An acid-base indicator has a `K_(a)` of `3.0 xx 10^(-5)`. The acid form of the indicator is red and the basic form is blue. (a) By how much must the `pH` change in order to change the indicator from `75%` red to `75%` blue?
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
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
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 .
An acid base indicator (K_(a) =10^(-5)) has its pH range 4.4 - 6.0. The correct statement (s) amongst the following is/are
The K, of an indicator HIn is 9 x 10^(4) , The percentage of the basic form of indicator is 10x in a solution of pH = 4. What is x ?
An acidic indicator ionises as I_(n) H hArr "In"^(-) + H^(+) . The molecular and ions of the indicator show different colours. The indicator changed it colour if its acidic of basic form completely predominant. Dissociation constant of an acidic indicator is 10^(-5) . At what p^(H) 80% of the indicator exists in molecular form ?
An acidic indicator ionises as I_(n) H hArr "In"^(-) + H^(+) . The molecular and ions of the indicator show different colours. The indicator changed it colour if its acidic of basic form completely predominant. An indicator with P^(Kin) = 5 is added to a solution with p^(H) = 5 . What is the percentage of acidic form of the indicator
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
