Answer:
The water of crystallization for the formula of the unknown hydrate is 2.
Explanation:
Mass of an unknown hydrate = 1.000 g
Molar mass of hydrate = 195.5 g/mol
MOles of unknown hydrate =[tex]\frac{1.000 g}{195.5 g/mol}=0.00512 mol[/tex]
Mass of hydrate after heating = 0.781 g
Mass of water lost due to heating = x
[tex]1.000 g = 0.781 g + x\\x = 1.000 g - 0.781 g = 0.219 g[/tex]
Moles of water lost =[tex]\frac{0.219 g}{18.01528 g/mol}=0.0122 mol[/tex]
[tex]AC.xH_2O+Heat\rightarrow AC+xH_2O[/tex]
1 Mole of hydrate has x moles of water and 0.00512 moles of hydrate has 0.0122 moles of water then we can write:
[tex]\frac{1 }{x}=\frac{0.00512 }{0.0122 }\\x\approx 2[/tex]
The water of crystallization for the formula of the unknown hydrate is 2.
