When ammonia gas (NH3) is bubbled through water that contains a few drops of phenolphthalein indicator, the water turn pink.Explain how the Bronsted Lowry theory of acids and bases can account for this observation,supporting your response with a chemical equation
The Brønsted-Lowry theory is frequently similarly joined with solution water
HCl(aq) + H2O (l) → H3O+(aq) +Cl−(aq)
NH3(aq) + HCl(aq) → NH4+(aq) + Cl−(aq)
Explanation:
Brønsted-Lowry theory
The Brønsted-Lowry theory is frequently similarly joined with solution water. Diffusing an acid in liquid to produce the hydronium ion and the anion of the acid is an acid-base effect. Acids are categorized as active or weak, depending on whether the stability favors the reactants or products. Hydrochloric acid, a strong acid, ionizes thoroughly in water to develop the hydronium and chlorine (Cl−) ions in a product-favored response.
HCl(aq) + H2O (l) → H3O+(aq) +Cl−(aq)
Using the Brønsted-Lowry theory, the effect of ammonia and hydrochloric acid in water is represented by the following equation:
NH3(aq) + HCl(aq) → NH4+(aq) + Cl−(aq)
Hydrochloric acid and the chlorine ion are one conjugate acid-base pair, and the ammonium ion and ammonia are the other. The acid-base reaction is the variation of the hydrogen ion from the acid (HCl) to the base (NH3). The equilibrium supports the more debilitated acid and base, in this case, the products.
