Final answer:
To find Kb for methylamine (CH3NH2), use the concentration of CH3NH3 (2.32 × 10-6 M) and CH3NH2 (0.20 M) in the solution. Kb is the equilibrium constant for the reaction of CH3NH2 with water to form CH3NH3+ and OH-. After calculation, the Kb will be 2.6776 × 10-5.
Step-by-step explanation:
To find Kb for methylamine (CH3NH2), we can use the concentration of CH3NH3 (2.32 × 10-6 M) and the concentration of CH3NH2 (0.20 M) in the solution. Kb is the equilibrium constant for the reaction of CH3NH2 with water to form CH3NH3+ and OH-.
The equation for this reaction is CH3NH2 + H2O ⇌ CH3NH3+ + OH-. At equilibrium, the concentrations of CH3NH3+ and OH- are equal to each other and equal to the concentration of the methylamine (2.32 × 10-6 M).
Kb can be calculated using the equation:
Kb = ([CH3NH3+][OH-]) / [CH3NH2]
Plugging in the given values:
Kb = ((2.32 × 10-6 M) × (2.32 × 10-6 M)) / (0.20 M)
= 2.6776 × 10-5
Therefore, the value of Kb for methylamine is 2.6776 × 10-5.