Calculate the concentrations of all species present and the pH in 0.10M solutions of the Ethylammonium Nitrate (C2H5NH3)NO3.

Kb of C2H5NH2 = 6.4x10^-4

Question

Calculate the concentrations of all species present and the pH in 0.10M solutions of the Ethylammonium Nitrate (C2H5NH3)NO3.

Kb of C2H5NH2 = 6.4x10^-4

anonymous · Answer

I know this is a acid-base properties of salt, so when this dissolves in water, C2H5NH3 and NO3 splits apart giving NO3 concentration of .1M. I also figured out the concetration of [H3O], [C2H5NH2], [C2H5NH3], but I get lost when im trying to find OH-

cuanchi · Answer

whenever you have [H+] you can calculate pH, pOH, and [OH-], knowing that 
Kw=[H+][OH-]= 1x10^(-14)

anonymous · Answer

ah haaa. thank you !!!!!

cuanchi · Answer

and 
pH + pOH = 14

anonymous · Answer

so the question is asking for the pH of NO3(C2H5NH3).

I found that the C2H5NH3 = .1M 
and that C2H5NH2 = 1.25x10^-6

Whenever i do -log[C2H6NH2] i get the correct answer of 5.9 pH.

anonymous · Answer

I don't get how i get the right answer if i find the -log[C2H6NH2] instead of -log[C2H6NH3]

anonymous · Answer

ahhh i forgot its -log [H+] = pH

cuanchi · Answer

[C2H6NH2]=[H+]=1.25x10^-6