Complexometric titration

Titration is a method of determining the concentration of a solution by adding a known volume of one solution to an unknown volume of another solution until the reaction is complete.

In actuality, titration is a process for determining the concentration of an unknown solution. It’s because of this that it’s known as quantitative analysis. Let’s take a closer look at the different sorts of titration.

Titration is a technique in which an analyte and a titrant are used. A calibrated concentration of titrant is added to an unknown quantity of analyte to determine the endpoint of titration for analysis, and when the endpoint is reached, the moles of titrant and analyte will be identical.

Titration

Titration is the technique of determining the concentration of a solution by calculating the volumes of reacting solutions required at the corresponding point of reaction. It’s a method of determining the concentration of an unknown solution by comparing it to a solution of known concentration.

Titration is a chemical method of estimating the amount of a constituent in a sample by combining the measured sample with an accurately known quantity of another substance in which the desired element reacts in a certain proportion.

Endpoint of Titration

At the equivalence point of a titration, an absolutely equivalent amount of titrant has been added to the sample. The endpoint is the point in the experiment when a signal identifies the reaction as complete. This signal could be represented by a change in the colour of an indicator or a change in an electrical property detected during the titration.

The titration error is the difference between the endpoint and its equivalence point, which can be decreased by selecting an appropriate end-point signal and detecting it. After understanding the nature of the titration process, the indicator for the coincidence should be carefully picked. When the indicator colour changes, the titration is finished.

Using the known concentration of the titrant and the endpoint as an approximation of the equivalence point, the endpoint is used to calculate the amount or concentration of the analyte.

Types of Titration

When it comes to processes and goals, titration can be divided into various categories. The most popular types of titration in quantitative chemical analysis are redox titration and acid-base titration. The types of titration are listed below.

• Acid Base Titration
• Complexometric Titration
• Precipitation Titration
• Redox Titration

Complexometric Titration

In complexometric titrations, a metal-ligand complexation reaction is used. Complexometric titrations are based on the formation of a complex between the analyte and the titrant.

The chelating substance EDTA is commonly used to titrate metal ions in solution. Take, for example, EDTA titrations. In analytical chemistry, EDTA (Ethylenediaminetetraacetic acid) is one of the most often used chelating agents for complexometric titrations.

Precipitation Titration

Certain analytes, such as  Cl-can be determined by titration with precipitating agents, which can be detected when titrated with AgNO3. Potassium chromate is a titration indicator for precipitation. The development of a coloured secondary precipitate is a direct titration endpoint (K2 CrO4). When silver nitrate is put into a solution of ammonium thiocyanate or sodium chloride, for example, it reacts to form white silver thiocyanate or silver chloride.

Redox Titration

Redox titration is a term for an oxidation-reduction process. When electrons are transported between reactive ions in aqueous solutions, the chemical reaction happens in this type of titration. The titration between oxalic acid solution and acidified KMnO4 The solution is a redox titration because the reaction is a redox reaction. In redox titration, the redox indicator is the indicator used.

Acid Base Titration

When an acidic or basic titrant reacts with a base or acid analyte, it is known as an acid-base titration. It’s an analytical method for estimating the concentration of an acid or base by precisely neutralising it with a known concentration standard solution of the same acid or base. A pH indicator is used to keep track of how the acid-base interaction is proceeding.

The colour indication is used to detect the equivalent point of an acid-base reaction in titration, and the acid-base indicator is also known as a pH indicator. Phenolphthalein and methyl-orange are two of the most used pH indicators.

Procedure of Acid Base Titration

• Rinse the burette with the standard solution, the pipette with the unknown solution, and the conical flask with distilled water.
• Transfer an accurately measured volume of the analyte, as well as a few drops of indicator, to the Erlenmeyer flask using the pipette. Fill the burette halfway with the standardised solution and write the volume down on a worksheet. At this point, we need a good estimate of how much known solution is needed to neutralise the unknown solution. Allow the solution in the burette to drain until the indicator changes colour, then record the value. This is the first titration, which isn’t particularly precise and should be excluded from any computations.
• Carry out at least three more titrations, this time more precisely, keeping in mind the endpoint’s approximate location. Record the initial and final readings on the burette before starting the titration and at the end.
• The endpoint is reached when the indicator changes colour permanently.

Conclusion

Titration is a method of determining the concentration of a solution by adding a known volume of one solution to an unknown volume of another solution until the reaction is complete.

At the equivalence point of a titration, an absolutely equivalent amount of titrant has been added to the sample. The endpoint is the point in the experiment when a signal identifies the reaction as complete.

The types of titration are listed below.

• Acid Base Titration
• Complexometric Titration
• Precipitation Titration
• Redox Titration