Hydrochloric Acid In Chemistry

803 Words 4 Pages
Physics practical theory:
Hydrochloric acid is a clear is a highly corrosive, strong mineral acid with many industrial uses.
Major production started in the Industrial Revolution, hydrochloric acid is used in the chemical industry as a chemical reagent in the large-scale production of PVC plastic, and MDI/TDI for polyurethane. It has numerous smaller-scale applications, including household cleaning, production of gelatine and other food additives, descaling, and leather processing. About 20 million tonnes of hydrochloric acid are produced worldwide annually.
Chemical properties and reactions:
Hydrogen chloride (HCl) is a monoprotic acid, which means it can dissociate to give up one H+ ion. In aqueous hydrochloric acid, the H+ joins a water
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It is one of the least hazardous strong acids to handle; despite its acidity, it consists of the non-reactive and non-toxic chloride ion. Intermediate-strength hydrochloric acid solutions are quite stable upon storage, maintaining their concentrations over time. These attributes, plus the fact that it is available as a pure reagent, make hydrochloric acid an excellent acidifying reagent.

Hydrochloric acid is the preferred acid in titrations for determining the amount of bases. Strong acid titrants give more precise results due to a more distinct endpoint.
Hydrochloric acid is frequently used in chemical analysis to prepare samples for analysis. Concentrated hydrochloric acid dissolves many metals and forms oxidized metal chlorides and hydrogen gas, and it reacts with basic compounds such as calcium carbonate or copper(II) oxide, forming the dissolved chlorides that can be analysed.
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Acid base titrations:
A titration is the addition of a measured volume of one solution, from a burette, to an unknown volume/concentration of another solution until the reaction between then is complete. An acid base titration is carried out to determine an unknown concentration by using a solution of known concentration. An indicator is used to show a dramatic and rapid colour change, at the end point of the titration.
Preparing a standard solution:
The substance used for the standard solution must have a high degree of purity, preferably solid, because this is easier to measure (using a scale) and the substance can’t absorb water or release water.
Oxalic acid and anhydrous sodium carbonate are used to make the standard solutions.
The solid crystals must be weighed accurately and then transferred to a volumetric flask. It must then be filled up to the mark, so that we have a known mass in a known volume.
The concentration can be calculated by using the formula n=m/M
Your number of moles can then be substituted to find the concentration

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