What would be the pH of a solution that liberates carbon dioxide from sodium carbonate. Give chemical equation and reason
Na2CO3 + 2H^+ ==> 2Na^+ + CO2 + H2O
The pH must be <7.0
thanks sir..
To determine the pH of a solution that liberates carbon dioxide from sodium carbonate, we need to understand the chemical equation and the behavior of the reactants.
The chemical equation for the reaction of sodium carbonate (Na2CO3) liberating carbon dioxide (CO2) can be represented as follows:
Na2CO3 + 2HCl -> 2NaCl + H2O + CO2
In this equation, sodium carbonate (Na2CO3) reacts with hydrochloric acid (HCl) to form sodium chloride (NaCl), water (H2O), and carbon dioxide (CO2). This reaction is known as a neutralization reaction.
The liberating of carbon dioxide occurs because sodium carbonate is a basic compound and reacts with the strong acid, hydrochloric acid, to form carbon dioxide gas. Carbon dioxide is a weak acid, and when it dissolves in water, it forms carbonic acid (H2CO3), which lowers the pH of the solution.
The pH scale ranges from 0 to 14, where a pH of 7 is considered neutral, values below 7 are acidic, and values above 7 are basic. Since the reaction between sodium carbonate and hydrochloric acid produces carbonic acid, which is a weak acid, the pH of the solution would be lower than 7. However, the exact pH value would depend on the concentration of the reactants and other factors like temperature.
To determine the actual pH of the solution, you would need to perform a pH measurement using a pH meter or pH indicator paper.