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Chapter 10: Q38P (page 232)

What is the difference between the isoelectric pH and the isoionic of a protein with many different acidic and basic substituents?

Short Answer

Expert verified
  • Isoelectric pH: protein carries no net electrical charge, but still contains positive and negative sites.
  • Isoionic pH: almost the same as isoelectric point, but in this case, the pH of a solution contains only protein, H+ andOH-

Step by step solution

01

Derivation of isoelectric pH and isoionicpH.

  • The pH forwhich a molecule essentially has almost no net electrical charge or is electrically neutral is characterizedas the isoelectric point (pI, pH (I), IEP).
  • The standard abbreviation for the isoelectric point is pH (I), though pI is also used and is used in this article for brevity.
  • 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

Determining the difference between isoelectric pH and isoionicpH.

  • In this task we will determine the difference between the isoionicand the isoelectric of a protein with different acidic and basic substituents.
  • Isoelectric pH: protein carries no net electrical charge, but still contains positive and negative sites.
  • The protein net charge is affected by the of the environment and protein can become positively or negatively charged due to the loss or gain of protons H+
  • Isoionic pH: almost the same as isoelectric point, but in this case the of a solution contains only protein, H+and OH- (no other ions are considered in isoionic pH ).

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Most popular questions from this chapter

  1. 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" Cr3++H2O⇋CrOH2++H+Ka1=10-3.80CrOH2++H2O⇋CrOH2++H+Ka2=10-6.40CrOH2++H2O⇋CrOH3aq+H+Ka3=10-6.40CrOH3aq+H2O⇋CrOH4-+H+Ka4=-11.40

(Yes, the values oflocalid="1654853051658" Ka2andlocalid="1654853058271" Ka3are 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" CrOH3SCrOH3aqKa3=10-6.80

What concentration of localid="1654853075036" CrOH3aqis in equilibrium with solid localid="1654853085944" CrOH3aqS?

(c) What concentration oflocalid="1654853094735" CrOH2+is in equilibrium with localid="1654853101499" CrOH3aqSif the solution localid="1654853109266" pHis adjusted tolocalid="1654853117749" 4.00?

Calculate αH2A,αHA-,αA2- for cis-butenedioic acid at pH 1.00, 1.92, 6.00, 6.27 and 10.00.

The acid HA has pKa= 4.00. Find the fraction in the form HA and the fraction in the form A- at pH = 5.00. Does your answer agree with what you

expect for the quotient [A2]/[HA] at pH 5.00?

How many grams of Na2CO3(FM 105.99) should be mixed with 5.00gof NaHCO3(FM 84.01) to produce 100mLof buffer with pH10.00?

The acid HA has pKa=7.00.

(a) Which is the principal species, HA or A-, at pH 6.00?

(b) Which is the principal species at pH 8.00?

(c) What is the quotient [A-]/[HA] at pH 7.00? At pH 6.00?
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