i At what `pH` will the mixture of `HCOOH` and `HCOONa` given buffer solution of higher capacity?
ii Calculate the ratio of `([HCOONa])/([HCOOH])` in a buffer of `pH 4.25. (K_(a)` of `HCOOH = 1.8 xx 10^(-4))`

i At what pH will the mixture of HCOOH and HCOONa given buffer solution of higher capacity? (K_(a) of HCOOH = 1.8 xx 10^(-4))

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 .

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 ratio of [HXOO^(-)] and [F^(-)] in a mixture of 0.2 M HCOOH (K_(a)=2xx10^(-4)) and 0.1 M HF (K_(a)=6.6xx10^(-4)) :

Calculate the ratio of [HXOO^(-)] and [F^(-)] in a mixture of 0.2 M HCOOH (K_(a)=2xx10^(-4)) and 0.1 M HF (K_(a)=6.6xx10^(-4)) :

Calculate solubility of AgCN (K_(sp)= 4 xx 10^(-16)) in a buffer solution of PH=3. [(K_a)_(HCN)= 4 xx 10^(-10)] .

How many moles of HCOONa must be added to 1L of a 0.1 M solution of HCOOH in order to prepare a buffer solution of pH = 3.4? (Given : K_(a) of HCOOH =2 times 10^(-4) at 298 K)