Question

6. There are two major theories of acids and bases in aqueous solutions: Arrhenius and Bronsted. a) In your own words, briefly explain the main difference between the two theories of acids and bases b) Which theory do you think is the most useful in chemistry? Explain your choice. c) Which of the following is an Arrhenius acid? A) H2SO4: B) LiOH; C) NH2CH3; D) CH3CH3; E) More than one of these is an Arrhenius acid. d) Which of the following is a Brønsted-Lowry acid? A) NH4+; B) CH4; C) NH2-D) NH3; E) Br2 e) Which of the following is a Brønsted-Lowry base? A) CH4: B) HCN; C) NH3; D) CI2; E) None of the above are Brønsted-Lowry bases. T i mante coid baconaire in the folloinntir

Answer 1

a )*According to arhenius theory an acid is a species which dissociate to form H+ in aqous solution .While according to bronsted theory and acid is a species that donate proton to another substance

* Bronsted Lowery bases are any substance that dissociate to form OH- in aqous solution .

Arhenius bases are any species that accept an proton

b) the bronsted theory is more useful than arhenius theory .

Arhenius could not classify substance unless they are dissolved in water . His defination of acids and bases are basically rely upon these substances dissociating in aqous solution . His theory also not explains why some substance which contains Hydrogen like HCl dissolve in water and gives H+ while CH4 not .

C) among the given options only H2So4 is an arhenius acid as it gives H+ in aqous solution.

H2So4 ↔️ H^+ + HSO4^-

D) Bronsted Lowery bases is

NH4+

NH4+ ↔️ NH3 + H+

E) among all given options only NH3 is proton accepter so it is bronsted base