In: Chemistry
For each of the following molecules, determine if they are acids or bases in the presence of water AND which definition (Arrhenius, Bronsted-Lowry, or Lewis) applies to each. [Note: Some molecules may fit multiple definitions.]
NO
H2S
Ca(OH)2
MgO
(COOH)2
BCl3
NH4+
C5H5N
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
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)
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
Kowing all thesee... we cna proceed further:
NO --> H2O + NO --> HNO2 + H+ --> ahrrenius acid, brosnted acid
H2S --> Arrhenius; since it donates H+, Bronsted, since it donates H+; lewis
Ca(OH)2 --> ahrrenius base, since it donates OH-
MgO --> MgO + H2O -> Mg(OH)2 + H2 --> if donates OH- then an ahrrenius base
(COOH)2 --> bronsted acid, ahreenius acid, donates H+
BCl3 --> Lewis acid, since it accepts lone pairs
NH4+ --> Arrhenius; since it donates H+, Bronsted, since it donates H+; lewis
C5H5N --> Bronsted base, since it accepts H+