Acid Base Titration Essay

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Title:
Acid base titration –Define the end point by using various indicators
Aim:
To define the end point of an acid-base titration effect by using various indicators.
Introduction:
The titration is a scientific method applied to define the specific amount of a substance by the substance with a known amount of another substance. The completed reaction of a titration is normally shown by the colour change or an electrical measurement.
The elements needed to be applied in a titration as a standard amount of the material present is precisely identified. The standard can be present both in the form of a pure substance or standard solution which solution whose composition is precisely identified. The standard can be equipped in two ways, primary standard or standardize by titration against some previously standardized solution. A primary standard
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Within the acid-base titration process, the molarity of antacid A, B and C can be found. The molarity of antacid A is 0.107 M, antacid B is 0.054 M and antacid C is 0.083 M
The reaction in the acid-base titrations is neutralization. During the neutralization, an acid and base react to produce salt and water. For example is when hydrogen ion (H+) reacts with hydroxyl ion (OH-) produce water (H2O). Since the reactants are colourless, a suitable indicator should be used to indicate the colour change at the end point.
The equivalence point can be determined through titration by adding minimum amounts of a substance (indicator). The colour will change when the equivalence point reached the solution. When a strong base is titrated with a strong acid or vice versa the pH of the solution will be about 7.0 at the equivalence point. The indicator used in this experiment is phenolphthalein. Phenolphthalein turned pink in alkaline solutions and colourless in acidic

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