What is the relationship between conjugated acid base to ka kb

The relationship between ka and kb of the conjugated acid-base pair is ka·kb=kw. The molecule or ion that can give protons is an acid, the molecule or ion that can accept a proton is a base, the acid that gives protons is converted into a corresponding base, and the base accepts protons into a corresponding acid. This pair of acids and bases that change to each other due to the gain and loss of protons is called a conjugated acid-base pair.

A conjugated acid-base pair is a pair of acids and bases that are linked by proton gains and losses. According to the acid-base proton theory.

Acid and base always exist in correspondence, the acid gives proton to become its conjugate base, and the base gets proton to become its corresponding conjugate acid, this relationship is called conjugation.

A pair of conjugated acids and bases, acidic.

The larger the ka, the more conjugated the base.

The smaller the kb, the more acidic the strength order of the conjugate base can be deduced.

The intensity order of the conjugated acids and bases, as well as their KA values, is listed here, but it is listed in the form of a list, so it is not convenient to publish it here.

See for yourself.

There is a definite relationship between the dissociation constants ka and kb of the conjugated acid-base pair. Taking HAC as an example, the derivation is as follows:

hac+h2o===>h3o+ +ac-ka===c(h3o+)*c(ac-)/c(hac)ac-+h2o==>hac+oh-

kb===c(hac)*c(oh-)/c(ac-)ka*kb= c(h3o+)*c(ac-)/c(hac) *c(hac)*c(oh-)/c(ac-)=c(h+)*c(oh-)=kw

There is a definite relationship between the dissociation constants of the conjugated acid-base pair ka and the lead kb.

ka is a weak acid.

The ionization equilibrium is constant.

KB is the ionization equilibrium constant of a weak base.

kw is the ionic product constant of water. Bu Jiheng.

kh is a weak base cation.

or weakly acid anion.

Hydrolysis constant.

Ksp is the solubility product constant of the insoluble substance.

The relationship between Ka and KB of the conjugated acid-base pair is that the larger the Ka of the acid, the smaller the KB of the conjugate base, so the strength order of the conjugate base can be deduced from the order of acidity. Acid-base defines a substance that can give protons as an acid, and a substance that can accept protons as a base. The base formed by the loss of a proton of an acid is called the conjugate base of the acid, and the latter becomes the conjugate acid of the base after gaining a proton.

The relationship between ka and kb of the conjugated acid-base pair is ka·kb=kw. The molecule or ion that can give protons is an acid, the molecule or ion that can accept a proton is a base, the acid that gives a proton to turn into a corresponding base, and the base that accepts a proton into a corresponding acid. This pair of acids and bases that change to each other due to the gain and loss of protons is called a conjugated acid-base pair.

The conjugated acid-base pair is a pair of acids and bases that are bound together by the proton gain and loss relationship. According to the acid-base proton theory, the acid and the base always exist in correspondence, the acid gives the macrobucket proton to become its conjugate base, and the base gets the proton to become its corresponding conjugate acid, this relationship is called the conjugate relationship.

Answer]: KA of conjugated acid-base pairs

The quantitative relationship with KB is KAKBKW

Because of this relationship, the acid and base of the proton theory of Hekong are not separated by each other, but are unified in the relation to the proton, i.e., acid(a)=h+

proton) + (b-

Due to the existence of this conjugation relationship of alkali, and at a certain temperature, kw is the fixed value, there must be a correspondence that the stronger a certain acid, the weaker the conjugate base.

In chemistry, ka means acidity equilibrium constant, kb means alkali equilibrium constant, and kw means the ionic product constant of water, and its function is to calculate the equilibrium constant of the corresponding substance separately.

All equilibrium constants (including ka, kb, kw all obey this formula) are expressed in the same formula, as follows:

The differential expression of all equilibrium Chang Shi feet is:

The relative definite integral is expressed in the form of:

In chemistry, we often use k to represent the equilibrium constant, and the subscript table returns to show a certain class of substances, such as a is the abbreviation of acid, mega high so ka is the equilibrium constant of acid, under specific conditions (such as temperature t, pressure p, solvent properties, ionic strength, etc.), when the reversible chemical reaction reaches the equilibrium state, the ratio of the concentration product of the product of the product to the reactant or the ratio of the product of the concentration of the reaction product to the reaction substrate.

Thermodynamically speaking, all reactions have reverse reactions, that is to say, all reactions have thermodynamic equilibrium and equilibrium constants. The greater the equilibrium constant, the more thorough the reaction.