Kb=[HCn][OH-]
[CN-]
Kb=[HCN][OH-]/[CN-]
The Kb value for CH3NH2(aq) is 4.4 x 10^-4.
Kb=[(Ch3)3 NH+][OH-] __________ [(Ch3)3 N]
kb=[C5H5NH+][OH-]______[C5H5N]
ka=[H+][CN-]/[HCN]
Kb=[HCN][OH-]/[CN-]
Kb = [CH3NH3 +] [OH-] / [CH3NH2]
The Kb value for CH3NH2(aq) is 4.4 x 10^-4.
Kb=[(Ch3)3 NH+][OH-] __________ [(Ch3)3 N]
ka=[H+][CN-]/[HCN]
kb=[C5H5NH+][OH-]______[C5H5N]
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
The Kb for C5H5N (pyridine) is 1.7 x 10^-9. This value indicates the strength of the base in solution, with lower values suggesting a weaker base and higher values indicating a stronger base.
Overall ionic equation: K+(aq) +OH-(aq)+ H30+(aq) + Cl-(aq)------>2H20 (l) + K+(aq) + Cl-(aq) Net ionic Equation OH-(aq)+ H30+(aq) ------>2H20 (l)
NH4OH + HC2H3O2 ---> NH4C2H3O2 + H2ONH4+ + OH- + H+ + C2H3O2- ---> NH4+ + C2H3O2- + H2OOH- (aq) + H+ (aq)---> H2O (l)
The Kb for (CH3)3N (trimethylamine) in water is a measure of the strength of the base (CH3)3NH in solution. It is used to calculate the equilibrium concentration of hydroxide ions (OH-) in solution when the base dissociates.
Kb=c5h5nh+oh- / c5h5n (apex.)