How would you prepare 250 mL of a 0.325 M solution of benzoic acid 1C7H6O22 in chloroform 1CHCl32?

Verified step by step guidance

1. Determine the molar mass of benzoic acid (C7H6O2) by adding the atomic masses of all the atoms in the formula.
2. Calculate the number of moles of benzoic acid needed using the formula: \( \text{moles} = \text{molarity} \times \text{volume in liters} \).
3. Convert the volume from milliliters to liters by dividing by 1000.
4. Calculate the mass of benzoic acid required using the formula: \( \text{mass} = \text{moles} \times \text{molar mass} \).
5. Weigh the calculated mass of benzoic acid and dissolve it in chloroform to make up a total volume of 250 mL.

Key Concepts

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. To prepare a solution, you need to know the desired molarity and the volume of the solution. In this case, a 0.325 M solution means there are 0.325 moles of benzoic acid in every liter of the solution. For 250 mL, you would calculate the moles needed based on this concentration.

Dilution and Solution Preparation

Preparing a solution involves dissolving a specific amount of solute in a solvent to achieve the desired concentration. In this scenario, you would weigh the appropriate mass of benzoic acid and then dissolve it in chloroform to reach a final volume of 250 mL. Understanding how to accurately measure and mix solutions is crucial for achieving the correct molarity.

Benzoic Acid and Chloroform Properties

Benzoic acid (C7H6O2) is a weak organic acid, while chloroform (CHCl3) is a non-polar solvent. The solubility of benzoic acid in chloroform is important to consider, as it affects how well the acid will dissolve. Knowing the properties of both the solute and solvent helps in predicting the behavior of the solution and ensuring that the desired concentration is achieved.