I made an iodine solution referring to the methodology provided in this link: https://www.thoughtco.com/vitamin-c-determination-by-iodine-titration-606322
$$\ce{KIO3 + 5KI + 3H2SO4->3I2 + 3H2O + 3K2SO4}$$
I want to calculate the molarity of the iodine solution produced from reacting $\pu{0.268g}$ of potassium iodate and $\pu{5g}$ of potassium iodide. I'm not sure how to calculate that.
I tried finding the limiting reactant and calculating the number of moles based off of that, but I'm not sure if that's right. Also, in order to calculate molarity you need volume. Based on the procedure outlined in the link, first I dissolved $\ce{KI}$ and $\ce{KIO_3}$ in $\pu{200ml}$ of water, but then I'd to add $\pu{30ml}$ of sulfuric acid and make it up to $\pu{500ml}$. So, I wonder what volume should I take into account when calculating molarity, $\pu{200ml}$ or $\pu{500ml}$?