(Solved): At some point during the course, you were introduced to salt hydrates. By heating asmall sample of a ...
At some point during the course, you were introduced to salt hydrates. By heating asmall sample of a hydrated salt, you evaporated all the water molecules bound to thesalt and thus collected the anhydrous version of salt. Use the data tabulated below todetermine the moles of water (H2O) per moles of anhydrous salt (PtCl4) by assumingthat your sample was platinum(IV) chloride n hydrate, PtCl4·nH2O.Mass of evaporating dish and sample before heating 48.70 gMass of evaporating dish 43.70 gMass of PtCl4·nH2OMass of evaporating dish and sample after heating to constant temperature 47.20 gMass of water in sampleMoles of PtCl4Moles of H2OMoles of water per moles platinum(IV) chloride At some point during the course, you were introduced to salt hydrates. By heating a small sample of a hydrated salt, you evaporated all the water molecules bound to the salt and thus collected the anhydrous version of salt. Use the data tabulated below to determine the moles of water
(H_(2)O)per moles of anhydrous salt
(PtCl_(4))by assuming that your sample was platinum(IV) chloride
nhydrate,
PtCl_(4)*nH_(2)O. \table[[Mass of evaporating dish and sample before heating,48.70 g],[Mass of evaporating dish,43.70 g],[Mass of
PtCl_(4)*nH_(2)O,],[Mass of evaporating dish and sample after heating to constant temperature,47.20 g],[Mass of water in sample,],[Moles of
PtCl_(4),],[Moles of
H_(2)O,],[Moles of water per moles platinum(IV) chloride
