number of moles of iodine used in the reaction is the same as the number of moles of ascorbic acid:
Number of moles of iodine (I2) = Number of moles of ascorbic acid
Next, we need to calculate the number of moles of ascorbic acid in the 0.1000 g sample. To do this, we'll use the molar mass of ascorbic acid, which is 176.12 g/mol:
Number of moles of ascorbic acid = Mass of sample / Molar mass
Number of moles of ascorbic acid = 0.1000 g / 176.12 g/mol
Now we can convert the number of moles of ascorbic acid into moles of iodine:
0.1000 g / 176.12 g/mol = moles of ascorbic acid
Since the ratio is 1:1, it means that the number of moles of iodine will be the same:
Moles of iodine = moles of ascorbic acid
Finally, to calculate the titer of the iodine solution, we divide the moles of iodine from the reaction by the volume of the iodine solution used:
Titer (Molarity) = Moles of iodine / Volume of iodine solution (L)
Titer = Moles of iodine / 0.02532 L
This will give us the titer of the iodine solution.