What is the [H3O+] (molarity) of a 0.1067 M methylamine? See reaction below
CH3NH2 + H2O ↔ CH3NH3+ + OH- Kb = 3.70e-4
a) 1.267e-12 b) 1.639e-12 c) 6.101e-3 d) 4.716e-3
What is the [H3O+] (molarity) of a 0.1067 M methylamine? See reaction below CH3NH2 + H2O...
The weak base methylamine, CH3NH2, has Kb= 4.2x10^-4. CH3NH2 + H2O -> CH3NH3+ + OH- Calculate the equilibrium hydroxide ion concentration in a 0.95 M solution of the base. [OH-] = What are the pH and pOH of the solution?
Methylamine, CH3NH4, is a weak base. A 0.504 M solution of methylamine has equilibrium concentrations of both CH3NH3^+ and OH^- equal to 0.0150 M. What is the Kb of the base? CH3NH2(aq) + H2O(l) <> CH3NH3^+(aq) + OH^-(aq)
Methylamine, CH3NH2, is a weak base and was featured in the TV show Breaking Bad. A 0.504 M solution of methylamine has equilibrium concentrations of both CH3NH,* and OH' equal to 0.0150 M. What is the Kb of the base? CH3NH2 (aq) + H20 (1) = CH3NH3* (aq) + OH (aq)
A) CH3NH2 (methyl amine) is a weak base. Give the correct chemical equation for the aqueous base dissociation reaction. CH3NH2(aq) + H2O(l) ⇋ CH3NH3+ (aq) + HO−(aq) CH3NH2(aq) + H2O(l) ⇋ CH3NH3+ (aq) + H3O+(aq) CH3NH2(aq) + H3O+(aq) ⇋ CH3NH3+ (aq) + H2O−(l) CH3NH2(aq) + H2O(l) ⇋ CH3NH− (aq) + H3O+(aq) B) What concentration of ammonia is required to have a solution with a pH of 11.23? Kb = 1.8x10-5
Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH2 tor (methylammonium chloride). Report answer to 2 decimal places. Kb CH3NH2) - 44 x 10-4 CH3NH2 (aq) + H200 + CH3NH3 (2) + OH(aq) Assuming equal initial concentrations of the given species, which of the following is the weakest acid in aqueous solution? O. HB Ky = 2.0 x 10-6 OB.HD K = 6.0 x 10-2 ОС: НЕ Kg = 4.0 x...
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH of 11.8, what is the initial molar concentration of methylamine in the solution? O A 2.6x10-4M O B 7.7x10-2M O c 3.4x10-5M O D 8.3x10-2M Triethylamine (C2H5)3N) has a pKb = 3.25. What is the value of the equilibrium constant K for this reaction: (C2H5)3NH(aq) + H2O(1) = (C2H5)3N(aq) + H3O+(aq)? O A 1.77x10-11 O B 5.62x10-4 o C More information is needed to...
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
What is the pH of a 0.650 M solution of methylamine (CH3NH2)? Kb=4.4x10-4
What is the Kb for methylamine, CH3NH2, if a solution prepared by dissolved 0.82 mol of methylamine in 425 mL of H2O has a pH of 12.46? (Ans: 4.4 x 10-4) A 0.100 M solution of formic acid, HCOOH, is 4.0% dissociated. Calculate Ka for formic acid. (Ans: 1.7 x 10-4)
What is the pH of the resulting solution if 30. mL of 0.432 M methylamine, CH3NH2, is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+ ?