In a `0.2M` aqueous solution of Ethylene diamine `(H_(2)NCH_(2)CH_(2)NH_(2)):`
Given `K_(b_(1))=8xx10^(-5)` & `K_(b_(2))=2.7xx10^(-8)` Find the pH of Solution .

Explanation

To find the pH of a 0.2 M aqueous solution of ethylene diamine (H₂NCH₂CH₂NH₂), we will follow these steps:

### Step 1: Identify the nature of ethylene diamine
Ethylene diamine is a diacidic base, meaning it can accept two protons (H⁺ ions) and has two base dissociation constants (K_b1 and K_b2).

### Step 2: Use the given values of K_b
We are given:
- K_b1 = 8 × 10^(-5)
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