Ionic EquilibriumHard
Question
Let the colour of the indicator HIn (colourless) will be visible only when its ionised form (pink) is 25% or more in a solution. Suppose HIn (pKa = 9.0) is added to a solution of pH = 9.6 predict what will happen. (Take log 2 = 0.3)
Options
A.pink colour will be visible
B.pink colour will not be visible
C.% of ionised form will be less than 25%
D.% of ionised form will be more than 25%
Solution
HIn → H+ + In-
KIn =
⇒ 
= 100.6 = 4
∴ % of [In-] in solution =
× 100 = 80%
so pink colour will be visible.
KIn =
⇒ = 100.6 = 4∴ % of [In-] in solution =
× 100 = 80%so pink colour will be visible.
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Ammonia forms the complex ion [Cu(NH3)4]2+ with copper ions in alkaline solutions but not in acidic solutions. What is t...Among the following acids which has the lowest pKa value?...When excess oxalic acid is added to CaCl2 solution, CaC2O4 is precipitated and the solution still contains some unprecip...Which of the following relation(s) is/are true for alkaline solution?...The equilibrium carbonate ion concentration after equal volumes of 0.7 M-Na2CO3 and 0.7 M-HCl solutions are mixed, is (K...