An acid-base indicator which is a weak acid has a pH value =5.45. At what concentration ratio of sodium acetate to acctic acid would the indicator show a colour half-way between those of its acid and conjugate base forms ? `[pK_(a)` of acetic acid =4.75, log 2=0.3]
In an acidic buffer solution (pH = 4.4) , the concentration ratio of acid and salt is 2 :1 . The value of dissociation constant of weak acid may be
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
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
50 mL of 0 . 02 M Na OH solution is mixed 50 mL of 0 . 6 M acetic acid solution, the pH of resulting solution is ( pK_(a) pf acetic acid is 4 . 76, log 5 = 0 . 70 )
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 ?
It has been found that the pH of a 0.01M soluiton of an organic acid is 4.15 . Calculate the concentration of the anion, the ionization constant of the acid and its pK_(a) .
A buffer solution is prepared by mixing 10 mL of 1.0 M acetic acid and 20 mL of 0.5 M sodium acetate and then diluted to 100 mL with distilled water, The pH of the buffer solution is ( pK_(a) of acetic acid is 4.76 )
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
