given that 40.14g sample of hydrated NiSO4 is reduced in mass to 22.14g upon heating.
Show that the formula of the hydrate is NiSO4.7H20
n / M
The Attempt at a Solution
22.14g/ 40.14g = 0.5516 (mol of NiSO4)
40.14g - 22.14 = (18 g H20 lost in heating)
18.0 / 18.02 = 0.9989 (mol of H20)
∴ mole ratio = 0.5516 : 0.9989
but this does not give the result in the ratios of 1:7 (NiSO4.7H20)
stoichiometry (or chem for that matter) isn't really my thing and I have about 10 questions similar to this, can someone please point me in the right direction please?