Answer Happy

9 THROUGH 12 PLEASE!!!!!
5. If the 0.2124 of potassium iodate are dissolved to make 250ml of solution what is the molarity? 6. If you remove a 25ml aliquot of potassium iodate from the 250ml of solution, a. How many moles potassium iodate is this? b. How many moles of iodate ions is this? 7. Calculate the moles represented by 0.5 g of potassium iodide. How many moles of iodide will this create? 8. Calculate the moles represented by 2.00 mL of 1.00MH2​SO4​. How many moles of hydrogen ions will this create? 9. Use equation (1) below and your answers to 6,7 , and 8 to calculate the limiting reagent. Use your answer from #9 to calculate the moles of I2​ that will be produced by the limiting reagent. 10. Using your moles of I2​, use equation (2) below to find the moles of Na2​ S2​O3​ necessary for a complete reaction. 11. If you used 25.30 mL of Na2​ S2​O3​ to do the titration, use the moles of Na2​ S2​O3​ from 10 and the volume to find the molarity. 12. Read through the lab and have a carefully organized lab set up where each piece of data you will enter has a labeled spot. For example, for each titration that you will perform, you will need a spot to record the initial volume, the final volume and the volume used in the experiment. You will also have a number of masses that you will be recording. 13. Apply Henry's Law below to calculate the concentration of oxygen in water (at 25∘C ). Henry's law is discussed in your textbook.
Lab Experiment The solution that you make this week will be used in the determination of dissolved oxygen in water samples. It is important that this solution be made up correctly. Be sure to check with you instructor when the lab requests you to do so. Because sodium thiosulfate is a hydrated compound, it is impossible to determine the exact amount of sodium and thiosulfate ions in a solution by weighing a particular mass since this mass contains an amount of water that will vary with humidity, exposure to air and many other variables. Consequently, you will only be able to make your sodium thiosulfate solution to approximately the desired molarity. In order to determine the exact concentration you will perform a titration using the sodium thiosulfate solution you have made with a compound which doesn't absorb water and thus can be weighed exactly. Potassium iodate, a free flowing solid that can be weighed out very accurately will be used in the standardization. From the volume of sodium thiosulfate solution necessary to titrate a potassium iodate solution of known concentration, the concentration of the sodium thiosulfate solution can be determined. The standardization is based on these reactions: IO3−​(aq)+5I−(aq)+6H+(aq)→3I2​(aq)+3H2​O2Na2​ S2​O3​+I2​(aq)→2Na++S4​O6−2​+2Na++2l−​