How can glycine act as a buffer at pH 6.00 and why? How can glycine act as a buffer at pH 6.00 and why? Please use
chemical equations to show how it can act as a buffer at this pH
specifically?

My work:
At pH 6.00 glycine acts as a buffer, because at pH 6.00 the condition is acidic and glycine is an amino acid, so its zwitterion forms an equilibrium, which means there is a positive charge on the N of the amino group and a negative charge on the carboxylate. So there are no sudden pH changes and we know buffer solutions resist sudden pH changes, so at pH 6.00 glycine acts as a buffer solution.
Equation:

What I need explained:
HOW does glycine act as a buffer at pH 6.00 with chemical equations, meaning to show an example of how it specifically buffers another species at pH 6.00 with the proper chemical equations.
Your equation is not correct for pH 6; it should be for pH 1. For pH 6, the equation should be:


If an acid is added, then the equation becomes:


and if a base is added, then the equation is: