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Up to the 1970s, commercial quantities of sulfuric acid were produced from anhydrous calcium sulfate. [14] Upon being mixed with shale or marl, and roasted at 1400°C, the sulfate liberates sulfur dioxide gas, a precursor to sulfuric acid. The reaction also produces calcium silicate, used in cement clinker production. [15] [16]
The inverse comproportionation reaction is the reaction occurring in the Claus process used for desulfurization of oil and gas crude products in the refining industry: H 2 S + 3 / 2 O 2 → SO 2 + H 2 O. By rewriting the last reaction in the inverse direction one obtains a reaction consistent with what is observed in the lime sulfur global ...
The sulfuric acid dissolves the carbonates in the hardened cement paste (HCP), and also calcium hydroxide (portlandite: Ca(OH) 2) and calcium silicate hydrate (CaO·SiO 2 ·nH 2 O), and causes strength loss, as well as producing sulfates which are harmful to concrete. [19] H 2 SO 4 + Ca(OH) 2 → CaSO 4 + 2 H 2 O H 2 SO 4 + CaO·SiO 2 ·n H 2 O ...
The same equation relating the concentrations of acid and base applies. The concept of neutralization is not limited to reactions in solution. For example, the reaction of limestone with acid such as sulfuric acid is also a neutralization reaction. [Ca,Mg]CO 3 (s) + H 2 SO 4 (aq) → (Ca 2+, Mg 2+)(aq) + SO 2− 4 (aq) + CO 2 (g) + H 2 O
1 Writing reactions. 2 Examples. 3 See also. ... Sulfuric acid, H 2 SO 4; Nitric acid, HNO 3; ... Calcium hydroxide, Ca(OH) 2; Strontium hydroxide, Sr ...
Solutions containing magnesium sulfate are generally more aggressive, for the same concentration. This is because magnesium also takes part in the reactions, replacing calcium in the solid phases with the formation of brucite (magnesium hydroxide) and magnesium silicate hydrates. The displaced calcium precipitates mainly as gypsum.
The hydrogen sulfide gas is biochemically oxidized in the presence of moisture to form sulfuric acid. The effect of sulfuric acid on concrete and steel surfaces exposed to severe wastewater environments can be devastating. [1] In the USA alone, corrosion causes sewer asset losses estimated at $14 billion per year. [2]
Calcium hydroxide is modestly soluble in water, as seen for many dihydroxides. Its solubility increases from 0.66 g/L at 100 °C to 1.89 g/L at 0 °C. [8] Its solubility product K sp of 5.02 × 10 −6 at 25 °C, [1] its dissociation in water is large enough that its solutions are basic according to the following dissolution reaction: