Question

How‌ ‌to‌ ‌choose‌ ‌an‌ ‌indicator‌ ‌for‌ ‌an‌ ‌acid‌ ‌base‌ ‌titration?‌ ‌

Answer 1

Hint: An acid-base titration is a laboratory method for determining the composition of a solution containing an acid or a base. The acid-base indicator is often an organic molecule that is a weak acid or basic, comparable to the compounds that give flowers their color.

Complete answer:
The solution contained in the flask includes an unknown quantity of base equivalents (or acid). The burette is calibrated to the closest 0.001 in volume. It is filled with a known concentration of strong acid (or base). From the burette, little amounts are applied until one drop permanently alters the indication color. (A sign that the equivalence point is approaching is the emergence, and then disappearance, of the hue that the indicator adopts beyond neutralization.) The entire quantity of acid (or base) is determined at the equivalence point using burette measurements. At the equivalence point, the number of equivalents of acid and base must be identical.
Alkalimetry, or alkalimetry, is the specific analytic application of acid-base titration to estimate the concentration of a basic (alkaline) material; acidimetry, or acidimetry, is the application of the same idea to an acidic substance.
Titration Materials
-burette
-white ceramic tile (used to see a color change in the solution)
-pipette
-pH meter (the type depends on the reactants)
-Conical flask or Erlenmeyer flask
-recalcitrant (a standard solution of known concentration; a common example is aqueous sodium carbonate)
-titrant, or analyte (the solution of unknown concentration)
The most frequently used acid-base indicators are as follows:
Phenolphthalein - Phenolphthalein is a colorless /(acid) and pink dye (alkali)
Methyl orange – Pink (acid) and yellow (alkali)

Note:
Several commonly used equivalence point markers include the following:
Titration of strong acids and bases using the phenolphthalein indicator.
Titration of weak acids and bases using bromothymol blue as an indication.
Titration between strong acid and mild base: methyl orange indicator the base is excessively basic $(pH > 13.5)$, whereas the acid is too acidic $(pH > 5.5)$: yellow alizarin indication.
The base is excessively basic $(pH > 13.5)$, whereas the acid is too acidic $(pH > 5.5)$: yellow alizarin indication.
The base is excessively basic $(pH > 13.5)$, whereas the acid is too acidic $(pH > 5.5)$: yellow alizarin indication.
The acid is at the bottom of the pH scale (e.g., pH 0.5) and the base is at the top (pH 8.5): indication of thymol blue.