Calculate the ratio of sodium formate and formic acid `(K_(a)=2xx10^(-4))` in a buffer solution of pH=4.3.

The ionization constant of formic acid is 1.8xx10^(-4) . Around what pH will its mixture with sodium formed give buffer solution of higher capacity. Calculate the ratio of sodium formate and formic acid in a buffer of pH 4.25 .

The ionization constant of formic acid is 1.8xx10^(-4) . Around what pH will its mixture with sodium formed give buffer solution of higher capacity. Calculate the ratio of sodium formate and formic acid in a buffer of pH 4.25 .

Calculate the pH of 0.2M sodium butyrate, (K_(a) for butyric acid is 2.0xx10^(-5))

50% neutralisation of a solution of formic acid (k_(a)=2xx10^(-4)) with NaOH would result in a solution having a hydrogen ion concentration of :

The pH of blood is 7,4 . If the buffer in blood constitute CO_(2) and HCO_(3)^(Theta) ions, calculate the ratio of conjugate base of acid (H_(2)CO_(3)) to maintain the pH of blood. Given K_(1) of H_(2)CO_(3) = 4.5 xx 10^(-7) .

The pH of 0.5 M aqueous solution of HF (K_(a)=2xx10^(-4)) is

What volume of 0.10 M sodium formate solution should be added to 50 mL of 0.05 M formic acid to produce a buffer solution of pH = 4.0 ? pK_a for formic acid = 3.80?

Calculate the concentration of the formate ion present in 0.100 M formic acid (HCOOH) solution at equilibrium (K_(a) = 1.7xx10^(-4)) .

Calculate the the ratio of conjugate base// weak acid required to prepare an aqueous solution of benzoic acid and sodium benzoate with pH of 4.5 . The acid dissociation constant of benzoic acid is 6.5 xx 10^(-5) .

The concentration of hydrogen ions in a 0.2M solution of formic acid is 6.4 xx 10^(-3) mol L^(-1) . To this solution, sodium formate is added so as to adjust the concentration of sodium formate to 1 mol L^(-1) . What will be the pH of this solution? The dissociation constant of formic acid is 2.4 xx 10^(-4) and the degree of dissociation fo sodium formate is 0.75 .