Question
A weak base that encompasses a concentration of 1.4 mol per litre has a percent ionization of 0.63%. Calculate the Kb of this weak base
Answers
Let's call a weak base BOH.
BOH ==> B^+ + OH^-
Kb = (B^+)(OH^-)/(BOH)
Look at the ICE chart.
I = initial concn (before ionization):
BOH = 1.4 mols/L.
(B^+) = 0
(OH^-) = 0
C = change in concn:
(B+) = +1.4*0.0063
(OH^-) = +1.4*0.0063
(BOH^-) = 1.4*0.9937 (0.9937 is the fraction from 100%-0.63% = 99.37%)
E = equilibrium concn:
(B^+) = 1.4*0.0063 = ??
(OH^-) = 1.4^0.0063 = ??
(BOH) = 1.4-(1.4*0.0063) OR (1.4*0.9937= ??)
Substitute the equilibrium numbers into Ka expression and calculate Ka.
BOH ==> B^+ + OH^-
Kb = (B^+)(OH^-)/(BOH)
Look at the ICE chart.
I = initial concn (before ionization):
BOH = 1.4 mols/L.
(B^+) = 0
(OH^-) = 0
C = change in concn:
(B+) = +1.4*0.0063
(OH^-) = +1.4*0.0063
(BOH^-) = 1.4*0.9937 (0.9937 is the fraction from 100%-0.63% = 99.37%)
E = equilibrium concn:
(B^+) = 1.4*0.0063 = ??
(OH^-) = 1.4^0.0063 = ??
(BOH) = 1.4-(1.4*0.0063) OR (1.4*0.9937= ??)
Substitute the equilibrium numbers into Ka expression and calculate Ka.
Related Questions
A weak base with a concentration of 1.3 mol/L has a percent ionization of 0.72%. What is the Kb of t...
A weak base with a concentration of 1.3 mol/L has a percent ionization of 0.72%. What is the Kb of t...
Methylaime, CH3NH2.
If a 0.100 mol/L solution of methyamine has a pH of 11.80, calculate the ioniza...
Aniline, C6H5NH2, is a weak base. If the hydroxide ion concentration of a 0.223 M solution is 9.7 1...