Question

1. Calculate the pH of a 0.175 M aqueous solution of hydroxylamine (NH₂OH, K_b = 9.1×10^-9) and the equilibrium concentrations of the weak base and its conjugate acid.

pH	=
[NH2OH]equilibrium	=	M
[NH3OH+]equilibrium	=	M

2. Calculate the pH of a 0.0440 M aqueous solution of dimethylamine ((CH₃)₂NH, K_b = 5.9×10^-4) and the equilibrium concentrations of the weak base and its conjugate acid.

pH	=
[(CH3)2NH]equilibrium	=	M
[(CH3)2NH2+ ]equilibrium	=	M

Answer 1