The concentration of fluroacetic acid `(K_(a)of acid =2.6xx10^(-3))`, which is required to get `[H^(+)]=1.50xx10^(-3)M` is:

What is the concentration of fluoracetic acid ( K_a of acid = 2.6xx10^(-3)) Which is required to get [H^+] = 1.50xx10^(-3) M ?

The concentration of acetic acid (K_(a)=1.8 xx 10^(-5)) required to give 3.5 xx 10^(-4) moles // litres of H_(3)O^(+) ions is

What concentration of FCH_(2)COOH (K_(a)=2.6xx10^(-3)) is needed so that [H^(+)] =2xx10^(-3) ?

What concentration of FCH_(2)COOH (K_(a)=2.6xx10^(-3)) is needed so that [H^(+)]=2xx10^(-3) ?

What concentration of FCH_(2)COOH (K_(a)=2.6xx10^(-3)) is needed so that [H^(+)] =2xx10^(-3) ?

Calculate the [CH_(2)FCOOH] (fluoroacetic acid) which is required to get [H^(o+)] = 1.5 xx 10^(-3)M. K_(a) of acid =2.6 xx 10^(-3) .

Calculate the [CH_(2)FCOOH] (fluoroacetic acid) which is required to get [H^(o+)] = 1.5 xx 10^(-3)M. K_(a) of acid =2.6 xx 10^(-3) .

The concentration of acetic acid required to get 3.5 xx 10^(-4) mole/lit of H^(+) ion is [K_(a) = 1.8 xx 10^(-5) ]

What concentration of dichloroacetic acid gives [H^(+)]=8.5xx10^(-3)M ? ("Given": K_(a)"of acid" = 5.0xx10^(-2)) .

How many times the proton concentration of formic acid (K_a = 2.1 xx 10^4) is greater than that of propionic acid (K_a=1.1 xx 10^(-5) ), if the molar concentrations of both acids are same?