. Do you (you) think that the amino acids in this experiment can be used as buffers for biochemical experiments? If so, please explain the pH range of its buffering effect.
Added by Lee T.
Step 1
To determine if the amino acids can act as buffers, we first need to know which specific amino acids are being studied, as different amino acids have different side chains and properties. Show more…
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Over what pH range(s) could valine be used as an effective buffer? Explain your answer, supporting it with what we have discussed about buffers and amino acids
Sri K.
Properties of a Buffer The amino acid glycine is often used as the main ingredient of a buffer in biochemical experiments. The amino group of glycine, which has a $\mathrm{p} K_{\mathrm{a}}$ of 9.6 can exist either in the protonated form $\left(-\mathbf{N H}_{3}^{+}\right)$ or as the free base $\left(-\mathrm{NH}_{2}\right),$ because of the reversible equilibrium $$\mathbf{R}-\mathbf{N H}_{3}^{+} \rightleftharpoons \mathbf{R}-\mathbf{N H}_{2}+\mathbf{H}^{+}$$ (a) In what $p$ H range can glycine be used as an effective buffer due to its amino group? (b) In a $0.1 \mathrm{M}$ solution of glycine at $\mathrm{pH} 9.0,$ what fraction of glycine has its amino group in the $-\mathbf{N H}_{3}^{+}$ form? (c) How much $5 \mathrm{M}$ KOH must be added to $1.0 \mathrm{L}$ of $0.1 \mathrm{M}$ glycine at $\mathrm{pH} 9.0$ to bring its pH to exactly $10.0 ?$ (d) When $99 \%$ of the glycine is in its $-\mathrm{NH}_{3}^{+}$ form, what is the numerical relation between the $\mathrm{pH}$ of the solution and the $\mathrm{p} K_{\mathrm{a}}$ of the amino group?
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