Pollution from fireworks occurs in a number of ways, one of which is the release of gases such as carbon dioxide (CO2) and sulfur dioxide (SO2) into the environment. These gases react further in the atmosphere to produce carbonic acid (H2CO3), a weak acid, and sulfuric acid (H2SO4) a strong acid. If the same number of moles of each of these acids were dissolved in equal volumes of water, how can I state and explain which of the resulting solutions would have the higher pH. Has this to do with the fact in weak acids the equilibrium lies well over to the left-hand side of the equation? But what does it means? Furthermore, which changes take place when each compound is dissolved in water? What are the two equations? Is the equilibrium state dynamic? This is what I was thinking but I feel like something is missing: The acid concentration of both compounds dissolved in water is the same, but sulfuric acid will have a higher pH and is therefore a stronger acid than carbonic acid. This is because the concentration of the ions for carbonic acid is lower compared with that of the sulfuric acid, which dissolves in water better. In the dissociation of sulfuric acid, more molecules dissociate into hydrogen ions than in the carbonic acid. In both acids the concentration of hydrogen ions exceeds the concentration of hydroxide ions, but in sulfuric acid is greater than in carbonic acid. When each compound is dissolved in water, their molecules are separated from one another and they change their original state into aqueous. Their equilibrium state is dynamic, in fact for both acids molecules are continuously breaking down into Bicarbonate/Sulfate ions and Hydronium ions and this is balanced by the reverse reaction where Bicarbonate/Sulfate ions and Hydronium ions recombining to give acetic and carbonic acid molecules. H2CO3 (aq) + H2O (l) ⇌ H3O+ (aq) + HCO3− (aq) H2SO4 (aq) + H2O (l) ⇌ H3O+ (aq) + HSO4− (aq) Thanks!