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Let the colour of the indicator Hin (col...

Let the colour of the indicator Hin (coloueless) will be visible only when its ionised form (pink) is `25%` or more in a solution. Suppose Hin `(pK_(a)=9.0)` is added to a solution of pH=9.6 predict what will happen? (Take log `2=0.3`)

A

pink colour will be visible

B

pink colour will not be visible.

C

`%` of ionised form will be less then `25%`

D

`%` of ionised form will be more in `25%`

Text Solution

AI Generated Solution

To solve the problem, we need to analyze the dissociation of the indicator \( \text{HIn} \) and how it relates to the pH of the solution. Here’s a step-by-step solution: ### Step 1: Understand the dissociation of the indicator The indicator \( \text{HIn} \) dissociates as follows: \[ \text{HIn} \rightleftharpoons \text{H}^+ + \text{In}^- \] Where \( \text{HIn} \) is the non-ionized (colorless) form and \( \text{In}^- \) is the ionized (pink) form. ...
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