17. Acid and Base Equilibrium

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

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.

Calculate the pH of a solution that is 0.0190 M in NaOH and 0.0870 M in sodium acetate (K_a for CH_3COOH = 1.75 x 10^-5). What is the pH?

What is the pH of a solution containing 400 mg of caffeine with a pKb of 10.4, if the solution has a 3.44% mass concentration and a density of 1.01 g/mL?

Calculate the pH of a 0.30 M solution of barium nitrite. Given that the Ka of HNO2 is 4.5 x 10^-4, what is the pH of the solution?

Calculate the pH of a solution that is 0.205 M in CH3NH2 and 0.155 M in CH3NH3Br. Assume the Kb for CH3NH2 is 4.4 x 10^-4.

Calculate the pH of a solution that is 0.205 M in CH3NH2 and 1.55 M in CH3NH3Br. Assume the Kb for CH3NH2 is 4.4 x 10^-4.

What is the theoretical pH of a 0.1 M solution of sodium acetate (NaC2H3O2), a weak base?

What is the pH of a 0.1 M solution of ammonia (NH3), a weak base with a Kb of 1.8 x 10^-5?

Which of the following methods can be used to estimate the pH of a weak base solution if the pKa values are not provided?