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In chemistry, Le Chatelier's principle (pronounced UK: / l ə ʃ æ ˈ t ɛ l j eɪ / or US: / ˈ ʃ ɑː t əl j eɪ /), also called Chatelier's principle, Braun–Le Chatelier principle, Le Chatelier–Braun principle or the equilibrium law, [1] is a principle used to predict the effect of a change in conditions on chemical equilibrium. [2]
Common-ion effect. In chemistry, the common-ion effect refers to the decrease in solubility of an ionic precipitate by the addition to the solution of a soluble compound with an ion in common with the precipitate. [1] This behaviour is a consequence of Le Chatelier's principle for the equilibrium reaction of the ionic association / dissociation.
In accordance with Le Chatelier's Principle, when the dissolution process is endothermic (heat is absorbed), solubility increases with rising temperature. This effect is the basis for the process of recrystallization , which can be used to purify a chemical compound.
Henry Louis Le Chatelier[1] (French pronunciation: [ɑ̃ʁi lwi lə ʃɑtəlje]; 8 October 1850 – 17 September 1936) was a French chemist of the late 19th and early 20th centuries. He devised Le Chatelier's principle, used by chemists and chemical engineers to predict the effect a changing condition has on a system in chemical equilibrium.
Following Le Chatelier's principle, the chemical equilibrium of the Earth's carbon cycle will shift in response to anthropogenic CO 2 emissions. The primary driver of this is the ocean, which absorbs anthropogenic CO 2 via the so-called solubility pump.
Weak. v. t. e. In chemistry, an acid dissociation constant (also known as acidity constant, or acid-ionization constant; denoted ) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction. known as dissociation in the context of acid–base reactions.
In calcium sulfate, the reason is that the dissolution reaction of calcium sulfate itself is exothermic and therefore is favored when the temperature decreases (then, the dissolution heat is more easily evacuated; see Le Chatelier's principle). In other terms, the solubility of calcium carbonate and calcium sulfate increases at low temperature ...
By Le Chatelier's principle, the release of CO 2 from the lungs pushes the reaction above to the left, causing carbonic anhydrase to form CO 2 until all excess protons are removed. Bicarbonate concentration is also further regulated by renal compensation , the process by which the kidneys regulate the concentration of bicarbonate ions by ...