The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solutions is found to be 10% If the molarity of the solution is 0.05M , the percentage hydrolysis of the salt should be :
Nature of aqueous solution of salts formed by weak acid and weak base is
The degree of dissociation of an acid HA in 0.1 M solution is 0.1%. Its dissociation constant is
Density of a 2.05 M solution of acetic acid in waer is 1.02 gas ml^(-1) . The molarity of the solution si
A weak acid HX has the dissociation constant 1xx 10 ^(-5) M.It forms a salt NaX on reactions with alkali. The percentage hydrolysis of 0.1 M solution of NaX is :
Hydrolysis constant of salt derived from strong acid and weak base is 2xx 10 ^(-5) .The dissociation constant of the weak base is
A monoprotic acid in a 0.1 M solution ionizes to 0.001 % . Its ionization constant is
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
A weak base BOH is tirated against 0.1 M of HCl solution. The following table indicates the volumes of HCl added and pH of solution. From this data the pK_b of base may be.
1.0 M solution of which of the following salts is most basic ?
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
