What is the correct relationship between the pH of isomolar solutions of sodium oxide `(pH_(1))`, sodium sulphide `(pH_(2))`, sodium selenide `(pH_(3))` , and sodium telluride `(pH_(4)) ` ?

Options

A. `pH_(1)gt pH_(2)~~pH_(3)gt pH_(4)`
B. `pH_(1)lt pH_(2)lt pH_(3) lt pH_(4)`
C. `pH_(1)lt pH_(2)lt pH_(3)~~ pH_(4)`
D. `pH_(1)gt pH_(2)gt pH_(3)gtpH_(4)`

Explanation

To determine the correct relationship between the pH of isomolar solutions of sodium oxide (Na2O), sodium sulfide (Na2S), sodium selenide (Na2Se), and sodium telluride (Na2Te), we need to analyze the basicity of their corresponding anions.

### Step-by-Step Solution:

1. **Identify the Anions**:
- Sodium oxide (Na2O) yields the oxide ion (O²⁻).
- Sodium sulfide (Na2S) yields the sulfide ion (S²⁻).
- Sodium selenide (Na2Se) yields the selenide ion (Se²⁻).
- Sodium telluride (Na2Te) yields the telluride ion (Te²⁻).

2. **Determine Basicity of Anions**:
- The basicity of these anions can be compared based on their ability to accept protons (H⁺). The stronger the base, the higher the pH of the solution.
- The order of basicity for these anions is as follows:
- O²⁻ (oxide) > S²⁻ (sulfide) > Se²⁻ (selenide) > Te²⁻ (telluride)

3. **Relate Basicity to pH**:
- Since the solutions are isomolar, the concentration of each anion is the same. Therefore, the anion with the highest basicity will result in the highest pH.
- Based on the order of basicity established in the previous step, we can assign pH values:
- pH₁ (for O²⁻) > pH₂ (for S²⁻) > pH₃ (for Se²⁻) > pH₄ (for Te²⁻)

4. **Conclusion**:
- The correct relationship between the pH values is:
- pH₁ > pH₂ > pH₃ > pH₄

### Final Answer:
- The correct relationship is: **pH₁ > pH₂ > pH₃ > pH₄**.