Oh, chemistry! Let's break it down, my friend.
(i) To find the molar mass of KIO3, we need to add up the atomic masses of potassium (K), iodine (I), and oxygen (O). The atomic masses are K = 39.1 g/mol, I = 126.9 g/mol, and O = 16.0 g/mol. So, KIO3 has a molar mass of 39.1 + (3 * 16.0) + 126.9 = 214.1 g/mol. And its associated uncertainty would be ¡¾0.0002 g/mol. So, the molar mass of KIO3 is 214.1 (¡¾0.0002) g/mol.
(ii) Now, let's find the molarity of the solution. Molarity (M) is defined as moles of solute per liter of solution. We know that we dissolved 0.2222 g of KIO3 in 50.00 mL of solution. First, we need to convert mL to L by dividing by 1000: 50.00 mL / 1000 = 0.05000 L.
Next, we need to find the number of moles of KIO3. We can do that by dividing the mass of KIO3 by its molar mass:
moles of KIO3 = 0.2222 g / 214.1 g/mol = 0.001037 mol.
Finally, we can find the molarity by dividing moles by liters: M = 0.001037 mol / 0.05000 L = 0.02074 M.
Since the mass of the solute was given with an uncertainty of ¡¾0.0002 g, the molarity will have the same relative uncertainty. Therefore, the molarity of KIO3 is 0.02074 (¡¾0.00002) M.
(iii) Ah, the purity question! If the reagent were only 99.9% pure, it means that 0.1% of it is impurities. It might not sound like much, but when it comes to calculations, every little bit counts! It would affect our results because the impurities would contribute to the mass and therefore to the molarity calculation. So, yes, the answer would be affected significantly if the reagent were only 99.9% pure. It's always better to work with pure substances in chemistry because we want precise results without any clowns messing around, right?