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Question 6D.15(b) in the 7th Edition of Chemical Principles asks to find the pH of a system with 0.055 M AlCl3. I am confused as to how to proceed with this problem, because I do not know how this molecule can create hydronium or oxide ions. Did anyone figure this one out?
Al3+ cations become hydrated by water molecules that act as Bronsted acids when they are placed in water so Al3+ will become Al(H2O)6 as seen in Table 12.8. Metal cations usually have 6H2O molecules attached to it. That will be used as your acid and you can set up the equation such that Al(H2O)6+H2O--> H3O+ Al(H2O)5OH.
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