Question- Hydroxylamine, NH2OH, is a weak base. The following is the equilibrium equation for its reaction with water: NH2OH(aq) + H2O(l) <----------> NH3OH+(aq) + OH- Kb = 9.1 x 10-9 What is the pOH of a 2.37 M NH2OH solution?
Note: Assume that the ionization of the base is small enough in comparison to its starting concentration that the concentration of unionized base is almost as large at equilibrium as it was originally. This will allow you to avoid having to solve the quadratic formula when doing your ICE table calculation.
1.15
3.83
4.99
6.72
8.13
Not confident which formulas/units I require to solve something like this