If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?(a) 65.0 mL of 0.0500 M HClO4 and 40.0 mL of 0.0750 M NaOH

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Calculate the moles of HClO_4 using the formula: moles = concentration \times volume.

Calculate the moles of NaOH using the formula: moles = concentration \times volume.

Compare the moles of HClO_4 and NaOH to determine which is in excess.

If HClO_4 is in excess, the solution is acidic. If NaOH is in excess, the solution is basic. If they are equal, the solution is neutral.

Conclude the nature of the resulting solution based on the excess reactant.

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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 reactants. In this case, HClO4 is a strong acid that dissociates completely in solution, while NaOH is a strong base that also dissociates completely. The reaction between them will produce water and a salt, and the resulting pH will depend on the relative amounts of acid and base present.

Molarity and Volume Calculations

Molarity (M) is a measure of concentration defined as moles of solute per liter of solution. To determine the resulting pH after mixing the solutions, one must calculate the moles of HClO4 and NaOH using their molarity and volumes. This allows for the assessment of which reactant is in excess and thus influences the final acidity or basicity of the solution.

Neutralization and pH

Neutralization occurs when an acid and a base react to form water and a salt, typically resulting in a solution with a pH close to 7 if they are present in stoichiometric amounts. If one reactant is in excess, the solution will be acidic or basic depending on whether the acid or base is in greater quantity. The final pH can be determined by comparing the moles of acid and base after mixing.

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