With the help of equation show that the aqueous solution of hydrogen carbonate is acidic.
To show that the aqueous solution of hydrogen carbonate (HCO3-) is acidic, we can look at the dissociation of hydrogen carbonate in water and the resulting equilibrium equation.
The dissociation of hydrogen carbonate in water can be represented by the following equation:
HCO3-(aq) ⇌ H+(aq) + CO3^2-(aq)
In this equation, hydrogen carbonate (HCO3-) reacts with water (H2O) to produce hydronium ions (H+, or protons) and bicarbonate ions (CO3^2-).
The equilibrium equation for this reaction can be written as:
HCO3-(aq) + H2O(l) ⇌ H+(aq) + CO3^2-(aq)
In an aqueous solution of hydrogen carbonate, the forward reaction represents the dissociation of hydrogen carbonate ions into hydronium and bicarbonate ions. This means that some of the hydrogen carbonate ions are converted into H+ ions, which are responsible for the acidic properties of the solution.
The presence of H+ ions in solution indicates acidity, as they can donate a proton (H+) to water or other substances, leading to acidic behavior.
Therefore, by considering the equilibrium equation and the presence of H+ ions, we can conclude that the aqueous solution of hydrogen carbonate is acidic.
The equation for the dissociation of hydrogen carbonate (HCO3-) in water is as follows:
HCO3- + H2O ⇌ H3O+ + CO32-
In this equation, hydrogen carbonate (HCO3-) reacts with water (H2O) to form a hydronium ion (H3O+) and a carbonate ion (CO32-).
The presence of hydronium ions (H3O+) in the solution indicates that it is acidic. The hydronium ions are responsible for the acidic properties of the solution, as they increase the concentration of protons (H+) in the solution.
Therefore, by the presence of H3O+ ions, we can conclude that the aqueous solution of hydrogen carbonate is acidic.