Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reaction can be generically symbolized as NX3(aq)+H2O(l)-->HNX3(aq)+OH^-(aq) where NX3 is the base and HNX3 is the conjugate acid. The equilibrium-constant expression for this reaction is
Kb=[HNX3^+][OH^-]/[NX3] where Kb is the base ionization constant.
PART A
1.) If Kb for NX3 is 5.0*10^-6, what is the pOH of a 0.175 M aqueous solution of NX3?
pOH=
2.) If Kb for NX3 is 5.0*10^-6, what is the percent ionization of a 0.325 M aqueous solution of NX3?