Name each of the following species for the following acid-base reactions. (The equilibrium lies to the right in each case, i.e., the product side is favored. If the species is an ion, include the word "ion" in the name. Use systematic names such as "methanol" instead of archaic names like "methyl alcohol" or "wood alcohol".)
(a) H3O+ (hydronium ion) + CH3O- (methoxide ion) <--> reverse reaction arrow
acid:?
base:?
conjugate acid:?
conjugate base:?
(b) CH3CH2O- (ethoxide ion) + HCl (hydrogen chloride) <--> reverse reaction arrow
acid:?
base:?
conjugate acid:?
conjugate base:?
(c) NH2- (amide ion) + CH3OH (methanol) <--> reverse reaction arrow
acid:?
base:?
conjugate acid:?
conjugate base:?

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

The species accepting a proton is considered as a base and after accepting a proton, it forms a conjugate acid.

The species losing a proton is considered as an acid and after loosing a proton, it forms a conjugate base

For the given chemical equation:

a) [tex]H_3O^++CH_3O^-\rightleftharpoons CH_3OH+H_2O[/tex]

acid : hydronium ion

base : methoxide ion

conjugate acid : methanol

conjugate base: water

b) [tex]CH_3CH_2O^-+HCl\rightleftharpoons CH_3CH_2OH+Cl^-[/tex]

acid : hydrogen chloride

base : ethoxide ion

conjugate acid : ethanol

conjugate base: chloride ion

c) [tex]NH_2^-+CH_3OH\rightleftharpoons NH_3+CH_3O^-[/tex]

acid : methanol

base : amide ion

conjugate acid : ammonia

conjugate base: methoxide ion

.