Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
HAH++A-
The acidity of a molecule (HA) depends on the stability of the conjugate base (A-).
This can be determined via ARIO rule
The stability of the -ve charge on the conjugate base depends on the following four factors.
1. The type of atom that carries the charge (A): Size and electronegativity of the -ve charge-carrying atom. Greater the size of the atom, the more stable the -ve charge. Similarly greater the electronegativity of the atom, the more stable the conjugate base.
2. Resonance (R): Resonance stabilizes the -ve charge by delocalization. Hence greater the chance for such resonance, the more stable the conjugate base.
3. Induction (I): Induction can also stabilize the -ve charge on the conjugate base by spreading it out.
4. The type of orbital where the charge resides (O): Shorter the size of the atomic orbital where the electron pair is residing, the greater its stability.
These factors construct the acronym, ARIO. While comparing the acidity of protons, we generally use ARIO as
the order of importance of these stabilizing effects.
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