Difference between endpoint and equivalence point

Difference Between Equivalence Point and Endpoint

difference between endpoint and equivalence point

Endpoint and equivalence point are the two most important concepts in chemistry titrations. This article unfolds the key difference between the endpoint and equivalence point in chemical titrations. Equivalence point in acid-base titration signals the completion of the reaction.

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Endpoint and equivalence point are the two most important concepts in chemistry titrations. The technique of titrations can occur in redox reactions, acid-base reactions, and many more reactions. It is predominantly used in acid-base reactions where it involves neutralization of another solution with the other to determine the unknown concentration. Basically, a standard solution with known concentration is carefully poured into another solution called the analyte with unknown concentration to calculate its concentration. During titration process, there are two stages that are reached, viz. Equivalence point, also called stoichiometric point, in a nutshell, is a point where the moles of the two solutions, acid and base, are equivalent or equal.

The equivalence point , or stoichiometric point , of a chemical reaction is the point at which chemically equivalent quantities of reactants have been mixed. In other words, the moles of acid are equivalent to the moles of base, according to the equation this does not necessarily imply a molar ratio of acid:base, merely that the ratio is the same as in the equation. It can be found by means of an indicator, for example phenolphthalein or methyl orange. The endpoint related to, but not the same as the equivalence point refers to the point at which the indicator changes color in a colorimetric titration. From Wikipedia, the free encyclopedia. This article relies largely or entirely on a single source.

Titration measures the concentration of an unknown solution that reacts with a solution of known concentration. The process is often used to check the purity of synthesized chemical compounds, such as pharmaceuticals. The ideal point for the completion of titration is known as the equivalence point. The end point demonstrates the equivalence point, typically by some form of indicator. For example, with a color indicator, the solution changes color when the titration reaches its end point. The completion of a titration is the end point, detected by some type of physical change produced by the solution, such as a color change.

The equivalence point in a titration is the point at which the added titrant is chemically equivalent completely to the analyte in the sample.
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The equivalence point is a chemistry term you'll encounter when you do a titration. However, it technically applies to any acid-base or neutralization reaction. Here's its definition and a look at methods used to identify it. The equivalence point is the point in a titration where the amount of titrant added is enough to completely neutralize the analyte solution. The moles of titrant standard solution equal the moles of the solution with unknown concentration. This is also known as the stoichiometric point because it is where the moles of acid are equal to the amount needed to neutralize the equivalent moles of base. Note this does not necessarily mean the acid to base ratio is

The equivalence point is when the ratio of the reactants is in the amounts specified by the equation. This is not always the case though. If you neutralise a weak base with a strong acid the final solution will not be neutral e. The same problem occurs when a strong base is neutralised by a weak acid. The salt produced is slightly alkaline. You need to choose an indicator which will change colour at the equivalence point. In this case methyl orange is suitable but phenolphthalein is not.

The key difference between equivalence point and endpoint is that the equivalence point in a titration is the point at which the added titrant is chemically equivalent completely to the analyte in the sample whereas the endpoint is the point where the indicator changes its colour. Titration is a technique we use widely in analytical chemistry to determine acids, bases , oxidants, reductants, metal ions and many other species. In a titration, a chemical reaction takes place. Here, an analyte reacts with a standard reagent, which we call as a titrant. We use an indicator in order to detect the endpoint of the reaction. But, it is not the actual point where the chemical reaction terminates.

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Titration methods are often used to identify and quantify the components in a solution mixture. Some titrations are done along with an indicator that is helpful in indicating the end of the chemical reaction.

Acid-base titration curves

If you use an indicator in a titration, the end point is the position at which the indicator changes colour. This may not be the exact point where the reactants have completely reacted but simply shows that a particular pH change has occurred. So if you use this to titrate an alkali and acid and were adding the alkali to the acid, it would turn pink somewhere between these two values. So end point is the point shown by an indicator. Equivalence point is the actual point where the reaction has just been completed and refers to the stoichiometric quantities of reactants eg when 1 mole HCl is added to 1 mole of NaOH.





  1. Fanuel G. says:

    The main difference between an equivalence point and an endpoint is that the former marks the end of the reaction whereas the latter is a point where the.

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