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The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Concentrated sulfuric acid has a powerful dehydrating property, removing water (H 2 O) from other chemical compounds such as table sugar and other carbohydrates, to produce carbon, steam, and heat. Dehydration of table sugar (sucrose) is a common laboratory demonstration. [ 21 ]
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/100 ml), unless shown otherwise. The substances are listed in alphabetical order.
Sulfuric(IV) acid (United Kingdom spelling: sulphuric(IV) acid), also known as sulfurous (UK: sulphurous) acid and thionic acid, [citation needed] is the chemical compound with the formula H 2 SO 3. Raman spectra of solutions of sulfur dioxide in water show only signals due to the SO 2 molecule and the bisulfite ion, HSO − 3 . [ 2 ]
The most important chemical sodium sulfate production is during hydrochloric acid production, either from sodium chloride (salt) and sulfuric acid, in the Mannheim process, or from sulfur dioxide in the Hargreaves process. [21] The resulting sodium sulfate from these processes is known as salt cake. Mannheim: 2 NaCl + H 2 SO 4 → 2 HCl + Na 2 SO 4
The first and faster [citation needed] process is the removal of hydrogen and oxygen as units of water by the concentrated sulfuric acid. This occurs because hydration of concentrated sulfuric acid is strongly thermodynamically favorable, with a standard enthalpy of reaction ( ΔH ) of −880 k J / mol .
Oleum is a useful form for transporting sulfuric acid compounds, typically in rail tank cars, between oil refineries, which produce various sulfur compounds as a byproduct of refining, and industrial consumers. Certain compositions of oleum are solid at room temperature, and thus are safer to ship than as a liquid.
Antimony(III) sulfate was first produced in 1827 by the reaction of antimony(III) oxide and 18 molar sulfuric acid at 200 °C: [1]. Sb 2 O 3 + 3 H 2 SO 4 → Sb 2 (SO 4) 3 + 3 H 2 O. The concentration of the sulfuric acid is important, as a lower concentration will produce basic antimony oxides, while a higher concentration will produce antimony(III) pyrosulfate.