Statement 1: ${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}$ on heating to ${250}^{o}C$ loses all the five ${\mathrm{H}}_2\mathrm{O}$ molecules and becomes anhydrous.

Statement 2: All five ${\mathrm{H}}_2\mathrm{O}$ molecules are coordinated to the central ${\mathrm{Cu}}^{2+}$ ion.

Statement 1: ${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}\left(\text{blue}\right)\stackrel{{250}^{\mathrm{o}}\mathrm{C}}{\to }{\mathrm{CuSO}}_4\left(\text{white}\right)+5{\mathrm{H}}_2\mathrm{O}\uparrow$. Anhydrous copper sulphate becomes white because there is no d-d transition of electron in absence of ligands according to crystal field theory.
Statement 2: Four water molecules are coordinated to ${\mathrm{Cu}}^{2+}$ and fifth one is hydrogen bonded to two water molecules and anion, ${\mathrm{SO}}_4^{2-}$.