An acid base indicator has `K_(HIn)=3.0xx10^(-5)`. The acid from of the indicator is red and the basic form is blue the change in `(H^(+))` required to change the indicator from 75% red to 75%blue is :-

An acid-base indicator has K_(a) = 3.0 xx 10^(-5) . The acid form of the indicator is red and the basic form is blue. Then:

An acid-base indicator has a K_(a) = 3.0 xx 10^(-5) . The acid form of the indicator is red and the basic form is blue. Then

An acid-base indicator has K_(a) = 3.0 xx 10^(-5) . The acid form of the indicator is red and the basic form is blue. Then:

An acid-base indicator has a K_(a) = 3.0 xx 10^(-5) . The acid form of the indicator is red and the basic form is blue. Then

An acid -base indicator has a Ka of 3.0 xx 10^(-5) The acid form of the indicator is red and the basic form is blue. Then

An acid base indicator has K_a of 3xx10^-5 . The acid form of the indicator is red and the basic form is blue. By how much must the pH change in order to change the indicator from 75% red to 75 % blue?

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.