What is the degree of dissociation of weak acid HA (C=0.1 M) in presence of strong acid HB (C=0.1 M) ? Given :`K_a`=(weak acid)=`10^(-6)`

The degree of dissociation of a 0.01 M weak acid is 10^(-3) . Its pOH is

If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :

If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :

If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :

The dissociation constant of weak acid HA is 1 xx 10^(-5) . Its concentration is 0.1 M . pH of that solution is

The degree of dissociation of a weak monoprotic acid of concentration 1.2xx10^(-3)"M having "K_(a)=1.0xx10^(-4 is

The degree of dissociation of a weak monoprotic acid of concentration 1.2xx10^(-3)"M having "K_(a)=1.0xx10^(-4 is

The dissociation constant of a weak acid HA is 1.2 xx 10 ^(-10) Calculate its pH in a 0.1 M solutions

The degree of dissociation of 0.1 M weak acid is 10^(-2) and the degree of dissociation of the same acid in 0.025M concentration is '*', then find 100x. __________ ?