`K_(a)` for formic acid and acetic acid are `1.8xx10^(-4)` and `1.8xx10^(-5)` respectively. The relative strength of acids is:

The K_(a) for formic acid and acetic acid are 2.1 xx 10^(-4) and 1.1 xx 10^(-5) , respectively. Calculate relative strength of acids

Dissociation constant (K_a) of formic acid and acetic acid are 2.5xx10^-4 and 0.5xx10^-5 respectively. The ratio of their relative strengths at the same concentration is

At certain temperature, dissociation constant of formic acid and acetic acid are 1.8xx10^(-4) and 1.8xx10^(-5) respectively. At what concentration of acetic solution, the H_3O^(+) ion concentration is same as that in 0.001 M formic acid solution

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 m-nitrobenzoic acid and acetic acid are 36.0× 10^(−5) and 1.8× 10^(−5) respectively. What are their relative strengths?

Conversion of Formic acid into acetic acid

The dissociation constants for HCOOH " and " CH_(3)COOH " are " 2.1 xx 10^(-4) " and " 1.8 xx 10^(-5) respectively. Calculate the relative strengths of the acids .

The first and second dissociation constants of an acid H_(2)A are 1.0xx10^(-5) and 5.0xx10^(-10) respectively. The overall dissociation constant of the acids wil be:

The dessociation cosntants of acetic acid and propionic acid are 1.0 xx 10^(-5) and 1.0 xx 10^(-6) respectively. The value of P^(K_(a)) (propionic acid) - P^(K_(a)) (Acetic acid) is

The K_(a) for CH_(3)COOH at 300 and 310 K are 1.8 xx 10^(-5) and 1.805 xx 10^(-5) , respectively. The enthalpy of deprotonation for acetic acid is 51.6 cal .