Dissociation constants of two acids `HA` and `HB` are respectively `4xx10^(-10)` and `1.8xx10^(-5)`, whose `pH` value will be higher for a given molarity:

Dissociation constant of two acids HA & HB are respectively 4xx10^(-10) & 1/8 xx10^(-5) M whose pH value will be higher

The dissociation constant of two acids HA_(1) and HA_(2) are 4.5 xx 10^(-4) and 1.8 xx 10^(-5) respectively. If both are having equal concentrations the relative strength of acids is

The dissociation constants of two acid HA_1 and HA_2 are 2.9xx10^(-4) and 1.8xx10^(-5) respectively The relative strengths of the acid will be :

The dissociation constants of two acids HA_(1) and HA_(2) are 3.0xx10^(-4) and 1.8xx10^(-5) respectively. The relative strengths of the acids will be approximately

The dissociation constants of two acids HA_(1) and HA_(2) are 3.0xx10^(-4) and 1.8xx10^(-5) respectively. The relative strengths of the acids will be approximately

The dissociation constant of two acids HA_1 and HA_2 are 3.0xx10^-4 and 1.8xx10^-5 respectively. The relative strengths of the acids is

The dissociation constant of two acids HA_(1) " and " HA_(2) are 3.14 xx 10^(-4) " and " 1.96 xx 10^(-5) respectively . The relative strength of the acids will be approximately

The acidic strength of two monobasic acids may be compared by comparing the hydronium ion concentrations of their aqueous solution of same molar concentration. The dissociation constants of acids HA and HB are 4 xx 10^(-6) and 2.5 xx 10^(-9) , respectively. How many times HA is stronger than HB ? Assume that for both the acids, the degree of dissociation at the concentration take, is negligible.