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 :

50% neutralisation of a solution of formic acid ( K_a=2xx106(-4) ) with NaOH would result in a solution having a hydrogen ion concentration of :

What is the pH of a 0.05 M solution of formic acid? (K_(a)=1.8xx10^(-4))

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

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

Hydrogen ion concentration of an aqueous solution is 1 xx 10^(-4)M . The solution is diluted with equal volume of water. Hydroxyl ion concentration of the resultant solution in terms of mol dm^(-3) is

In a solution of formic acid (K_a=1.7xx10^(-4)) , the [H^+] =2.3xx10^(-3) .What is the concentration of formic acid in mol L^(-1) ?

Two solutions A and B have pH values of 4 and 10, respectively. Which solution has more hydrogen ion concentration?