Final answer:
The correct way to prepare a solution with the desired volume and molarity is often to dilute a concentrated solution. However, in this scenario, none of the options accurately describe the proper dilution process to achieve 435 ml of 0.231 M sodium hydroxide. Proper dilution would involve measuring 435 ml of the existing solution and not adding any water, contrary to what options A through D suggest.
Step-by-step explanation:
To prepare a solution of a specific concentration from a more concentrated solution, you need to dilute the original solution with water. The important concept here is that molarity (M) times volume (V) equals moles of solute (n), which remains constant before and after the dilution. This relationship is commonly expressed as M1V1 = M2V2 where M1 and V1 are the molarity and volume of the initial solution, and M2 and V2 are the molarity and volume of the final solution.
Looking at the options presented in the question, options B and D would change the molarity of the original solution, which is not what we want. Option C is not appropriate because it involves adding a solution of a different concentration. Therefore, the correct preparation method is option A: Add 435 ml of water to 500 ml of 0.231 M sodium hydroxide.
However, there seems to be a misunderstanding in the question itself. To maintain the molarity of 0.231M but for a volume of 435ml, we would actually keep 435ml of the original solution and discard or use the other 65ml elsewhere. In this case, no water would be added since adding water would dilute the solution and change its molarity.
Based on precedent examples, such as Example 5.4.14 and similar scenarios in preparing solutions, we would dilute a known volume of a more concentrated solution to achieve the desired molarity and volume.