1. Everyone said hydrogen bonding.. I was like the only one who said ion-dipole interactions.. Crud.. xD
2. Yap.. Same. (water vapour at first, brown gas in the end)
3. Now, this is the thing.. I felt that the enthalpy change would JUST be the same because HCl and HNO3 both dissociate almost fully in water and it would leave almost "no effect." That is if I articulated well. All I wrote in the paper was that with the two acids, the ionic equation would still be about the same so.. Again crud..
4. The only thing I said was that bidentate ligands were more stable (this is the damn conclusion).. I also said the products are energetically more stable than the reactants (also conclusion instead of explanation).. After searching, I found out it was possibly because there are more moles on the products in equilibrium II. That level of analysis is crazy for just a one mark question.. xD
5. My concentration was too big. I think I got 7 mol dm-3 or something. Way too much to dilute a 1 x 10^-4 mol dm-3 to a 1 x 10^-7 mol dm-3. I just used random "initial concentration, reacting concentration, equilibrium concentration" thing and everything just got weird..
6. I said one of them was more acidic because one weakens the -OH bond more because one alkyl group is more electron-donating, so the the electrons are pulled more toward the C=O bond and make a more delocalised strucutre, less H+ blah blah blah
7. I have no clue. I wrote CH3NH2 + H+ -> CH3NH3+
CH3NH3Cl -> CH3NH3+ + Cl-.I'm way off from you guys..
In conclusion, shoot.