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This question involves ranking solutions based on their pH, taking into account whether they are acidic, basic, or neutral. Here’s a step-by-step breakdown:

### Step 1: Analyzing the Acid and Base Constants (Ka and Kb)
- **Hydrocyanic acid (HCN)** has \( K_a = 4.9 \times 10^{-10} \).
- **Hypochlorous acid (HClO)** has \( K_a = 3.0 \times 10^{-8} \).
- **Aniline (C\(_6\)H\(_5\)NH\(_2\))** has \( K_b = 4.3 \times 10^{-10} \).
- **Ammonia (NH\(_3\))** has \( K_b = 1.8 \times 10^{-5} \).

The relative strengths of these acids and bases can help us predict the pH behavior of their corresponding salts.

### Step 2: Identifying the Nature of Each Salt Solution
1. **NaCN**:
   - NaCN is a salt of a weak acid (HCN) and a strong base (NaOH).
   - This salt will undergo hydrolysis to produce a basic solution.

2. **NH\(_4\)Br**:
   - NH\(_4\)Br is a salt of a weak base (NH\(_3\)) and a strong acid (HBr).
   - It will hydrolyze to form an acidic solution.

3. **KClO**:
   - KClO is a salt of a weak acid (HClO) and a strong base (KOH).
   - It will produce a basic solution upon hydrolysis.

4. **C\(_6\)H\(_5\)NH\(_3\)Cl**:
   - C\(_6\)H\(_5\)NH\(_3\)Cl is a salt of a weak base (aniline) and a strong acid (HCl).
   - This will produce an acidic solution.

### Step 3: Ranking the Solutions by pH
Based on the above:
1. **NH\(_4\)Br** and **C\(_6\)H\(_5\)NH\(_3\)Cl** are acidic, but NH\(_4\)Br should be slightly less acidic than C\(_6\)H\(_5\)NH\(_3\)Cl due to the stronger Kb of ammonia.
2. **NaCN** and **KClO** are basic, with NaCN expected to be more basic than KClO because HCN is a weaker acid than HClO.

Thus, the order from **lowest to highest pH** would be:
1. **C\(_6\)H\(_5\)NH\(_3\)Cl** (lowest pH, most acidic)
2. **NH\(_4\)Br**
3. **KClO**
4. **NaCN** (highest pH, most basic)

Would you like further explanation on each salt's hydrolysis behavior?

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### Related Questions
1. How do Ka and Kb values impact the acidity or basicity of a salt solution?
2. What is the role of hydrolysis in determining the pH of a salt solution?
3. Why does NaCN produce a basic solution while NH\(_4\)Br produces an acidic one?
4. How can we experimentally determine the pH of these salt solutions?
5. What are some real-life applications where pH control via salt solutions is crucial?

### Tip
To predict if a salt solution is acidic or basic, check the strength of the original acid and base that formed the salt; the stronger component often dictates the pH outcome.

Consider the data on weak acids and bases, and rank the solutions (0.1 M NaCN, 0.1 M NH4Br, 0.1 M KClO, 0.1 M C6H5NH3Cl) in order of increasing pH.

Analyze the acid-base properties of salts NaCN, NH4Br, KClO, and C6H5NH3Cl based on Ka and Kb values. Understand hydrolysis effects and rank solutions by pH, identifying the most acidic and most basic solutions.

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