Question

In which one of the following reactions does the nitric acid act a5 Bronsted-Lowry base? a.HNO; (&q) + H,0 () H;ot (1q) NO;" (aq) b.HNO, (aq) H" (aq) NO,-(4q) c.HNO; (aq) + 2H,SO (aq) NO; (aq) + 2HSO4- (aq) + H;O"(aq0

d.HNOz (a4) + CH COOH (a4 CH,COOH;" (aq) NO;- (4q)

Answer 1

The correct reaction where nitric acid acts as a Bronsted-Lowry base is option B: HNO3 (aq) + H2O (l) ⟶ H3O+ (aq) + NO3- (aq). Thus the correct option is B: HNO3 (aq) + H2O (l) ⟶ H3O+ (aq) + NO3- (aq).

Step-by-step explanation:

Nitric acid (HNO3) is a strong acid capable of donating a proton (H+) to other substances, typically behaving as a Bronsted-Lowry acid. However, in the given reaction, HNO3 accepts a proton (H+) from water (H2O), forming the hydronium ion (H3O+) and the nitrate ion (NO3-). This donation of a proton from water to nitric acid signifies the nitric acid acting as a Bronsted-Lowry base.

This reaction illustrates the behavior of nitric acid as it undergoes protonation from water, demonstrating its dual nature as both an acid and a base depending on the circumstances.

In the context of acid-base reactions, the Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Nitric acid is typically recognized as a strong acid due to its ability to donate a proton, but in certain scenarios, it can also act as a base by accepting a proton from another species. This dual nature of nitric acid showcases the versatility of acids and bases in different chemical environments. Thus the correct option is B: HNO3 (aq) + H2O (l) ⟶ H3O+ (aq) + NO3- (aq).

Answer 2

Nitric acid (HNO3) acts as a Brønsted-Lowry base in the reaction HNO3 (aq) + H+ (aq) → NO3- (aq), where it accepts a proton to form the conjugate base NO3-.

Step-by-step explanation:

The question is asking in which reaction nitric acid (HNO3) acts as a Brønsted-Lowry base. According to Brønsted-Lowry theory, a base is a proton acceptor. Among the given reactions, the one where HNO3 acts as a Brønsted-Lowry base is option b: HNO3 (aq) + H+ (aq) → NO3- (aq). In this reaction, HNO3 accepts a proton (H+) and forms its conjugate base (NO3-).

Net ionic equations that show other species acting as Brønsted-Lowry acids and bases are:

• HNO3 (aq) + H2O (l) → H3O+ (aq) + NO3- (aq) - HNO3 is an acid.
• NH3 (aq) + H2O (l) → NH4+ (aq) + OH- (aq) - NH3 is a base.
• H2S (aq) + H2O (l) → H3O+ (aq) + HS- (aq) - H2S is an acid.