Which of the following salt is alkaline in water

Options

A. `C Cl_(4)`
B. `O_(2)`
C. NaBr
D. `CHBr_(3)`

Explanation

To determine which of the given salts is alkaline in water, we need to analyze the nature of each salt based on the cation and anion it contains. An alkaline solution is one that has a pH greater than 7, indicating it is basic.

### Step-by-Step Solution:

1. **Identify the Salts**: The salts we need to analyze are CCl4, O2, NaBr, and CHBr3.

2. **Analyze CCl4**:
- Cation: C^4+
- Anion: Cl^-
- Chloride ion (Cl^-) comes from hydrochloric acid (HCl), which is a strong acid. Therefore, CCl4 will produce an acidic solution in water.

3. **Analyze O2**:
- O2 is a neutral molecule and does not dissociate into ions in water. Thus, it does not affect the pH of the solution. Therefore, O2 is neither acidic nor basic.

4. **Analyze NaBr**:
- Cation: Na^+
- Anion: Br^-
- Sodium ion (Na^+) comes from sodium hydroxide (NaOH), which is a strong base, and bromide ion (Br^-) comes from hydrobromic acid (HBr), which is a strong acid. Since Na^+ is from a strong base and Br^- is from a strong acid, the solution of NaBr will be neutral.

5. **Analyze CHBr3**:
- Cation: CHBr3^+
- Anion: Br^-
- The cation CHBr3^+ is derived from a weak base (since it is a brominated hydrocarbon) and the anion Br^- comes from a strong acid (HBr). This combination indicates that the solution will be acidic.

6. **Conclusion**:
- From the analysis, we find that CCl4 is acidic, O2 is neutral, NaBr is neutral, and CHBr3 is acidic. None of these salts produce an alkaline solution.

### Final Answer:
None of the provided salts are alkaline in water.