For each of the following reactions, identify the acid and the base. Also indicate which acid–base definition (Lewis, Brønsted–Lowry) applies. In some cases, more than one definition may apply. XeO3 + OH−→ [HXeO4]− Pt + XeF4 → PtF4 + Xe C2H5OH + H2SeO4 → C2H5OH2+ + HSeO4− [CH3Hg(H2O)]+ + SH− ⇌ [CH3HgS]− + H3O+ (benzyl)3 N + CH3COOH → (benzyl)3 NH+ + CH3COO− SO2 + HCl → OSO ··· HCl
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.
For each of the following reactions, identify the acid and the base. Also indicate which acid–base definition (Lewis, Brønsted–Lowry) applies. In some cases, more than one definition may apply.
XeO3 + OH−→ [HXeO4]−
Pt + XeF4 → PtF4 + Xe
C2H5OH + H2SeO4 → C2H5OH2+ + HSeO4−
[CH3Hg(H2O)]+ + SH− ⇌ [CH3HgS]− + H3O+
(benzyl)3 N + CH3COOH → (benzyl)3 NH+ + CH3COO−
SO2 + HCl → OSO ··· HCl
The Lewis acid-base theory, named after chemist Gilbert N. Lewis, defines an acid as an electron pair acceptor and a base as an electron pair donor. According to this theory, a Lewis acid is a chemical species that can accept a pair of electrons to form a covalent bond, while a Lewis base is a chemical species that can donate a pair of electrons to form a covalent bond. This definition of acid and base is more general than the Brønsted-Lowry theory, which defines an acid as a proton (H+) donor and a base as a proton acceptor.
According to the Brønsted-Lowry acid-base theory, the key factor in acid-base reactions is the transfer of a proton from an acid to a base. In other words, a Brønsted acid is a species that has a hydrogen ion (H+) that can be donated to a base, while a Brønsted base is a species that has a lone pair of electrons that can accept a proton.
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