In the calculations it was assumed that: a. Before any acetic acid was added, essentially all the indicator was in the In-form.
b. After the HCl was added, essentially all the indicator was in the HIn form.

Required:
Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine:

1. The fraction of the indicator in the HIn form in solution B before any of solution A was added.
2. The fraction of the indicator in the In- form after the HCl was added.

Following are the responses to the given points:

Explanation:

Form the above-given question, it indicates that the bromate ion green ionizes in water to form a green-blue solution, therefore the before adding the HCL it indicator was in anionic from hence it is written as In^{-} therefore the HCL is mixed which the anion is protonated to give HIN

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