Calculate the pH of 500mL Solution of 1 M BOH (K_(b)=2.5xx10^(-5))
Calculate pH of a resultant solution of 0.1 M HA (K_(a)=10^(-6)) and 0.5 M HB (K_(a)=2xx10^(-6)) at 25^(@)C.
Calculate the pH of 0.1 MNH_(3) solution. K_(b) = 1.8 ** 10^(-5)
% dissociation of a 0.024M solution of a weak acid HA(K_(a)=2xx10^(-3)) is :
The vapour pressur of 0.01molal solution of weak base BOH in water at 20^(@)C is 17.536mm . Calculate K_(b) for base. Aqueous tension at 20^(@)C is 17.540mm . Assume molality and molarity same.
For 10^(-4) M BOH (weak base) , K_(b)=5xx10^(-5)) :
For a solution obtained by mixing equal volumes of 0.02M KOH solution &0.2M B (weak diacidic base), (K_(b_(1))=10^(-7) & K_(b_(2))=10^(-14)) . Find the pH of solution
Calculate the [OH^(-)] in 0.01M aqueous solution of NaOCN(K_(b) for OCN^(-)=10^(-10)) : (a) 10^(-6) M (b) 10^(-7) M (c) 10^(-8) M (d)None of these
pH of a salt solution of weak acid (pK_(a) = 4) & weak base (pK_(b) = 5) at 25^(@)C is :
pOH of a 0.004M aqueous solution of diacidic weak base B (pK_(b_(1))=3.7&pK_(b_(2))=7.3) is:
