Acetic acid and sodium hydrogen sulfate are mixed in water.
a) Write a balanced net ionic equation for the transfer of one proton in this Bronsted-Lowry acid base reaction (include only species that take part in the reaction).
b) Label the acid, base, conjugate acid, conjugate base, and conjugate acid-base pairs.
c) Which will be favored at equilibrium, reactants or products? Explain your reasoning.
Solution
molecular equation,
CH3COOH(aq) + NaHSO4(aq) ------> CH3COONa(aq) + H2SO4(aq)
Net ionic equation with respect to Bronsted acid base theory,
H+(aq) + HSO4-(aq) ------> H2SO4(aq)
CH3COO-(aq) + Na+(aq) ------> CH3COONa(aq)
CH3COOH(aq)Â Â + NaHSO4(aq) ------> CH3COONa(aq)Â Â + H2SO4(aq)
Bronsted acid   Bronsted Base     Conjugate base   conjugate acid
Since Acetic acid is a weak electrolyte so it can dissociates weakly compare to NaHSO4 and further CH3COONa and H2SO4 are strong electrolytes they can easily dissociates into ions. so the reaction shifts generally to backward direction. i.e., reactants side.
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Acetic acid and sodium hydrogen sulfate are mixed in water- a) Write a.docx
1. Acetic acid and sodium hydrogen sulfate are mixed in water.
a) Write a balanced net ionic equation for the transfer of one proton in this Bronsted-Lowry acid
base reaction (include only species that take part in the reaction).
b) Label the acid, base, conjugate acid, conjugate base, and conjugate acid-base pairs.
c) Which will be favored at equilibrium, reactants or products? Explain your reasoning.
Solution
molecular equation,
CH3COOH(aq) + NaHSO4(aq) ------> CH3COONa(aq) + H2SO4(aq)
Net ionic equation with respect to Bronsted acid base theory,
H+(aq) + HSO4-(aq) ------> H2SO4(aq)
CH3COO-(aq) + Na+(aq) ------> CH3COONa(aq)
CH3COOH(aq)Â Â + NaHSO4(aq) ------> CH3COONa(aq)Â Â + H2SO4(aq)
Bronsted acid   Bronsted Base     Conjugate base   conjugate acid
Since Acetic acid is a weak electrolyte so it can dissociates weakly compare to NaHSO4 and
further CH3COONa and H2SO4 are strong electrolytes they can easily dissociates into
ions. so the reaction shifts generally to backward direction. i.e., reactants side.
