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Acid dissociation constants are also essential in aquatic chemistry and chemical oceanography, where the acidity of water plays a fundamental role. In living organisms, acid–base homeostasis and enzyme kinetics are dependent on the p K a values of the many acids and bases present in the cell and in the body.
In physical chemistry, the Arrhenius equation is a formula for the temperature dependence of reaction rates.The equation was proposed by Svante Arrhenius in 1889, based on the work of Dutch chemist Jacobus Henricus van 't Hoff who had noted in 1884 that the Van 't Hoff equation for the temperature dependence of equilibrium constants suggests such a formula for the rates of both forward and ...
Numerical values of these thermodynamic properties are collected as tables or are calculated from thermodynamic datafiles. Data is expressed as temperature-dependent values for one mole of substance at the standard pressure of 101.325 kPa (1 atm), or 100 kPa (1 bar).
Since Tris' pKa is more strongly temperature dependent, its use is not recommended in biochemical applications requiring consistent pH over a range of temperatures. Moreover, the temperature dependance of the pKa (and in turn buffer solution pH) makes pH adjustment difficult. [8] (E.g., the 'room temperature' pH adjustment would not translate ...
The pH-dependent effects cannot be added in the same straightforward way and have to be accounted for using Boltzmann summation, Tanford–Roxby iterations or other methods. The interplay of the intrinsic p K a values of a system with the electrostatic interaction energies between titratable groups can produce quite spectacular effects such as ...
In chemistry, biochemistry, and pharmacology, a dissociation constant (K D) is a specific type of equilibrium constant that measures the propensity of a larger object to separate (dissociate) reversibly into smaller components, as when a complex falls apart into its component molecules, or when a salt splits up into its component ions.
The concentration of the species LH is equal to the sum of the concentrations of the two micro-species with the same chemical formula, labelled L 1 H and L 2 H. The constant K 2 is for a reaction with these two micro-species as products, so that [LH] = [L 1 H] + [L 2 H] appears in the numerator, and it follows that this macro-constant is equal ...
The strength of an inorganic acid is dependent on the oxidation state for the atom to which the proton may be attached. Acid strength is solvent-dependent. Acid strength is solvent-dependent. For example, hydrogen chloride is a strong acid in aqueous solution, but is a weak acid when dissolved in glacial acetic acid .