Arrhenius Acid/Base
Arrhenius acid/base is the first theory on acid/base definitions, it is mostly true for general applications.
Arrhenius acid is any type of substance that will dissociate in water to form hydrogen ions [H+]. That is, an acid increases the concentration of H+ ions in an aqueous solution.
Arrhenius base is any type of substance that will form hydroxide [OH−] ions. It typically must increase pH since OH- increases in concentration.
Examples of Arrhenius acid
HCl, H2SO4, H3PO4 à they will donate 1, 2, and 3 protons to solution i.e. H+
Examples of Arrhenius base
NaOH, Ca(OH)2, and; avoid NH3, since it is basic, yet will not donate OH from its NH3 equation.
Bronsted Lowery Acid/Bases
First, let us define Bronsted Lowry acid/base:
Bronsted Lowry acid: any species that will donate H+ (protons) in solution, and makes pH lower (i.e HCl)
Bronsted Lowry base: any species that will accept H+ (protons) in solution, and makes pH higher (NH3 will accept H+ to form NH4+)
Typically, acid/bases are shown in the left (reactants)
when we write the products:
Bronsted Lowery conjugate base = the base formed when the B.L. acid donates its H+ proton ( i.e. HCl -> Cl-
Bronsted Lowery conjugate acid = the acid formed when the B.L. base accept its H+ proton ( i.e. NH4+ has accept H+ proton)
Note that, typically conjugate bases/acids are shown in the right (product) side
So, from your reaction:
H2Y- transforms to H3Y; it is gaining and H+, so it is a BASE
H2Z- transforms to HZ2-; it is losing H+, so it is an ACID
then,
H3Y is the conjugate ACID (since it could donate H+ to form H2Y-)
and HZ2- is the conjugate BASE ( since it could accept H+ to form H2Z-)
Lewis Acid/Base
Lewis acid and base theory deals mainly with electron transfer, rather than proton transfer (H+).
A Lewis acid will accept an electron pair
A Lewis base will donate an electron pair
Examples of a Lewis base:
Anything that will accept negatively charged species will do, such as halides, complex anions, etc…
Examples of a Lewis acid:
BH3, AlCl3, FeCl3, H+
Knowing all this....
A)
Ahrrenius base must be
NaOH, since it will donate OH- to solution
B)
Bronsted base will be:
NH3, since it can accept H+ from solution, to form
NH3 + H+ --> NH4+
C)
finally,
Br- is a lewis base, since it can donate electron pais
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