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

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

Verified step by step guidance

Calculate the moles of HBr using the formula: moles = concentration \(\times\) volume.

Calculate the moles of KOH using the formula: moles = concentration \(\times\) volume.

Compare the moles of HBr and KOH to determine which one is in excess.

If HBr is in excess, the solution is acidic. If KOH is in excess, the solution is basic. If they are equal, the solution is neutral.

Use the stoichiometry of the reaction HBr + KOH \(\rightarrow\) KBr + H_2O to understand the neutralization process.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Reactions

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.

Concentration and Volume Calculations

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

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.

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