The formula for borax is written as $\ce{Na2B4O7.10H2O}$ and also as $\ce{Na2[B4O5(OH)4].8H2O}$.  
From the structure, it obvious from where the 2nd formula comes. But the question I have is, what is the water of crystallisation in Borax, 8 or 10?

More specifically, I was to know what's the proper defintion of water of crystallisation? If it is just the number of water molecules present in the crystal structure, not directly bonded to the molecule (Which is what I thought) then the answer should be 8.  
But one my teachers said it should be 10, as written in the formula, while the other who used to say 8 couldn't give an explanation to following

"Borax, when heated loses all 10 water molecules. When dissolved in water, all 10 water molecules are lost*. So even though they're bonded to the boron, the 2 water molecules behave the same way as the other 8, chemically"  
*Just to mention, the full compound breaks up anyways, so I'm not so convinced with this argument


Another compound which came up in my mind during this was $\ce{CuSO4.5H2O}$, The structure of which is [![Structure of CuSO4.5H2O][1]][1]  

What would be the water of crystalisation in Copper Sulphate? I'm sure there will be lot more compounds having $\ce{H2O}$ molecules bonded like this. What would be the "Water of crystallisation" in them and what's the proper definition of it? 

Unlike Borax, Copper Sulphate doesn't lose all water molecules at once on heating, just opposite of the argument given above for Borax. 
[![Heating reaction of Copper Sulphate][2]][2]


  [1]: https://i.sstatic.net/DyWu7.png
  [2]: https://i.sstatic.net/mQico.png