Indicators are weak acids whose two forms wear different colours - the ratio flips with pH, and the colour flips with it. Choosing the right one is about matching its transition range to your titration's equivalence point. This is the real knowscape from knowhere, not a picture of one. Drag it. Watch what actually changes.
An acid and base don't just meet — they trade protons, and whoever accepts becomes the new proton-holder ready to give it back. Indicators are just molecules that change colour when they win or lose that proton, and neutralisation is the trade run to completion. Every question here is asking: where did the proton go, and what did that cost the pH?
Acid-base indicators are weak acids that exist in two differently coloured forms, with the ratio between them determined by pH, and their effective transition range should match the vertical section of a titration curve.
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