$\backslash$table$[[$Substances$,$Mass $($Grams$)],[$Mass of crucible,$24\mathrm{.}36$ grams$],[$Mass of crucible and ANHYDROUS sample,$28\mathrm{.}31$ grams$],[$Mass of CuSo$4,],[$Moles of CuSo$4,]]$

$\backslash$table$[[$Substances$,$Mass $($Grams$)],[$Mass of crucible and hydrated sample,$30\mathrm{.}52$ grams,$],[$Mass of crucible and ANHYDROUS sample,$28\mathrm{.}31$ grams,$],[$Mass of CuSo$4,,],[$Moles of CuSo$4,,]]$

#$1$ Calculate mass of water, mass of compound $\%$ water mass in the sample of hydrated copper $($II$)$ sulfate showing calculations

#$2$ Based on the result determine the chemical formula for CuSo$4*H2O$

#$3$ Suppose you heated a sample of hydrated ionic compound in a test tube, what might you expect to see near the mouth of the test tube, explain $($what you expect to see$)$

#$4$ Calculate the percentage composition of the hydrated copper $($II$)$ sulfate

#$5$ Do you think it's, more useful to have the percent by mass of a hydrate or the percentage composition, explain. $($ pick which one you think is the best and explain your reasoning$)$