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A salt with this anion is sometimes called an acid oxalate, monobasic oxalate, or hydrogen oxalate. The equilibrium constant (K a) for loss of the first proton is 5.37 × 10 −2 (pK a = 1.27). The loss of the second proton, which yields the oxalate ion, has an equilibrium constant of 5.25 × 10 −5 (pK a = 4.28).
In coordination chemistry, a stability constant (also called formation constant or binding constant) is an equilibrium constant for the formation of a complex in solution. It is a measure of the strength of the interaction between the reagents that come together to form the complex. There are two main kinds of complex: compounds formed by the ...
3 (i.e. the first acid dissociation constant for carbonic acid), K 2 is the equilibrium constant for the reaction HCO − 3 ⇌ H + + CO 2− 3 (i.e. the second acid dissociation constant for carbonic acid), and DIC is the (unchanging) total concentration of dissolved inorganic carbon in the system, i.e. [CO 2] + [HCO − 3] + [CO 2− 3].
The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change. For a given set of reaction conditions, the equilibrium constant is ...
However, the equilibrium constant for the loss of two protons applies equally well to the equilibrium [M(H 2 O) n] z+ - 2 H + ⇌ [MO(H 2 O) n-2] (z-2)+ + H 2 O. because the concentration of water is assumed to be constant. This applies in general: any equilibrium constant is equally valid for a product with an oxide ion as for the product with ...
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
At chemical equilibrium, the reaction quotient Q r of the product activity (a Red) by the reagent activity (a Ox) is equal to the equilibrium constant (K) of the half-reaction and in the absence of driving force (ΔG = 0) the potential (E red) also becomes nul. The numerically simplified form of the Nernst equation is expressed as:
An attempt to quantify the 'softness' of a base consists in determining the equilibrium constant for the following equilibrium: BH + CH 3 Hg + ⇌ H + + CH 3 HgB. where CH 3 Hg + (methylmercury ion) is a very soft acid and H + (proton) is a hard acid, which compete for B (the base to be classified). Some examples illustrating the effectiveness ...