Question

Identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid and the conjugate base for each of the following reactions.

1. H2CO3(aq) + H2O+(aq) <-----> H3O+(aq) + HCO3-(aq)

2. NH3(aq) + H2O(l) <-----> NH4+ (aq) + OH -(aq)

3. HNO3 (aq) <-----> H2O(l) H3O+(aq) + NO3- (aq)

4. C5H5N (aq) + H2O(l) <-----> C5H5NH+(aq) + OH- (aq)

Answer 1

1. H₂CO_3(aq) + H₂O_(aq) H₃O⁺_(aq) + HCO₃^-_(aq)

Bronsted-Lowry acid - H₂CO_3(aq)

Bronsted-Lowery base -  H₂O_(aq)

conjugate acid - H₃O⁺_(aq)

conjugate base -  HCO₃^-_(aq)

2. NH_3(aq) + H₂O_(l) NH₄⁺_(aq) + OH^-_(aq)

Bronsted-Lowry acid -  H₂O_(l)

Bronsted-Lowery base - NH_3(aq)

conjugate acid - NH₄⁺_(aq)

conjugate base - OH^-_(aq)

3. HNO_{3 (aq)} + H₂O_(l) H₃O⁺_(aq) + NO₃^-_(aq)

Bronsted-Lowry acid - HNO_{3 (aq)}

Bronsted-Lowery base - H₂O_(l)

conjugate acid - H₃O⁺_(aq)

conjugate base - NO₃^-_(aq)

4. C₅H₅N _(aq) + H₂O(l) C₅H₅NH⁺_(aq) + OH^-_(aq)

Bronsted-Lowry acid - H₂O(l)

Bronsted-Lowery base - C₅H₅N _(aq)

conjugate acid - C₅H₅NH⁺_(aq)

conjugate base - OH^-_(aq)

According to bronsted-lowery theory acid are species those give hydrogen ion to another species and base are those accept hydrogen ion.