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?
The weak base methylamine, CH3NH2, has Kb= 4.2x10^-4. CH3NH2 + H2O -> CH3NH3+ + OH- Calculate...
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) 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 and concentrations of CH3NH2 and CH3NH3+ in a 0.0445M Methylamine (CH3NH2) Calculate the pH and concentrations of CH3NH2 and CH3NH3 in a 0.0445 M methylamine (CH3NH2) solution. The Kb of CH3NH2-4.47 x10 Number pH11.520 Number CH,NH0.0409 Number CH, NH, |-| | 0.00446
The Kb value for methylamine is 4.2x10^-4. What is the pH of an aqueous solution for which the label reads 0.042M CH3NH2?
The Kb of methylamine (CH3NH2) is 4.4x10^-4. What is the Ka of methylamine, and what is the pOH and pH of a 0.100M solution of methylamine in water?
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
Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH of a 0.200 M Ca(OH)2 2. Calculate the equilibrium concentrations for [OH-], [HB+), and [B], the pH and pOH for a 0.200 M pyridine solution. (CsH5N) Kb = 1.4 X 10-9 3. Calculate the equilibrium concentrations for [OH-], [HB], and [B], the pH and pOH for a 0.200 M methylamine. (CH3NH2) Kb = 4.4 X 10-4 4. Calculate the equilibrium concentrations for [OH-], [HB+],...
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
Calculate the hydroxide concentration of a 0.024 M methylamine solution. Kb is 4.2 x 10-4 This problem has a second part in the problem below.... part 1 .What is the OH- concentration? B) Consider the same 0.024 M methylamine solution. Kb is 4.2 x 10-4 part 2 -- what is the pH?