Which of the following is soluble in water ?

Options

A. `CS_2`
B. `C_2H_5OH`
C. `C C I_4`
D. `CHCI_3`.

Answer

To determine which of the given compounds is soluble in water, we need to analyze the polarity of each compound. Water is a polar solvent, and it generally dissolves polar substances. Here’s a step-by-step solution:

### Step 1: Identify the nature of water
Water (H₂O) is a polar solvent. This means that it can effectively dissolve other polar substances due to the principle of "like dissolves like."

**Hint:** Remember that polar solvents tend to dissolve polar solutes, while non-polar solvents dissolve non-polar solutes.

### Step 2: Analyze each option for polarity
1. **CS₂ (Carbon disulfide)**:
- CS₂ is a linear molecule and has a symmetrical structure, resulting in a net dipole moment of zero. Therefore, it is non-polar.
- **Conclusion**: CS₂ is not soluble in water.

2. **Alcohols**:
- Alcohols contain hydroxyl (-OH) groups which are polar due to the electronegativity difference between oxygen and hydrogen. This makes alcohols polar molecules.
- **Conclusion**: Alcohols are soluble in water.

3. **CCl₄ (Carbon tetrachloride)**:
- CCl₄ has a tetrahedral structure and is symmetrical, resulting in a net dipole moment of zero. Thus, it is non-polar.
- **Conclusion**: CCl₄ is not soluble in water.

4. **CHCl₃ (Chloroform)**:
- CHCl₃ has a polar C-Cl bond, resulting in a net dipole moment that is not zero. However, it is only slightly polar compared to water.
- **Conclusion**: CHCl₃ is slightly soluble in water but not completely.

### Step 3: Summarize the findings
Based on the analysis:
- CS₂: Not soluble in water (non-polar)
- Alcohols: Soluble in water (polar)
- CCl₄: Not soluble in water (non-polar)
- CHCl₃: Slightly soluble in water (slightly polar)

### Final Answer
The only compound that is soluble in water is **option number 2 (Alcohols)**.

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