Publication

Catalysis at room temperature ionic liquid|water interface: H2O2 generation

Hubert Girault, Gunther Wittstock
2015
Journal Articles

Abstract

H2O2 is produced at the interface between a room-temperature ionic liquid with decamethylferrocene as electron donor and an acidic aqueous solution. The electron donor can be regenerated electrochemically.

Official source

https://infoscience.epfl.ch/entities/publication/52755ab8-6be7-4dca-8046-a6bdaefc34db

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Hubert Girault, Gunther Wittstock
2015
Journal Articles

Abstract

Official source

https://infoscience.epfl.ch/entities/publication/52755ab8-6be7-4dca-8046-a6bdaefc34db

About this result

Related concepts (11)

Aqueous solution

An aqueous solution is a solution in which the solvent is water. It is mostly shown in chemical equations by appending (aq) to the relevant chemical formula. For example, a solution of table salt, or sodium chloride (NaCl), in water would be represented as . The word aqueous (which comes from aqua) means pertaining to, related to, similar to, or dissolved in, water. As water is an excellent solvent and is also naturally abundant, it is a ubiquitous solvent in chemistry.

Acid

An acid is a molecule or ion capable of either donating a proton (i.e. hydrogen ion, H+), known as a Brønsted–Lowry acid, or forming a covalent bond with an electron pair, known as a Lewis acid. The first category of acids are the proton donors, or Brønsted–Lowry acids. In the special case of aqueous solutions, proton donors form the hydronium ion H3O+ and are known as Arrhenius acids. Brønsted and Lowry generalized the Arrhenius theory to include non-aqueous solvents.

Acid strength

Acid strength is the tendency of an acid, symbolised by the chemical formula HA, to dissociate into a proton, H+, and an anion, A-. The dissociation of a strong acid in solution is effectively complete, except in its most concentrated solutions. HA -> H+ + A- Examples of strong acids are hydrochloric acid (HCl), perchloric acid (HClO4), nitric acid (HNO3) and sulfuric acid (H2SO4). A weak acid is only partially dissociated, with both the undissociated acid and its dissociation products being present, in solution, in equilibrium with each other.

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