Hydrochloric acid tank may be produced with 2 different raw materials as polyester and polyethylene. It is generally suitable for hydrochloric acid stocked as a 37% concentrate in 2 product groups. Polyethylene tanks are produced by 40% thickening. The stock temperature value for hydrochloric acid storage should not exceed 40 degrees. In particular, tanks exposed to direct sunlight in the open air should be covered and the temperature should be balanced.

Hydrochloric Acid Tank

Polythene Hydrochloric Acid Tank

Polythene hydrochloric acid tank is produced by using 40% more material than product standards. This ratio is applied to provide the tank withstand the overload that the concentrate ratio will provide. For example, an acid with a concentration of 30% to be put in a 10 tonne tank would have a weight of 13 tonnes. Therefore, polyethylene products need to be thickened. The outlet rakors are also external threaded made of PE material or PVC free flanges. Requested changes for outlet rakor size may affect product prices.
For more detailed product specifications, you can visitpolythene acid tanks.

Vinylester Hydrochloric Acid Tanks

Vinylester HCl acid tanks can be produced horizontally or vertically in desired dimensions. Surface tissue that used for inner side of tank provides the best trapping of the fiber resin and increases the chemical resistance of the product. Then the required amount of glass fiber is used according to the product volume and processed with vinylester epoxy resin.
Vinylester acid tanks, which have a flexible structure in terms of equipment, can have many equipments such as outlet rakor, free flange, manway and integrated level indicator.

Hydrochloric Acid Tank

20 Ton Hydrochloric Acid Tank

The maximum concentration ratio for the storage of vinylester hydrochloric acid tanks is 37% and the maximum temperature is 40 degrees.
İstenilen ölçüde yatay veya dikey olarak üretilebilen ve 5 yıllık garanti süresine sahip olan ürünlerimizin polietilen asit tanklarına göre maliyeti daha yüksektir.

What Is Hydrochloric Acid?

Hydrochloric acid is the salt of hydronium ion, H3O+ and chloride. It is usually prepared by treating HCl with water.
However, the speciation of hydrochloric acid is more complicated than this simple equation implies. The structure of bulk water is infamously complex, and likewise, the formula H3O+ is also a gross oversimplification of the true nature of the solvated proton, H+, present in hydrochloric acid. A combined IR, Raman, X-ray and neutron diffraction study of concentrated solutions of hydrochloric acid revealed that the primary form of H+ in these solutions is H5O2+, which, along with the chloride anion, is hydrogen-bonded to neighboring water molecules in several different ways. (In H5O2+, the proton is sandwiched midway between two water molecules at 180°). The author suggests that H3O+ may become more important in dilute HCl solutions. (See Hydronium for further discussion of this issue.)
Hydrochloric acid is a strong acid, since it is completely dissociated in water. It can therefore be used to prepare salts containing the Cl– anion called chlorides.
As a strong acid, hydrogen chloride has a large Ka. Theoretical attempts to assign the pKa of hydrogen chloride have been made, with the most recent estimate being −5.9. However, it is important to distinguish between hydrogen chloride gas and hydrochloric acid. Due to the leveling effect, except when highly concentrated and behavior deviates from ideality, hydrochloric acid (aqueous HCl) is only as acidic as the strongest proton donor available in water, the aquated proton (popularly known as “hydronium ion”). When chloride salts such as NaCl are added to aqueous HCl, they have only a minor effect on pH, indicating that Cl− is a very weak conjugate base and that HCl is fully dissociated in aqueous solution. Dilute solutions of HCl have a pH close to that predicted by assuming full dissociation into hydrated H+ and Cl−.
Of the six common strong mineral acids in chemistry, hydrochloric acid is the monoprotic acid least likely to undergo an interfering oxidation-reduction reaction. 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 titration for determining the amount of bases. Strong acid titrants give more precise results due to a more distinct endpoint. Azeotropic, or “constant-boiling”, hydrochloric acid (roughly 20.2%) can be used as a primary standard in quantitative analysis, although its exact concentration depends on the atmospheric pressure when it is prepared.
Hydrochloric acid is frequently used in chemical analysis to prepare (“digest”) samples for analysis. Concentrated hydrochloric acid dissolves many metals and forms oxidized metal chlorides and hydrogen gas. It also reacts with basic compounds such as calcium carbonate or copper(II) oxide, forming the dissolved chlorides that can be analyzed.