Question

Write Bronsted acid-base equilibrium equations for the following: b) Show the acid-base conjugated species, labeling all species c) Indicate if the species on the right or left of the reaction are favored/which way does the equilibrium lie?. Also can you explain why it shifts towards to the right or left? That's mostly the part I am having trouble understanding.

HSO4-   + HSO3-  < - >

HF + NO2-

H2CO3  + NH3

Answer 1

Bronsted acid-base equilibria

HSO4- (acid) + HSO3- (base) <==> SO4^2- (conjugate base) + H2SO3 (conjugate acid)

Equilibrium les to the right, so products are favoured. HSO4- is a stronger acid than HSO3-.

HF (acid) + NO2- (base) <==> F- (conjugate base) + HNO2 (conjugate acid)

Reactants are favored. HNO2 is a strogner acid than HF

H2CO3 (acid) + NH3 (base) <==> HCO3- (conjugate base) + NH4+ (conjugate acid)

Reactants are favoured. NH4+ is a strogner acid than H2CO3