Calculate the PH and concentrations of CH3NH2 and CH3NH3+ in a 0.0445M Methylamine (CH3NH2)
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Calculate the PH and concentrations of CH3NH2 and CH3NH3+ in a 0.0445M Methylamine (CH3NH2) Calculate the...
Calculate the pH and concentrations of CH NH, and CH NH; in a 0.0293 M methylamine (CH, NH,) solution. The Kb of CH3NH, is 4.47 x 10-4. pH = [CH, NH] = [CH, NH}=
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?
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)...
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...
Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. 1.61 8.75 5.25 12.39
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)
A chemistry graduate student is given 125. mL of a 0.10 M methylamine (CH3NH2 solution. Methylamine is a weak base with K,-4.4x 10- . what mass of CH3NH3 Br should the student dissolve in the CH3NH2 solution to turn it into a buffer with pH = 10.50? You may assume that the volume of the solution doesn't change when the CH3NH3 Br is dissolved in it. Be sure your answer has a unit symbol, student dissalve in the CH,NH, solution...
(17.2b.3) A 8.57×10-2-M aqueous solution of CH3NH2 (methylamine) has a pH of 11.8. Calculate the pH of a buffer solution that is 8.57×10-2 M in CH3NH2 and 0.156 M in CH3NH3+.
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)
Calculate the pH of a solution prepared by mixing equal volumes of 0.18M methylamine (CH3NH2, Kb = 3.7