The concentration of `H^(+)` ion in a `0.2 M` solution of `HCOOH` is `6.4xx10^(-3) "mole" L^(-1)`. To this solution `HCOONa` is added so as to adjust the concentration of `HCOONa` to one mole per litre. What will be the `pH` of this solution? `K_(a)` for `HCOOH` is `2.4xx10^(-4)` and the degree of dissociation of `HCOONa` is `0.75`

The [H^(+)] in 0.2M solution of formic acid is 6.4xx10^(-3) mol litre^(-1) . To this solution formate is added so as to adjusrt the conc.of sodium formate to one mol per litre. What will be pH of this solution ? (K_(a) for HCOOH=2.4xx10^(-4)) and degree of dissociation of HCOONa = 0.75 )

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 .

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 .

What concentration of HCOO^(-) is present in a solution of weak of 0.01 M HCOOH (K_(a)=1.8xx10^(-4) and 0.01 M HCl?

What concentration of HCOO^(-) is present in a solution of weak of 0.01 M HCOOH (K_(a)=1.8xx10^(-4) and 0.01 M HCl?

What concentration of HCOO^(-) is present in a solution of weak of 0.01 M HCOOH (K_(a)=1.8xx10^(-4) and 0.01 M HCl?