Glycine `[NH_(2)CH_(2)COOH)` is basic and acidic due to presence of `-NH_(2)` and `-COOH` group. It acquires a `H^(o+)` to form `overset(o+)NH_(3)COOH`, which is a diprotic acid with `K_(1) = 4.5 5 xx10^(-3)` and `K_(2) = 1.7 xx 10^(-10)`. In a `0.01M` solution of neutral glycine,
a. What is the `pH` and
b. What percent of the glycine is in the cationic form at equilibrium?

Explanation

To solve the problem regarding glycine, we will follow these steps:

### Step 1: Understand the Ionization of Glycine
Glycine (NH₂CH₂COOH) can exist in three forms:
1. Cationic form (H₃N⁺CH₂COOH) - when it accepts a proton.
2. Neutral form (H₂NCH₂COOH) - when it is neither gaining nor losing protons.
3. Anionic form (H₂NCH₂COO⁻) - when it donates a proton.

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