PH of solution (not enough infromation?)

[Haxx0rm4ster]

Both are confusing me. I don't know what information to use (K values)
I'd really appreciate some help!


Calculate the concentration of all species present in a 0.25M solution of ethylammonium chloride (C2H5NH3CL)
(Not sure you if you may need this, but C2H5NH2 has a Kb value of 5.6*10^-4... it is not given in the question, it's in the appendixes of my book, which are used a lot in these problems)



Calculate the pH of a 0.050M Al(NO3)3 solution. Ka value for Al(H2O)6 3+ is 1.4*10^-5.



EDIT: hmmm after reading analyzing it a little bit, I think I'm supposed to find the Kb of C2H5NH2 for the first one.. in other words
1ee-14/5.6ee-4
right?
And that would lead to the answer being
[C2H5NH3 +] = 0.25M (% dissociation is insignificant)
[Cl -] = 0.25M
[H +] = [C2H5NH2] = 2.1ee-6M
Does this look right?

 

[GCT]

Hi, both of these questions involve setting up an equilibrium constant equation. So you can start by showing us this setup for both problems.