Which equation represents for the solution of `H_(2)S` in water?

Options

A. `[H^(+)]=2[S^(-2)]+[HS^(-)]+[OH^(-)]`
B. `[H^(+)]=[OH^(-)]`
C. `[H^(+)]=[S^(-2)]+[HS^(-)]+[H^(+)]`
D. `[H^(+)]=[S^(-2)]+[HS^(-)]+[OH^(-)]`

Answer

To determine which equation represents the solution of hydrogen sulfide (H₂S) in water, we can follow these steps:

### Step 1: Understand the Dissociation of H₂S in Water
When hydrogen sulfide (H₂S) is dissolved in water, it can dissociate into ions. The dissociation can be represented as follows:
\[ \text{H}_2\text{S} \rightleftharpoons \text{H}^+ + \text{HS}^- \]
This indicates that one molecule of H₂S produces one hydrogen ion (H⁺) and one hydrosulfide ion (HS⁻).

### Step 2: Consider the Ionization of Water
In pure water, water molecules also dissociate into ions:
\[ \text{H}_2\text{O} \rightleftharpoons \text{H}^+ + \text{OH}^- \]
This shows that water produces hydrogen ions (H⁺) and hydroxide ions (OH⁻).

### Step 3: Combine the Dissociation Equations
When H₂S is dissolved in water, the overall reaction can be represented as:
\[ \text{H}_2\text{S} + \text{H}_2\text{O} \rightleftharpoons \text{H}^+ + \text{HS}^- + \text{OH}^- \]
This equation shows that H₂S contributes to the concentration of H⁺ ions in the solution, while water contributes both H⁺ and OH⁻ ions.

### Step 4: Charge Balance
In any solution, the total positive charge must equal the total negative charge. In this case, the positive charges come from H⁺ ions, and the negative charges come from HS⁻ and OH⁻ ions. Therefore, the equation must balance in terms of charge.

### Step 5: Identify the Correct Option
Based on the dissociation of H₂S and the ionization of water, the correct equation representing the solution of H₂S in water will be the one that shows the formation of H⁺, HS⁻, and OH⁻ ions while maintaining charge balance.

### Conclusion
The correct equation that represents the solution of H₂S in water is:
\[ \text{H}_2\text{S} + \text{H}_2\text{O} \rightleftharpoons \text{H}^+ + \text{HS}^- + \text{OH}^- \]

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