Assignment:
Question 1. Methylamine, CH3NH2, is a weak base that reacts according to the equation CH2NH2 + H2O <--> CH3NH3^1+ + OH^1-. The value of the ionization constant, Kb, is 5,25 x 10^-4. Methylamine forms salts such as methylammonium nitrate, (CH3NH3^1+)(NO3^1-).
Question 2. Calculate the pH of a solution maded by adding 0.0100 mole of a solid methylammonium nitrate to 120.0 mL of a 0.225-molar solution of methylamine. Assume that no volume change occurs. (The answer i got was pH=11.15)
Question 3. How many moles of either NaOH OR HCl (state clearly which you choose) should be added to the solution in (b) to produce a solution that has a pH of 11.00? Assume that no volume change occurs.
Provide complete and step by step solution for the question and show calculations and use formulas.