The acidity constants for citric acid are \(\mathrm{p} K_{a 1}=3.13, \mathrm{p} K_{a 2}=4.72,\) and \(\mathrm{p} K_{a 3}=6.33\)
a. Write expressions for \(\alpha_{0}, \alpha_{1}, \alpha_{2},\) and \(\alpha_{3}\) as a function of the \(K_{o}\) values and \(\left\{\mathrm{H}^{+}\right\}\)
b. Identify the region where each species is dominant.
c. Determine which terms in the denominators for the \(\alpha\) values are significant at pH 7.5 (terms contributing less than \(5 \%\) to the summation can be considered negligible). For a solution with \(10^{-1} M\) total citrate, write out an approximate equation of the form \(\log C_{i}=\) constant \(+n(\mathrm{pH})\) for each citrate species at \(\mathrm{pH}\) 7.5, approximating the dominant species' concentration as TOTCit.
d. Draw a \(\log C-\mathrm{pH}\) diagram for a solution with \(10^{-1} \mathrm{MTOTCit}\). Include the pH range \(1.0<\mathrm{pH}<8.0\).
e. Find the \(\mathrm{pH}\) of the following solutions:
i. \(10^{-1} \mathrm{M} \mathrm{H}_{3} \mathrm{Cit}+\) water.
ii. \(10^{-1} M \mathrm{Na}_{2} \mathrm{HCit}+\) water.
iii. \(0.05 \mathrm{M} \mathrm{Na}_{3} \mathrm{Cit}+0.05 \mathrm{M} \mathrm{NaH}_{2} \mathrm{Cit}+\) water.
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2. The acidity constants for citric acid are \(\mathrm{p} K_{a 1}=3.13, \mathrm{pK}_{a 2}=4.72,\) and \(\mathrm{p} K_{a 3}=6.33\)a. Write expressions for \(\alpha_{0}, \alpha_{1}, \alpha_{2},\) and \(\alpha_{3}\) as a function of the \(K_{a}\) values and \(\left\{\mathrm{H}^{+}\right\}\)b. Identify the region where each species is dominant.c. Determine which terms in the denominators for the \(\alpha\) values are significant at \(\mathrm{pH} 7.5\) (terms contributing less than \(5 \%\) to the summation can be considered negligible). For a solution with \(10^{-1} M\) total citrate, write out...
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