An indicator has `pK_(In)=5.3`. In a certain titration, this indicator is found to be `80%` ionized in its acid form. Thus, `pH` of the solution is

An indicator has pk_in = 5.3 . In a certain solution, this indicator is found to be 80% in its acid from. What is the pH of the solution ?

An acid base indicator has K_(a)=1.0xx10^(-5) the acid form of the indicator is red and the bais form is blue. Calculate the pH change required to change the colour of the indicator from 80% red to 80% blue.

A Certain monoprotic acid (weak) serves as indicator . Assuming that colour change is seen when 1//3^(rd) of the indicator has been converted to ions and that at end point the pH of solution is 6 , what is the value of pK_(In) ?

A Certain monoprotic acid (weak) serves as indicator . Assuming that colour change is seen when 1//3^(rd) of the indicator has been converted to ions and that at end point the pH of solution is 6 , what is the value of pK_(In) ?

What fraction of an indicator H"in" is in the basic form at a pH of 6 if pK_(a) of the indicator is 5 ?

What fraction of an indicator Hi n is the basic form at a pH of 5 if the pK_(a) of the indicator is 6 ?

What fraction of an indicator H"in" is in the basic form at a pH of 6 if pK_(a) of the indicator is 5 ?

At pH=2 half of the indicator thylmol blue ( an acid type indicator)is in unionised form,find the % of indicator in unionised form in the solution with [H^(+)]=4xx10^(-3)M

An acid base indicator has K_(a)=1.0xx10^(-5) the acid form of the indicator is red and the basic form is blue. Calculate the pH change required to change the colour of the indicator from 80% red to 80% blue.