[VISUAL] Of the three solutions listed in the table above, which one, if any, has the greatest elect — Solutions Chemistry Question

STEPS:

1. Identify the core chemical concept tested:
The question tests your understanding of the electrical conductivity of aqueous solutions. For a solution to conduct electricity, it must contain mobile, charged particles (ions) that can move freely through the solvent to carry an electrical current.

2. Analyze each of the three solutes to determine its behavior in water:
* $\text{HC}_2\text{H}_3\text{O}_2$ (Acetic acid): This is a weak organic acid. When dissolved in water, it only partially dissociates into $\text{H}^+$ and $\text{C}_2\text{H}_3\text{O}_2^-$ ions, meaning the vast majority of the molecules remain intact and uncharged. It is a weak electrolyte.
* $\text{KI}$ (Potassium iodide): This is a highly soluble ionic salt. When dissolved in water, it dissociates completely into its component potassium ions ($\text{K}^+$) and iodide ions ($\text{I}^-$). It is a strong electrolyte.
* $\text{CH}_3\text{OH}$ (Methanol): This is a covalent molecular compound. Although it is polar and dissolves well in water, it does not dissociate into ions. It is a non-electrolyte.

3. Compare the concentration of mobile ions in each solution:
Because all three solutions share the same initial solute concentration of $0.1\text{ M}$:
* The $0.1\text{ M KI}(aq)$ solution undergoes complete dissociation to produce a high concentration of free ions ($\approx 0.2\text{ M}$ total ions).
* The $0.1\text{ M HC}_2\text{H}_3\text{O}_2(aq)$ solution yields a very low concentration of free ions due to limited dissociation.
* The $0.1\text{ M CH}_3\text{OH}(aq)$ solution yields virtually zero free ions.

4. Conclude which solution has the highest conductivity:
The potassium iodide solution, $\text{0.1 M KI}(aq)$, has by far the highest concentration of mobile ions and will therefore exhibit the greatest electrical conductivity. This corresponds directly to Option B.

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WHY_OTHERS_WRONG:

• Option A is incorrect: The number of atoms within a molecule does not determine its electrical conductivity. Even though acetic acid ($\text{HC}_2\text{H}_3\text{O}_2$) has more atoms per molecule than $\text{KI}$, it is a weak electrolyte that only dissociates to a very small extent, making it a much weaker conductor.
• Option C is incorrect: While methanol ($\text{CH}_3\text{OH}$) molecules can form hydrogen bonds with water, hydrogen bonding only explains solubility, not conductivity. Because methanol molecules do not dissociate into charged ions, the solution cannot carry an electrical current.
• Option D is incorrect: While the analytical concentrations of the solutes are identical, their dissociation behaviors are fundamentally different. Electrical conductivity depends heavily on whether a solute is a strong, weak, or non-electrolyte, not just its concentration.