In the reaction between a strong acid and a weak base, what is the resulting condition of the solution?

In the reaction between a strong acid and a weak base, the strong acid donates protons (H⁺ ions) to the weak base. This process results in the formation of a conjugate acid from the weak base and, because the strong acid fully dissociates in solution, it contributes a significant concentration of hydrogen ions.

Since the weak base does not provide as many hydroxide ions to neutralize the added protons, the solution as a whole shifts towards higher acidity. As a result, the pH of the solution decreases, indicating a more acidic condition. The dynamic nature of the reaction also means that upon the complete reaction of the strong acid with the weak base, there will be an excess of hydrogen ions compared to hydroxide ions, which reinforces the acidic nature of the solution.

In contrast, other outcomes such as increased basicity, neutrality, or an equilibrium state are not accurate because of the inherent strength difference between the strong acid and the weak base. The strong acid will dominate the reaction, ultimately leading to a solution that is acidic.