What is the pH of a 0.200 M CH3NH3Br solution, given that the Kb of CH3NH2 is 4.4 × 10^(-4)?

A solution of sodium acetate (NaCH3COO) has a pH of 9.64. The acid-dissociation constant (Ka) for acetic acid is 1.8 x 10^-5. What is the molarity of the sodium acetate solution?

What is the expression for the equilibrium constant (Kb) for the dissociation of a weak base in water?

What is the pH of a 0.05 M sodium fluoride solution, given that F⁻ has a Kb of 1.59 x 10⁻¹¹?

What is the pH of a 0.145 M solution of (CH3)3N, given that the Kb of (CH3)3N is 6.4 × 10⁻⁵?

What is the pH of a 0.225 M (CH3)2NH2Br solution, given that the Kb of (CH3)2NH is 5.4 × 10⁻⁴?

What is the pH of a 7.0 × 10⁻³ M NH₃ solution? (Kb = 1.8 × 10⁻⁵ for NH₃)

What is the pH of a one liter solution that is 0.100 M in NH3 and 0.100 M in NH4Cl after 1.4 g of NaOH has been added? Kb for NH3 is 1.8 × 10^-5.

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10⁻⁴ for methylamine.