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There are four main types of titrations. Titration is an essential process in a chemistry laboratory. It is used to determine the concentration of an unknown solution against a solution with a known concentration. Titration is also known as volumetric analysis or titrimetry. It uses a quantitative analytical method. Titrations are carried out by preparing a standard solution termed titrant, whose concentration and volume are known. The titrant is filled in a burette which is clamped. The unknown solution whose concentration is to be determined is kept below the clamped burette in a conical flask; it is referred to as an analyte or a titrant. The titrant is released dropwise into the titrant with which it reacts until exact chemical equivalence is achieved.
The quantity of titrant utilised for chemical equivalence is then noted and this measure is used to calculate the concentration of the unknown solution using the basic formula.
\begin{equation}
\mathrm{N}_1 \mathrm{~V}_1=\mathrm{N}_2 \mathrm{~V}_2
\end{equation}
Titration is the process of using the stoichiometry principle to calculate the concentration of an unknown solution.
In a beaker or an Erlenmeyer flask, a very exact amount of the analyte is added
Preparing a titrant/titrator, which is a standard solution with a set volume and concentration, is a necessary step in the titration process.
This titrant is then made to react with the analyte until an endpoint or equivalence point is achieved.
At this point, the concentration of the analyte can be calculated by measuring the titrant used.
When the amount of titrant and titrate become equal to one another, the point of equivalence is addressed.
As mentioned earlier there are 4 main types of titration. They are:
Acid-base titration
Redox titration
Precipitation titration
Complexometric titration
Acid-base titrations primarily rely on the solution-based neutralisation of an acid and a base. More importantly, a standard base solution is used to evaluate an acid's potency. Another name for this procedure is acidimetry.
Strong and weak acids can be distinguished based on how much dissociation produces
H+ ions when an acid is dissolved in water. If a known quantity of acid is titrated against a powerful base, the acid concentration can be determined by taking into account that the neutralisation reaction has finished. For the same reason, the titration procedure only employs a strong base. Thus, in this instance, the strong base is the titrant, also known as the standard solution, while the acid solution is the titrate.
The Procedure is As Follows:
Using a pipette, the necessary volume of the base with the predetermined concentration is taken, and it is then added to the titrating flask.
In the Burette, the unknown acid concentration is added, and the base is then allowed to react with the acid drop by drop.
An indication for determining the endpoint is also included in the titration flask.
Due to the presence of the indicator, the colour of the solution in the titration flask changes when the reaction is complete.
Phenolphthalein, an indicator that turns pink in basic solution and is colourless in acid and neutral solution, can be used for this purpose.
It is challenging to detect or obtain the endpoint when the acid is very weak. Because the conjugate base of a weak acid is a strong base, the weak acid's salt is titrated against a strong acid for this purpose.
As an illustration, CH3COOH is a weak acid. However, CH3COONa is a solid foundation. HNO3, HCl, H2SO4, and HClO3 are examples of strong acids.
bases might be either strong or weak. The procedure is the same as in the case of acid titration, with the exception that the base is an unknown solution (titrate), and the titrant is a potent acid. Methyl orange or methyl red indicators, which are orange in acidic solutions and yellow in basic and neutral solutions, can be utilised in this situation.
A redox reaction between the analyte and titrant is the basis of a redox titration. A potentiometer and/or a redox indicator may be used in this process.
A typical illustration of a redox titration is the production of iodide by treating an iodine solution with a reducing agent while employing a starch indicator to help identify the endpoint.
When all the iodine is used up, the blue colour vanishes because iodine (I2) can be converted to iodide (I), for example, by the action of thiosulfate. Iodometric titration is the term used for this.
Most frequently, the reduction of iodine to iodide occurs as the final step in a chain of events where the previous reactions are utilised to change an unknown quantity of the solute (the chemical being examined) into an equivalent quantity of iodine, which may then be titrated.
In the intermediate reactions, additional halogens (or haloalkanes) besides iodine are occasionally utilised because they are more readily obtainable in better-measured standard solutions and/or react with the solute more quickly.
The equivalence point, where the blue turns a little bit colourless, is more distinct in iodometric titration than it is in certain other analytical or maybe by volumetric methods, thus the extra steps may be justified.
precipitation titration involves the production of precipitate while using the titration method. In a precipitation titration, the analyte and titrant combine to generate a precipitate, which is an insoluble material. It continues until all of the analytes have been consumed. Silver ions are utilised to quantify chloride using this method.
The Precipitation Titration Principle
The following examples illustrate the precipitation titration principle:
The quantity of precipitating agent added equals the amount of substance precipitating
Essentially 3 types of precipitation titration are followed.
Precipitation titration has various uses, including the following:
The halide ions are found via precipitation titration.
Salt content in different foods and beverages is measured via precipitation titration.
Different medicines are analysed using precipitation titration.
The concentration of the anion in the analyte is determined via precipitation titration.
Complexometric titration is a volumetric analysis in which the creation of a coloured complex identifies the endpoint of the analysis or titration. It is most helpful for figuring out a mixture of several metal ions in a solution.
Additionally called chelatometry. This kind of titration uses an indicator that can produce a distinct colour change that shows when the titration has reached its endpoint.
The concentration of metal ions in the solution is determined using complexometric titrations. It is a volumetric analysis because, during titration, the volume of the analyte, titrant, and even indicator is crucial. For the complexometric titration, indicators like calcein and Eeriochrome black T are utilised, among others.
The amount of total hardness in water is estimated via complexometric titration.
To determine the metal content in medicines, it is commonly employed in the pharmaceutical business.
Many cosmetic items contain titanium dioxide. Complexometric titration can be used to analyse this.
Urine sample analysis is done using it.
It has many applications in analytical chemistry.
Titration is a very useful laboratory technique. Although recent advances in analytical techniques have taken place which involves the use of various spectroscopic methods for the detection of unknown substances. UV spectroscopy, NMR, IR, and mass spectroscopy are to name a few. Titrations are mainly used in food industries and pharmaceutical manufacturing for the determination of the molar concentration of reactants.
As per latest 2024 syllabus. Physics formulas, equations, & laws of class 11 & 12th chapters
As per latest 2024 syllabus. Chemistry formulas, equations, & laws of class 11 & 12th chapters
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