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)`.

CM fluorcacetic acid solution was found to contain [H^(+)]=1.5xx10^(-3)M.K_(a) of fluroacetic acid = 2.5xx10^(-3) .Then : value of C

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)) .

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 ?

Calculate the pH at which an acid indicator with K_(a), = 1.0 xx 10^(-5) changes colour when the indicator concentration is 1.0 xx 10^(-3) M

Glycine [NH_(2)CH_(2)COOH) is basic and acidic due to presence of -NH_(2) and -COOH group. It acquires a H^(o+) to form overset(o+)NH_(3)COOH , which is a diprotic acid with K_(1) = 4.5 5 xx10^(-3) and K_(2) = 1.7 xx 10^(-10) . In a 0.01M solution of neutral glycine, a. What is the pH and b. What percent of the glycine is in the cationic form at equilibrium?

Calculate the pH at which an acid indicator with K_a =1.0 xx 10^(-5) changes colour when the indicator concentration is 1.0 xx 10^(-3) M .