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Ionization of a compound in Chemistry is the process by which neutral molecules are divided into charged ions in a solution. According to the Arrhenius Theory, acids are substances that dissociate in an aqueous medium to produce hydrogen ions, H+ ions, and bases are substances that dissociate in an aqueous medium producing OH- ions. The strength of acids and bases can be defined based on the degree of ionization of acids and bases.
Here in this article, we will learn about, Ionization Definition, Arrhenius Concept of Acid and Base, and Explanation of Arrhenius Acid and Base Ionization concept, Examples, and others in detail.
Table of Content
Ionization of a compound is defined as the process in which a compounds dissociates into its constituent ions. When a compound whether acidic or basic is dissolved into an aqueous solution, they dissociate into positive and negative ion respectively. In case of acids, the H+ ions are release and in case of base OH- ions are released. Sometimes, the ionization is not easy such as in salts. The compounds that is to be dissolved in the given solvent is called the electrolyte and its dissociation is measured in form of degree of dissociation.
Degree of Ionization of any compound is defined as the ratio of the number of molecule undergoing dissociation to total number of molecules of the compound. It is defined using the symbol "α"(Degree of Ionization)
Arrhenius explain the concept of acid and base as the compounds that in aqueous medium generates ions. "An acid is a compound that produces an Hydrogen Ions(H+) in the aqueous solution" whereas "Base is a compouns that produces Hydoxyl Ions(OH-) in the aqueous medium."
Ionization of Acid(HCl)
HCl(aq.) → H+ + Cl-
Ionization of Base(KOH)
KOH(aq.) → K+ + OH-
Accoring to Arrhenius, the dissociation equillibrium of acid and base are dynamic in nature. Suppose we take an acid HA and HA has higher tendency to donate eclectrons than H3O+ then in that case HA acts as strong acid.
HA + H2O ⇌ H3O+ + A-
Now, stronger acid denotes protons the equlibrium moves in the direction of formation weaker base. This implies that a strong acid generally have a weaker base.
Degree of ionisation of the acids and bases contributes to their strength. The degree of ionisation might vary depending on the acidic and basic substances. Ionization constant of acid and base is the constant that tells us the strength of acid and the base. Higher the dissociation constant of acid and base higher is the strength of acid and base.
Degree of ionisation refers to the acidity or baseness of an acid or base. A strong acid ionizes completely in the water, whereas a weak acid just ionizes partially in the aqueous solution. Now an Arrhenius Acid ionizes as,
HA (aq) + H2O ⇌ H3O+ (aq) + A–
Now, the equllibrium constant is,
Ka = [H3O+] [A–] / [HA]
where Ka is the ionization constant of acid and hiher the value of Ka higher is the strength of the acid.
In an aqueous solution, some bases, such as Lithium Hydroxide or Sodium Hydroxide, totally dissociate into their ions and are referred to as strong bases. Now an Arrhenius Base ionizes as,
A + H2O ⇌ OH– + HA+
Now, the equllibrium constant is,
Kb = [OH–] [HA+] / [A]
where Kb is the base ionization constant and higher value of Kb represent the higher strength of the base.
Ionization of various acid and bases are added below,
The ionization of some popular acids are discussed below:
HCl (Hydrochloric Acid) is a strong acid and it ionizes as,
HCl + H2O ⇌ Cl- + H3O+
CH3COOH (Acetic Acid) is a weak acid and it ionizes as,
CH3COOH + H2O ⇌ CH3COO‾ + H3O+
The ionization of some popular bases are discussed below:
NaOH (Sodim Hydroxide) is a strong base and it ionizes as,
NaOH + H2O ⇌ Na+ + OH-
NH4OH (Ammonium Hydroxide) is a weak base and it ionizes as,
NH3 + H2O ⇌ NH4+ (aq) + OH‾(aq)
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