If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?(a) 50.0 mL of 0.100 M HBr and 30.0 mL of 0.200 M KOH

Acid-base reactions involve the transfer of protons (H+) between substances. In this case, HBr is a strong acid that dissociates completely in solution, releasing H+ ions, while KOH is a strong base that dissociates to produce OH- ions. The reaction between H+ and OH- leads to the formation of water, which is crucial for determining the acidity or basicity of the resulting solution.

To analyze the resulting solution's pH, it is essential to calculate the moles of H+ and OH- present after mixing. This involves using the concentration (Molarity) and volume of each solution to find the total moles of acid and base. The stoichiometry of the reaction will help determine if there is an excess of H+ or OH-, which dictates whether the solution is acidic, basic, or neutral.

Neutralization is the process where an acid and a base react to form water and a salt, typically resulting in a solution that is neutral (pH 7) if equal moles of acid and base are present. In this scenario, determining whether the moles of H+ from HBr equal the moles of OH- from KOH will indicate if the solution is neutral, acidic, or basic after the reaction.