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Protein kinase B (PKB), also known as Akt, is the collective name of a set of three serine/threonine-specific protein kinases that play key roles in multiple cellular processes such as glucose metabolism, apoptosis, cell proliferation, transcription, and cell migration.
RAC(Rho family)-alpha serine/threonine-protein kinase is an enzyme that in humans is encoded by the AKT1 gene.This enzyme belongs to the AKT subfamily of serine/threonine kinases that contain SH2 (Src homology 2-like) protein domains. [5]
For example, phosphorylation of BAD, the Bcl-2 family member, on Ser136 causes translocation from the mitochondrial membrane to the cytosol, where it is sequestered by 14-3-3 proteins. [27] Akt phosphorylates Caspase-9 on Ser196, preventing a caspase cascade leading to cell death.
As the name suggests, a non-nucleophilic base is a sterically hindered organic base that is a poor nucleophile.Normal bases are also nucleophiles, but often chemists seek the proton-removing ability of a base without any other functions.
In inorganic chemistry, bicarbonate (IUPAC-recommended nomenclature: hydrogencarbonate [2]) is an intermediate form in the deprotonation of carbonic acid. It is a polyatomic anion with the chemical formula H C O − 3. Bicarbonate serves a crucial biochemical role in the physiological pH buffering system. [3]
Creatine (/ ˈ k r iː ə t iː n / or / ˈ k r iː ə t ɪ n /) [1] is an organic compound with the nominal formula (H 2 N)(HN)CN(CH 3)CH 2 CO 2 H.It exists in various tautomers in solutions (among which are neutral form and various zwitterionic forms).
Also acid ionization constant or acidity constant. A quantitative measure of the strength of an acid in solution expressed as an equilibrium constant for a chemical dissociation reaction in the context of acid-base reactions. It is often given as its base-10 cologarithm, p K a. acid–base extraction A chemical reaction in which chemical species are separated from other acids and bases. acid ...
[c] [2] For example, a hypothetical weak acid having K a = 10 −5, the value of log K a is the exponent (−5), giving pK a = 5. For acetic acid, K a = 1.8 x 10 −5, so pK a is 4.7. A higher K a corresponds to a stronger acid (an acid that is more dissociated at equilibrium).