What is the correct increasing order of the pH of the following solutions with equal concentrations?

Options

A. `HClltNaOHltCH_(3)COOH`
B. `HClltCH_(3)COOHltNaOH`
C. `NaOHltHClltCH_(3)COOH`
D. `CH_(3)COOHltNaOHltHCl`

Answer

To determine the correct increasing order of pH for the given solutions (HCl, NaOH, and CH3COOH) with equal concentrations, we need to analyze the nature of each solution:

### Step-by-step Solution:

1. **Identify the nature of each solution:**
- **HCl (Hydrochloric acid)**: This is a strong acid. Strong acids completely dissociate in water, resulting in a low pH.
- **NaOH (Sodium hydroxide)**: This is a strong base. Strong bases completely dissociate in water, resulting in a high pH, close to 14.
- **CH3COOH (Acetic acid)**: This is a weak acid. Weak acids do not completely dissociate in water, resulting in a pH that is higher than strong acids but lower than neutral (7).

2. **Determine the pH values:**
- Since HCl is a strong acid, it will have the lowest pH value among the three solutions.
- NaOH, being a strong base, will have the highest pH value.
- CH3COOH, as a weak acid, will have a pH value that is higher than HCl but lower than NaOH.

3. **Establish the order of pH values:**
- Based on the analysis:
- HCl < CH3COOH < NaOH
- This means that the pH of HCl is the lowest, followed by the pH of CH3COOH, and finally the pH of NaOH is the highest.

4. **Conclusion:**
- The correct increasing order of the pH of the solutions is:
- HCl < CH3COOH < NaOH

### Final Answer:
The correct increasing order of the pH of the solutions is:
**HCl < CH3COOH < NaOH**