You prepared a NaCl solution by adding 58.44 g NaCl to a 1-L volumetric flask and then adding w

step 1 So say you wanted to make a one molar solution of sodium chloride. And what you did was you took

You prepared a NaCl solution by adding 58.44 g NaCl to a...

You prepared a $\mathrm{NaCl}$ solution by adding $58.44 \mathrm{~g} \mathrm{NaCl}$ to a $1-\mathrm{L}$ volumetric flask and then adding water to dissolve it. When you were finished, the final volume in your flask looked like this: The solution you prepared is (a) Greater than $1 \mathrm{M}$ because you added more solvent than necessary. (b) Less than $1 \mathrm{M}$ because you added less solvent than necessary. (c) Greater than $1 \mathrm{M}$ because you added less solvent than necessary. (d) Less than $1 \mathrm{M}$ because you added more solvent than necessary. (e) $1 \mathrm{M}$ because the amount of solute, not solvent, determines the concentration.

You prepared a $\mathrm{NaCl}$ solution by adding $58.44 \mathrm{~g} \mathrm{NaCl}$ to a $1-\mathrm{L}$ volumetric flask and then adding water to dissolve it. When you were finished, the final volume in your flask
looked like this:
The solution you prepared is
(a) Greater than $1 \mathrm{M}$ because you added more solvent than necessary.
(b) Less than $1 \mathrm{M}$ because you added less solvent than necessary.
(c) Greater than $1 \mathrm{M}$ because you added less solvent than necessary.
(d) Less than $1 \mathrm{M}$ because you added more solvent than necessary.
(e) $1 \mathrm{M}$ because the amount of solute, not solvent, determines the concentration.

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Key Concepts

Molarity

Molarity is a measure of concentration defined as the number of moles of solute dissolved per liter of the total solution. It is calculated by dividing the number of moles of solute by the final volume of the solution, making it independent of the individual volumes of solute or solvent before mixing, as long as the final volume is accurately measured.

Volumetric Flask Calibration

A volumetric flask is a lab instrument calibrated to contain an exact volume when the solution reaches a marked level. This tool ensures precision in solution preparation because when the solute is dissolved and water is added until the calibration mark, the final volume accounted for includes both the solute and the solvent, thereby determining the correct molarity.

Solution Preparation Procedure

The process of accurately preparing a solution involves dissolving the solute completely and then adding solvent until the total volume matches the desired measurement mark. This method guarantees that any volume contribution from the solute is properly included in the final solution volume, ensuring that the calculated concentration is correct.

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