You are being interviewed for a high paying laboratory position. Your final interview question is this. "Explain in detail how you would go about preparing 1.00L of a 1.00 M solution of sodium chloride."

Question

You are being interviewed for a high paying laboratory position.  Your final interview question is this.  "Explain in detail how you would go about preparing 1.00L of a 1.00 M solution of sodium chloride."

BlackTom AI · Accepted Answer

The prompt presents a single multiple-choice option, but the provided data shows no list of alternative choices to evaluate alongside the given answer. This means we cannot compare multiple approaches or identify incorrect methods from a set of distractors; instead, we can focus on what the single listed method suggests and why it aligns with standard procedures for preparing a 1.00 L of 1.00 M NaCl solution.

First, the task is to prepare 1.00 L of a 1.00 M solution of sodium chloride. The target number of moles needed is calculated by multiplying the desired volume by the desired molarity: 1.00 L × 1.00 mol/L = 1.00 mol NaCl.

The option states to weigh out 58.44 g of NaCl, which is correct because the molar mass of NaCl is 58.44 g/mol, so 1.00 mol corresponds to 58.44 g. The next step is dissolving the salt in less than 1.00 L of deionized water in a beaker and then transferring the solution to a 1.00 L volumetric flask, rinsing the beaker with water and adding the rinses to the flask. This practice helps ensure all salt is transferred and collected in the final mixture, minimizing losses.

Finally, adding deionized water up to the calibration (volume) line and mixing thoroughly is the standard approach for achieving an accurate final volume of 1.000 L. The emphasis on using a volumetric flask is important because it provides a precise 1.000 L total volume, which is essential for attaining exactly 1.00 M concentration.

If we consider potential caveats or common pitfalls that are not explicitly listed in the option, one might note the following: ensure the volume is truly 1.000 L, not 1.2 L or 0.9 L, which would yield a different molarity; use an analytical balance with adequate precision to weigh 58.44 g; ensure the solution is homogeneous after final dilution; and consider temperature effects on volume, though for aqueous solutions at moderate temperatures, this is typically within acceptable tolerances for a standard lab preparation.

Since there are no additional answer options provided to critique or compare, we cannot identify a specific incorrect method within a set of alternatives. However, if there were mistakes to flag, they would typically include miscalculating the required mass, diluting to a volume incorrectly (e.g., to 1.00 L without using a volumetric flask, or neglecting to account for trace losses in transfer), or using an inaccurate balance or impure water that would alter the final concentration.

In summary, the described steps in the provided answer align with standard laboratory practice for preparing 1.00 L of 1.00 M NaCl: compute moles, weigh the correct mass, transfer carefully, and dilute to exactly 1.000 L in a volumetric flask with thorough mixing.

You are being interviewed for a high paying laboratory position. Your final interview question is this. "Explain in detail how you would go about preparing 1.00L of a 1.00 M solution of sodium chloride."

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