1- In the titration between potassium iodate and the sodiumthiosulfate solution, if the titration is not performed immediatelyafter the addition of the sulfuric acid, how would this likelyaffect the calculated concentration of your diluted sodiumthiosulfate solution?
2- Why did the titrations performed need to be startedimmediately after adding the sulfuric acid?
3- A sample of bleach was analyzed as in this procedure. Theonly procedural difference is that the student weighed out thebleach solution used instead of pipetting a certain volume ofbleach. The student weighed out 0.634 g of commercial bleachsolution. It was found that it required 13.24 mL od 0.0732 M sodiumthiosulfate solution to react with the iodine produced. What is thepercentage of sodium hypochlorite in this bleach sample?
4- The active ingredient in many commercial liquid bleaches issodium hypochlorite. The bottle lists the percentage of sodiumhypochlorite as 6.0%. If the density of commercial bleach is 1.084g/mL of 0.150 M sodium thiosulfate is required to reach the endpoint in a titration similar to the one performed in thisexperiment, if a student analyzed a 2.0 mL sample of bleach.
