To solve the question regarding NaCl, MgCl₂, and CaSO₄, we need to classify these compounds based on their electrolyte types. Let's break down the solution step by step.
### Step 1: Identify the dissociation of each compound
- **NaCl**: When dissolved in water, NaCl dissociates into Na⁺ and Cl⁻ ions.
- **MgCl₂**: When dissolved, MgCl₂ dissociates into Mg²⁺ and 2 Cl⁻ ions.
- **CaSO₄**: When dissolved, CaSO₄ dissociates into Ca²⁺ and SO₄²⁻ ions.
### Step 2: Determine the charge on cations and anions
- **NaCl**:
- Cation: Na⁺ (charge +1)
- Anion: Cl⁻ (charge -1)
- Type: 1:1 electrolyte
- **MgCl₂**:
- Cation: Mg²⁺ (charge +2)
- Anion: Cl⁻ (charge -1)
- Type: 2:1 electrolyte
- **CaSO₄**:
- Cation: Ca²⁺ (charge +2)
- Anion: SO₄²⁻ (charge -2)
- Type: 2:2 electrolyte
### Step 3: Classify the electrolytes
- **NaCl** is a 1:1 type electrolyte.
- **MgCl₂** is a 2:1 type electrolyte.
- **CaSO₄** is a 2:2 type electrolyte.
### Step 4: Evaluate the options given in the question
1. **1:1, 2:1, and 2:2 type electrolytes** - This option is correct based on our classification.
2. **Strong, weak, and strong electrolytes** - This option is incorrect because both NaCl and MgCl₂ are strong electrolytes.
3. **Electrolytes with different values of A** - This option is incorrect because the value of A (equivalent conductance) is dependent on concentration and temperature, not on the type of electrolyte.
4. **Electrolytes with same molar conductivity** - This option is incorrect because molar conductivity varies with the number of ions produced in solution.
### Conclusion
The correct classification for NaCl, MgCl₂, and CaSO₄ is that they are **1:1, 2:1, and 2:2 type electrolytes**, respectively.
### Final Answer
**NaCl, MgCl₂, and CaSO₄ are known as 1:1, 2:1, and 2:2 type electrolytes, respectively.**
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