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R is the gas constant and T is the absolute temperature. Note that pK a = −log(K a) and 2.303 ≈ ln(10). At 25 °C, ΔG ⊖ in kJ·mol −1 ≈ 5.708 pK a (1 kJ·mol −1 = 1000 joules per mole). Free energy is made up of an enthalpy term and an entropy term. [11] =
where [] is not included because in dilute solution the solvent is essentially a pure liquid with a thermodynamic activity of one. [2]: 668 K a is variously named a dissociation constant, [3] an acid ionization constant, [2]: 668 an acidity constant [1] or an ionization constant.
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An equilibrium constant is related to the standard Gibbs free energy change of reaction by = , where R is the universal gas constant, T is the absolute temperature (in kelvins), and ln is the natural logarithm.
The solvent (e.g. water) is omitted from this expression when its concentration is effectively unchanged by the process of acid dissociation. The strength of a weak acid can be quantified in terms of a dissociation constant , K a {\displaystyle K_{a}} , defined as follows, where [ X ] {\displaystyle {\ce {[X]}}} signifies the concentration of a ...
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.
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The gas constant occurs in the ideal gas law: = = where P is the absolute pressure, V is the volume of gas, n is the amount of substance, m is the mass, and T is the thermodynamic temperature. R specific is the mass-specific gas constant. The gas constant is expressed in the same unit as molar heat.