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The sulfate ion carries an overall charge of −2 and it is the conjugate base of the bisulfate (or hydrogensulfate) ion, HSO − 4, which is in turn the conjugate base of H 2 SO 4, sulfuric acid. Organic sulfate esters , such as dimethyl sulfate , are covalent compounds and esters of sulfuric acid.
An example hydroxylation reaction involves the oxidation of barbituric acid to alloxane. [9] Another application of the reagent in organic synthesis is in coupling reactions of alkanes. As an example tert -butanol is dimerized with Fenton's reagent and sulfuric acid to 2,5-dimethyl-2,5-hexanediol. [ 10 ]
If it is the result of a reaction between a strong acid and a strong base, the result is a neutral salt. Weak acids reacted with weak bases can produce ionic compounds with both the conjugate base ion and conjugate acid ion, such as ammonium acetate. Some ions are classed as amphoteric, being able to react with either an acid or a base. [59]
Bacterial activity in sewers – anaerobic sulfate reduction at work in the organic-rich sludges accumulated under water in the conduits produces hydrogen sulfide gas (H 2 S). After its released in the air of the galleries, H 2 S is further oxidized into sulfuric acid by atmospheric oxygen.
Sodium bisulfate, also known as sodium hydrogen sulfate, [a] is the sodium salt of the bisulfate anion, with the molecular formula NaHSO 4. Sodium bisulfate is an acid salt formed by partial neutralization of sulfuric acid by an equivalent of sodium base, typically in the form of either sodium hydroxide (lye) or sodium chloride (table salt).
In the case of water electrolysis, Gibbs free energy represents the minimum work necessary for the reaction to proceed, and the reaction enthalpy is the amount of energy (both work and heat) that has to be provided so the reaction products are at the same temperature as the reactant (i.e. standard temperature for the values given above ...
The reaction is consistent with the Brønsted–Lowry definition because in reality the hydrogen ion exists as the hydronium ion, so that the neutralization reaction may be written as H 3 O + + OH − → H 2 O + H 2 O. When a strong acid is neutralized by a strong base there are no excess hydrogen ions left in the solution.
The iodine clock reaction is a classical chemical clock demonstration experiment to display chemical kinetics in action; it was discovered by Hans Heinrich Landolt in 1886. [1] The iodine clock reaction exists in several variations, which each involve iodine species (iodide ion, free iodine, or iodate ion) and redox reagents in the presence of ...