A weak base, `B`, has basicity constant `K_(b)=2xx10^(-5)`. The `pH` of any solution in which `[B]=[BH^(+)]` is

Calcuate the degree of ionisation and pH of 0.05 M solution of a weak base having the ionization constant (K_(b)) is 1.77xx10^(-5). Also calculate the ionisation constant of the conjugate acid of this base.

Calcuate the degree of ionisation and pH of 0.05 M solution of a weak base having the ionization constant (K_(b)) is 1.77xx10^(-5). Also calculate the ionisation constnat of the conjugate acid of this base.

Calcuate the degree of ionisation and pH of 0.05 M solution of a weak base having the ionization constant (K_(b)) is 1.77xx10^(-5). Also calculate the ionisation constnat of the conjugate acid of this base.

For 10^(-4) M BOH (weak base) , K_(b)=5xx10^(-5)) :

For 10^(-4) M BOH (weak base) , K_(b)=5xx10^(-5)) :

A solution contains equimolar concentration of a weak acid HA and its conjugate base A^(-) , p K_(b) of A^(-) is 9 . The pH of the solution is

For a weak base BOH,K_(b)=10^(-4) .Calculate pH of 10^(-4)BOH solution. (Take log6.2=0.79)

For a weak base BOH,K_(b)=10^(-4) .Calculate pH of 10^(-4)BOH solution. (Take log6.2=0.79)

A solution contains equimolar concentration of a weak acid HA and its conjugate base A^(-) . pK_(b) of A^(-) is "9." The pH of the solution is

K_(a) for a weak monobasic acid is 1.0xx10^(-6) . The pK_(b) of its conjugate base base is