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Chapter 10: Q10DE (page 229)

Calculate the pH of a $0.010 M$ solution of each amino acid in the form drawn here

Short Answer

Expert verified

The isoionic Ph is $= 10.37$

Step by step solution

01

Step 1: Define the term isoionic ph.

When a pure, neutral polyprotic acid is dissolved in water, the isoionic point or isoionic pH is obtained.

The isoelectric point is the pH at which the polyprotic acid's average charge is zero (0).

02

Calculate the isoionic PH

The pH of a neutral, polyprotic molecule in pure solution.

The only ions present are $H^{+}, {OH}^{-}$

Isoionic is the name given to polyprotic species.

$[H +] = \sqrt{\frac{K_{2} K_{3} F + K_{2} K_{w}}{K_{2} + F}}$

Where F is the formal concentration.

Here Arginine has four forms $H_{3} A^{2 +}, H_{2} A^{+}, HA$ and $A^{-}$

HA form shown as

$[H +] = \sqrt{\frac{K_{2} K_{3} (0.010) + K_{2} K_{w}}{K_{2} + 0.010}}$

$= 4.28 脳 10^{- 11} MpH = 10.37$

Thus the isoionic Ph is $= 10.37$

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Most popular questions from this chapter

(a) Which two of the following compounds would you mix to make a buffer of $^{pH}$ 7.45: $^{H_{3} {PO}_{4}}$ (FM 98.00), $^{{NaH}_{2} {PO}_{4}}$ (FM 119.98), $^{{Na}_{2} {HPO}_{4}}$ (FM 141.96), and $^{{Na}_{3} {PO}_{4}}$ (FM 163.94)?

(b) If you wanted to prepare $^{1.00 L}$ of buffer with a total phosphate concentration of $^{0.0500 M}$ , how many grams of each of the two selected compounds would you mix together?

(c) If you did what you calculated in part (b), you would not get a pH of exactly 7.45. Explain how you would really prepare this buffer in the lab.

Fractional composition in a triprotic system. For a triprotic system, the fractional composition equations where are $D = {[H^{+}]}^{3} + K_{1} {[H^{+}]}^{2} + K_{1} K_{2} [H^{+}] + K_{1} K_{2} K_{3}$ Use these equations to create a fractional composition diagram analogous to Figure 10-4 for the amino acid tyrosine. What is the fraction of each species at $pH 10.00$ ?

$伪_{H_{3} A} = \frac{{[H^{+}]}^{3}}{D} 伪_{H^{2}} = \frac{K_{1} K_{2} [H^{+}]}{D} 伪_{H_{2} A} = \frac{K_{1} {[H^{+}]}^{2}}{D} 伪_{A^{3}} = \frac{K_{1} K_{2} K_{3}}{D}$

How many millilitres of 1.00 M KOH should be added to 100 mL of solution containing 10.0 g of histidine hydrochloride

[His? HCI (HisH1) (CI2), FM 191.62 ] to get a pH of 9.30 ?

Draw the structures of the predominant forms of glutamic acid and tyrosine at $pH 9.0$ and $pH 10.0$ What is the second most abundant species at each ?.

The diprotic acid $H_{2} A$ has ${pK}_{1} = 4.00$ and ${pK}_{2} = 8.00$ .

(a) At what pH is $[H_{2} A]$ = $[H A^{-}]$ ?

(b) At what pH is $[H A^{-}]$ = $[A^{2 -}]$ ?

(c) Which is the principal species at pH 2.00: $H_{2} A, {HA}^{-}$ or $A^{2 -}$ ?

(d) Which is the principal species at pH 6.00?

(e) Which is the principal species at pH 10.00?

See all solutions

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