`H_(2)` can displace the metal from its aqueous solution.

Options

A. `Li^(+)`
B. `Sr^(2+)`
C. `A1^(3+)`
D. `Ag^(+)`

Explanation

To determine whether hydrogen gas (H₂) can displace a metal from its aqueous solution, we need to refer to the electrochemical series, which ranks elements based on their reactivity. Here’s a step-by-step solution:

### Step 1: Understand the Electrochemical Series
The electrochemical series is a list of elements arranged in order of their standard electrode potentials. The higher an element is in the series, the more reactive it is. Reactive metals can displace less reactive metals from their compounds in solution.

### Step 2: Identify the Position of Hydrogen
In the electrochemical series, hydrogen (H⁺) is positioned above certain metals like silver (Ag⁺). This means that hydrogen can displace metals that are below it in the series.

### Step 3: Identify Metals that Hydrogen Can Displace
To determine which metals can be displaced by hydrogen, we need to look at the metals that are positioned below hydrogen in the electrochemical series. According to the series, metals like Ag⁺ are below H⁺, which means that H₂ can displace Ag⁺ from its aqueous solution.

### Step 4: Conclusion
Based on the electrochemical series, hydrogen gas (H₂) can displace metals that are below it in the series, such as Ag⁺. Therefore, it can be concluded that H₂ can displace silver ions from an aqueous solution.

### Final Answer
Yes, H₂ can displace metals from their aqueous solutions, specifically those that are below it in the electrochemical series, such as Ag⁺.

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