give me an example in which H2SO4 behaves as strong acid
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Infobox references
The acid's corrosiveness towards other materials can be mainly described due to its strong acidic nature, and if at a high concentration its dehydrating alongside oxidizing properties. It is also hygroscopic, readily absorbing water vapor from the air.[6] Upon contact, sulfuric acid can cause severe chemical burns and even secondary thermal burns due to dehydration; it is very dangerous even at lower concentrations.[7][8]
Sulfuric acid is a very important commodity chemical, and a nation's sulfuric acid production is a good indicator of its industrial strength.[9] It is widely produced with different methods, such as contact process, wet sulfuric acid process, lead chamber process and some other methods.[10]
Sulfuric acid is also a key substance in the chemical industry. It is most commonly used in fertilizer manufacture,[11] but is also important in mineral processing, oil refining, wastewater processing, and chemical synthesis. It has a wide range of end applications including in domestic acidic drain cleaners,[12] as an electrolyte in lead-acid batteries, in dehydrating a compound, and in various cleaning agents.
Physical properties
Grades of sulfuric acid
Although nearly 100% sulfuric acid solutions can be made, the subsequent loss of SO
3 at the boiling point brings the concentration to 98.3% acid. The 98.3% grade is more stable in storage, and is the usual form of what is described as "concentrated sulfuric acid". Other concentrations are used for different purposes. Some common concentrations are:[13][14]
Mass fraction
H2SO4 Density
(kg/L) Concentration
(mol/L) Common name
<29% 1.00-1.25 <4.2 diluted sulfuric acid
29–32% 1.25–1.28 4.2–5.0 battery acid
(used in lead–acid batteries)
62–70% 1.52–1.60 9.6–11.5 chamber acid
fertilizer acid
78–80% 1.70–1.73 13.5–14.0 tower acid
Glover acid
93.2% 1.83 17.4 66 °Bé ("66-degree Baumé") acid
98.3% 1.84 18.4 concentrated sulfuric acid
"Chamber acid" and "tower acid" were the two concentrations of sulfuric acid produced by the lead chamber process, chamber acid being the acid produced in the lead chamber itself (<70% to avoid contamination with nitrosylsulfuric acid) and tower acid being the acid recovered from the bottom of the Glover tower.[13][14] They are now obsolete as commercial concentrations of sulfuric acid, although they may be prepared in the laboratory from concentrated sulfuric acid if needed. In particular, "10M" sulfuric acid (the modern equivalent of chamber acid, used in many titrations) is prepared by slowly adding 98% sulfuric acid to an equal volume of water, with good stirring: the temperature of the mixture can rise to 80 °C (176 °F) or higher.[14]
Sulfuric acid reacts with its anhydride, SO
3, to form H
2S
2O
7, called pyrosulfuric acid, fuming sulfuric acid, Disulfuric acid or oleum or, less commonly, Nordhausen acid. Concentrations of oleum are either expressed in terms of % SO
3 (called % oleum) or as % H
2SO
4 (the amount made if H
2O were added); common concentrations are 40% oleum (109% H
2SO
4) and 65% oleum (114.6% H
2SO
4). Pure H
2S
2O
7 is a solid with melting point of 36 °C.
Pure sulfuric acid has a vapor pressure of <0.001 mmHg at 25 °C and 1 mmHg at 145.8 °C,[15] and 98% sulfuric acid has a <1 mmHg vapor pressure at 40 °C.[16]
Pure sulfuric acid is a viscous clear liquid, like oil, and this explains the old name of the acid ('oil of vitriol').
Commercial sulfuric acid is sold in several different purity grades. Technical grade H
2SO
4 is impure and often colored, but is suitable for making fertilizer. Pure grades, such as USP grade, are used for making pharmaceuticals and dyestuffs. Analytical grades are also available.
Nine hydrates are known, but four of them were confirmed to be tetrahydrate (H2SO4·4H2O), hemihexahydrate (H2SO4·6 1⁄2H2O) and octahydrate (H2SO4·8H2O).
Polarity and conductivity
Equilibrium of anhydrous sulfuric acid[17]
Species mMol/kg
HSO−
4 15.0
H
3SO+
4 11.3
H
3O+ 8.0
HS
2O−
7 4.4
H
2S
2O
7 3.6
H
2O 0.1
Anhydrous H
2SO
4 is a very polar liquid, having a dielectric constant of around 100. It has a high electrical conductivity, caused by dissociation through protonating itself, a process known as autoprotolysis.[17]
2 H
2SO
4 ⇌ H
3SO+
4 + HSO−
4
The equilibrium constant for the autoprotolysis is[17]
Kap (25 °C) = [H
3SO+
4][HSO−
4] = 2.7×10−4
The comparable equilibrium constant for water, Kw is 10−14, a factor of 1010 (10 billion) smaller.
In spite of the viscosity of the acid, the effective conductivities of the H
3SO+
4 and HSO−
4 ions are high due to an intramolecular proton-switch mechanism (analogous to the Grotthuss mechanism in water), making sulfuric acid a good conductor of electricity. It is also an excellent solvent for many reac