Final answer:
In a neutralization reaction between 100 ml, 0.1 n H₂SO₄ and 100 ml, 0.1 m Ba(OH)2, both the acid and base will neutralize each other completely, resulting in a neutral solution with a pH of 7.
Step-by-step explanation:
To calculate the pH of the resulting solution when 100 ml, 0.1 n H₂SO₄ solution is mixed with 100 ml, 0.1 m Ba(OH)2 solution, we need to consider the neutralization reaction between the acid and the base. Barium hydroxide (Ba(OH)2) is a strong base and sulfuric acid (H₂SO₄) is a strong acid, which means they will react to form water and a salt, in this case, barium sulfate (BaSO4).
First, we need to find the number of moles of each reactant. Since both solutions have the same volume and concentration, and the reaction between H₂SO₄ and Ba(OH)2 occurs in a 1:1 ratio, they will fully neutralize each other. After the reaction, there will be no excess acid or base, resulting in a neutral pH of 7.
As a practical note, when a strong acid reacts with a strong base, the resulting solution's pH will typically be neutral if the acid and base are mixed in stoichiometrically equivalent amounts. This example does not take into account the minor effect of the autoionization of water on the pH, which is generally negligible in comparison to the concentration of the strong acid and base in the solution.