Part A

Classify each of these compounds as an Arrhenius acid, an Arrhenius base, or neither.

C2H6, Ba(OH)2, H2SO4, AgOH, H3PO3, HCL, Mn(OH)2, HI, KCI, KOH

Part B

Classify each of these compounds as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither

HNO3, HF, HNO2, (CH3)2NH, C3H7NH2, NH3, NaBr, CH2CI2

Answer:

Arrhenius acid --> will donate H+

Arrhenius base --> will donate OH-

C2H6 --> could donate H+ to form C2H5- (not likely) but it could happen.... this exercise will likely take "neither" as an answer

Ba(OH)2 --> Ahrrenius base, since OH will be donated

H2SO4 --> Arrhenius acid, 2H+ available

AgOH --> Arrhenius base, since OH- is present

H3PO3 --> Arrhenius acid, 3H+ present

HCL--- > Arrhenius acid, H+ will be donated

Mn(OH)2 --> Arrhenius base, OH-

HI --> H+ + I-, so Arrhenius aci

KCI; neutral, none

KOH --Arrhenius base, donate OH-

B)

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+)

HNO3 --> Donates H+Brønsted-Lowry acid

HF --> donates H+Brønsted-Lowry acid

HNO2 --> donates H+Brønsted-Lowry acid

(CH3)2NH --> accepts H+, (CH3)2NH2+

C3H7NH2 --> accepts H+, Brønsted-Lowry base

NH3 --> NH4+ + OH-. Brønsted-Lowry base

NaBr = neutral

CH2CI2 = neutral