Search results
14 sie 2020 · For an aqueous solution of a weak acid, the dissociation constant is called the acid ionization constant (K_a). Similarly, the equilibrium constant for the reaction of a weak base with water is the base ionization constant (K_b). For any conjugate acid–base pair, K_aK_b = K_w.
- Autoionization of Water and pH
Recall that because of its highly polar structure, liquid...
- Definitions of Acids and Bases
Acids and bases have been known for a long time. When Robert...
- Autoionization of Water and pH
29 wrz 2021 · The K w is the ionic product of water. It is the equilibrium constant for the dissociation of water at 298 K; Its value is 1.00 x 10-14 mol 2 dm-6; For the ionisation of water the equilibrium expression to find K w is as follows: H 2 O (l) ⇌ H + (aq) + OH-(aq) As the extent of ionisation is very low, only small amounts of H + and OH - ions ...
Relationship: Ka×Kb=Kw where Kw is the ion-product constant for water (1.0×10−14 at 25°C). Importance in Chemical Reactions. Predicting Direction: Ka and Kb can help predict the direction of acid-base reactions. Equilibrium Position: Understanding the strength of acids and bases helps in determining the position of equilibrium in a reaction.
28 kwi 2021 · There is a simple relationship between the magnitude of \(K_a\) for an acid and \(K_b\) for its conjugate base. Consider, for example, the ionization of hydrocyanic acid (\(HCN\)) in water to produce an acidic solution, and the reaction of \(CN^−\) with water to produce a basic solution:
The dissociation constant of a weak acid, denoted as Ka, is a measure of the strength of the acid. It represents the equilibrium constant for the dissociation reaction of the acid in aqueous solution, where the acid donates a proton (H+) to water to form its conjugate base (A-) and a hydronium ion (H3O+).
Theoretical background. The acid dissociation constant for an acid is a direct consequence of the underlying thermodynamics of the dissociation reaction; the p Ka value is directly proportional to the standard Gibbs free energy change for the reaction.
Explains the meaning of the terms strong and weak as applied to acids, and introduces pH, Ka and pKa
