Maximum Conductivity is observed for the following aqueous ion.

Options

A. `K^(+)`
B. `NA^(+)`
C. `Li^(+)`
D. `H^(+)`

Explanation

To determine which aqueous ion exhibits maximum conductivity, we need to consider the factors that influence conductivity, primarily the mobility of the ions in solution. Here’s a step-by-step solution:

### Step 1: Understand Conductivity
Conductivity in an aqueous solution is influenced by the concentration of ions and their mobility. Mobility refers to how easily ions can move through the solution, which is affected by their size and charge.

**Hint:** Remember that smaller ions generally have higher mobility because they can move more freely in the solution.

### Step 2: Analyze Ion Sizes
Consider the ions in question: H⁺, Li⁺, Na⁺, and K⁺. As we move down the group in the periodic table, the size of the ions increases due to the addition of electron shells.

**Hint:** Compare the sizes of the ions. Which one is the smallest?

### Step 3: Compare Mobilities
Since smaller ions can move more easily, we can infer that H⁺ (hydrogen ion) will have the highest mobility among the ions listed because it is the smallest.

**Hint:** Recall that the mobility of an ion is inversely related to its size.

### Step 4: Conclude on Conductivity
Given that H⁺ has the smallest size and thus the highest mobility, it will also have the maximum conductivity in an aqueous solution compared to Li⁺, Na⁺, and K⁺.

**Hint:** Think about how the size of an ion affects its ability to conduct electricity in a solution.

### Final Answer
The aqueous ion that exhibits maximum conductivity is **H⁺** (hydrogen ion).