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Chapter 10: Q2P (page 230)

Write the general structure of an amino acid. Why do some amino acids in Table $10 - 1$ have two pK values and others three?

Short Answer

Expert verified

The general structure of an amino acid:

The values of pK between amino acids differ from one another because these values apply to the residues - ${NH}_{3}^{+}, - {CO}_{2} H$ , and occasionally $- R$ .

Step by step solution

01

Definition of amino acid.

Amino acids are chemical molecules possessing amino and carboxylate $- C O - 2$ functional groups, as well as a particular side chain for each amino acid.

02

The pH of lysine.

The following is an amino acid's general structure ( denotes a carbon-carbon chain):

The values in Table $10 - 1$ , as well as their pK values, will be considered next. Each amino acid has a unique structure and amount of residues, resulting in a pH shift due to its amphoteric (acidic + basic) nature. Therefore, the values of pK between amino acids differ from one another because these values apply to the residues - ${NH}_{3}^{+}, - {CO}_{2} H$ , and occasionally $- R$ .

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Most popular questions from this chapter

Fractional composition in a tetraprotic system. Prepare a fractional composition diagram analogous to Figure 10-4 for the tetraprotic system derived from hydrolysis of $^{{Cr}^{+}}$ :

localid="1654853037629" $C r^{3 +} + H_{2} O 鈬� C r {(O H)}^{2 +} + H^{+} K_{a 1} = 10^{- 3.80} C r {(O H)}^{2 +} + H_{2} O 鈬� C r {(O H)}_{2}^{+} + H^{+} K_{a 2} = 10^{- 6.40} C r {(O H)}_{2}^{+} + H_{2} O 鈬� C r {(O H)}_{3} (a q) + H^{+} K_{a 3} = 10^{- 6.40} C r {(O H)}_{3} (a q) + H_{2} O 鈬� C r {(O H)}_{4}^{-} + H^{+} K_{a 4} =^{- 11.40}$

(Yes, the values oflocalid="1654853051658" $^{K_{a 2}}$ andlocalid="1654853058271" $^{K_{a 3}}$ are equal.)

(a) Use these equilibrium constants to prepare a fractional composition diagram for this tetraprotic system.

(b) You should do this part with your head and your calculator, not your spreadsheet. The solubility of is given by

localid="1654853063951" $C r {(O H)}_{3} (S) C r {(O H)}_{3} (a q) K_{a 3} = 10^{- 6.80}$

What concentration of localid="1654853075036" $^{Cr {(OH)}_{3} (aq)}$ is in equilibrium with solid localid="1654853085944" $^{C r {(O H)}_{3} (a q) (S)}$ ?

(c) What concentration oflocalid="1654853094735" $^{C r {(O H)}^{2 +}}$ is in equilibrium with localid="1654853101499" $^{C r {(O H)}_{3} (a q) (S)}$ if the solution localid="1654853109266" $^{p H}$ is adjusted tolocalid="1654853117749" $^{4.00}$ ?

Consider the diprotic acid $H_{2} A$ with $K_{1} = 1.00 脳 10^{- 4}$ and $K_{2} = 1.00 脳 10^{- 8}$ .Find the pH and concentrations of $H_{2} A, {HA}^{-}$ , and $A^{2 -}$ in

(a)role="math" localid="1654926233413" $0.100 {MH}_{2} A;$

(b) role="math" localid="1654926403235" $0.100 MNaHA$ ;

(c) $0.100 {MNa}_{2} A$ .

Use three cycles of approximation by the method of Box $10 - 2$ to calculate $[H^{+}], [H_{2} A], [{HA}^{-}],$ and $[A^{2}]$ inrole="math" localid="1654933890973" $0.00100 M$ monosodium oxalate, NaHA.

Find the pH with $1.50 {gNaN}_{2} P$ instead of 1.20 g.

(a) Using activity coefficients, calculate the pH of a solution containing a 2.00:1.00 mole ratio of ${HC}^{2} : C^{3 -}$ ( $H_{3} C$ = citric acid). The ionic strength is 0.010 M.

(b) What will be the pH if the ionic strength is raised to 0.10 M and the mole ratio ${HC}^{- 2} : C^{3 -}$ is kept constant?

See all solutions

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