2.18 gg of bleach solution are treated with excess KI to generate I3- according to Equation 1 on page 161 in the lab manual. 27.08 mLmL of the standardized S2O32- solution in Part B are required to reach the endpoint of the titration. How many mmoles of S2O32- is this? (Use Equation 2.)

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

Using the periodic table, complete the table to describe each atom. type in your answers

What is the correct lewis structure for chloroform chcl3