A) CH3NH2 (methyl amine) is a weak base. Give the correct chemical equation for the aqueous...

Question

Question

A) CH₃NH₂ (methyl amine) is a weak base. Give the correct chemical equation for the aqueous base dissociation reaction.

B) What concentration of ammonia is required to have a solution with a pH of 11.23? K_b = 1.8x10^-5

Answer 1

Answer #1

ph po-14-11-23

Answer 2

Similar Homework Help Questions

A 25.00 mL sample of a 0.250 M aqueous solution CH3NH2 (a weak base) is titrated...

A 25.00 mL sample of a 0.250 M aqueous solution CH3NH2 (a weak base) is titrated with an 0.100 M aqueous solution of HCl (a strong acid.) The molecular and net ionic equation for the reaction is provided below. The Kb value used for CH3NH2 is 4.4x10^-4. Find the pH of the solution after addition of 15.00 mL of the aqueous solution of HCl Molecular: CH3NH2 (aq) + HCl (aq) → CH3NH3+ + Cl— Net ionic: CH3NH2 (aq) + H+ →...
The weak base methylamine, CH3NH2, has Kb= 4.2x10^-4. CH3NH2 + H2O -> CH3NH3+ + OH- Calculate...

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, CH3NH2, is a weak base and was featured in the TV show Breaking Bad. A...

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)

Methylamine, CH3NH4, is a weak base. A 0.504 M solution of methylamine has equilibrium concentrations of...

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)
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from...

In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from water to form the hydroxide ion, OH −, and hydrazoic acid, HN3, according to the following equation. N3−(aq) + H2O(l) equilibrium reaction arrow OH −(aq) + HN3(aq) The base-dissociation constant (Kb) for this base is 4.04 ✕ 10−10. If a 0.082 M solution of azide ions is prepared, what is the final pH of the solution? (Assume that the temperature is 25°C.)
Determine the ammonia concentration of an aqueous solution that has a pH of 11.30. The equation...

Determine the ammonia concentration of an aqueous solution that has a pH of 11.30. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is below: Determine the ammonia concentration of an aqueous solution that has a pH of 11.30. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is below: a)9.0 × 10-3 mol L-1 b)2.7 mol L-1 c)0.22 mol L-1 d)2.0 × 10-3 mol L-1 NH3(aq) + H20(1) = NH4+(aq) + OH-(aq) NH3(aq)...

A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4)...

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)...
4. Use of the base methyl amine (CH3NH2) to replace ozone-damaging compounds is becoming more widespread....

4. Use of the base methyl amine (CH3NH2) to replace ozone-damaging compounds is becoming more widespread. Methyl amine is now used to make pesticides and herbicides to protect potatoes and tomatoes. The K) for CH3NH2 is 4.2 x 10". (A) What would be the pH of a 0.0010 M solution of this base?! Solution:
Which of the following is the correct chemical equation for the "Kb" reaction for the weak...

Which of the following is the correct chemical equation for the "Kb" reaction for the weak base C10H7O− (2-naphthoxide ion)? A) C10H7O− + H3O+ ⇌ C10H7OH + H2O B) C10H7OH + H2O ⇌ C10H7O− + H3O+ C) C10H7O− + H+ ⇌ C10H7OH D) C10H7OH + OH− ⇌ C10H7O− + H2O E) C10H7O− + H2O ⇌ C10H7OH + OH− Given that the Ka value for 2-naphthol (C10H7OH) is 2.7×10-10, what is the value of Kb for the conjugate base C10H7O−?

The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For...

The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....