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### 1. Problem Overview
You are given a **table with weak acids and weak bases**, including their **Ka** (acid dissociation constant) or **Kb** (base dissociation constant). The goal is to **rank the pH of four solutions** (NaCN, NH4Br, NaCl, and C2H5NH3Cl) in **increasing order of pH** (i.e., from lowest to highest).

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### 2. Analyzing the Solutions
Each solution will contain a salt that influences the pH, depending on whether it forms acidic, basic, or neutral solutions. Let’s break each salt down:

- **0.1 M NaCN**:
  - CN⁻ is the conjugate base of **HCN** (a weak acid).
  - NaCN will produce a **basic solution** because CN⁻ will hydrolyze water to form OH⁻.
  
- **0.1 M NH4Br**:
  - NH4⁺ is the conjugate acid of **NH3** (a weak base).
  - NH4Br will produce an **acidic solution** because NH4⁺ will donate protons (H⁺) to water.

- **0.1 M NaCl**:
  - Na⁺ and Cl⁻ come from a **strong base (NaOH)** and **strong acid (HCl)**, respectively.
  - This solution will be **neutral**, with a pH ≈ 7.

- **0.1 M C2H5NH3Cl**:
  - C2H5NH3⁺ is the conjugate acid of **ethylamine** (C2H5NH2, a weak base).
  - This salt will produce an **acidic solution** since C2H5NH3⁺ will donate protons to water.

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### 3. Expected pH Ranking
Now, let's rank the pH of these solutions based on their acidic or basic nature:

1. **NH4Br** (most acidic, lowest pH)
2. **C2H5NH3Cl** (acidic, but less than NH4Br)
3. **NaCl** (neutral, pH = 7)
4. **NaCN** (basic, highest pH)

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### 4. Final Answer
Here is the correct order for the solutions from **lowest to highest pH**:
1. **NH4Br** (lowest pH, most acidic)
2. **C2H5NH3Cl**
3. **NaCl**
4. **NaCN** (highest pH, most basic)

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Would you like a deeper explanation of the hydrolysis reactions, or is there anything else you’d like clarified?

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**Related Questions:**
1. What is the equation for the hydrolysis of CN⁻ in water?
2. How can you calculate the exact pH of NH4Br?
3. Why does NaCl have no effect on the pH of the solution?
4. What is the relationship between Ka and Kb for conjugate acid-base pairs?
5. How do concentration and strength of acids/bases affect pH?

**Tip:** When ranking salts by pH, always consider whether the ions come from strong or weak acids/bases—this helps predict whether the solution will be acidic, basic, or neutral.

Rank the solutions (NaCN, NH4Br, NaCl, and C2H5NH3Cl) in increasing order of pH based on given Ka and Kb values for weak acids and bases.

Learn how to rank solutions (NaCN, NH4Br, NaCl, and C2H5NH3Cl) in order of increasing pH using given Ka and Kb values for weak acids and bases. This problem covers acid-base chemistry concepts, pH calculations, and the hydrolysis reactions of salts.

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