The amount of i₃⁻(aq) in a solution can be determined by titration with a solution containing a known concentration of s₂o₂⁻³(aq) (thiosulfate ion). the determination is based on the net ionic equation 2s₂o₃²⁻(aq)+i₃⁻(aq)⟶s₄o₆²⁻(aq)+3i⁻( aq). given that it requires 38.1 ml of 0.440 m na₂s₂o₃(aq) to titrate a 25.0 ml sample of i₃⁻(aq), calculate the molarity of i₃⁻(aq) in the solution.

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.)