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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 the pH 6.00 glycine act as a buffer solution, because at pH 6.00 the condition is acidic and we know glycine is amino acid, so it is gets equilibrium with zwitter ion, means there is positive charge on N of amino group and negative charge on carboxylate. So there is pH no changes suddenly and we know buffer solution resist the sudden change in pH, so the at the pH 6.00 glycine act as a buffer solution. Equation – enter image description here

what I need is that

HOW glycine acts 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.

Thanks.

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  • $\begingroup$ I rolled back your edit, as it just becomes a "homework-dump" (off topic) otherwise. $\endgroup$ – user15489 Jul 12 '15 at 1:34
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Your equation is not correct for pH 6; it should be for pH 1. For pH 6, the equation should be:
enter image description here

If an acid is added, then the equation becomes:
enter image description here

and if a base is added, then the equation is:
enter image description here

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