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10-37. Which four amino acids in Table 10-1have acidic substituents (that donate a proton) and which three have basic substituents (that accept a proton)?

Short Answer

Expert verified

Acidic substituents that donate a proton and Basic substituents that accept a proton are given.

Step by step solution

01

Derivation of acidic and basic substituents.

  • Proteins are made up of amino acids that have an acidic carboxylic acid group, a basic amino group, and a variable substituent called R.

  • Because the carboxyl group is more acidic than the ammonium group, the nonionized form spontaneously rearranges to the zwitterion, which has both positive and negative sites

02

Determining the acidic and basic substituents.

In this problem we will determine which four amino acids from Table 10-1 have acidic substituents and which three have basic substituents.

Acidic substituents

Acidic substituents that donate a proton are given below:

  • aspartic acid

  • cysteine

  • glutamic acia

  • tyrosine

Basic Substituents

Basic substituents that accept a proton are given below:

  • arginine

  • histidine

  • tysine

Therefore the acidic and basic substituents are found.

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Most popular questions from this chapter

Draw the structures of the predominant forms of glutamic acid and tyrosine at pH9.0and pH10.0What is the second most abundant species at each ?.

Write the general structure of an amino acid. Why do some amino acids in Table10-1have two pK values and others three?

(a) Which two of the following compounds would you mix to make a buffer of pH7.45: H3PO4(FM 98.00), NaH2PO4(FM 119.98), Na2HPO4(FM 141.96), and Na3PO4(FM 163.94)?

(b) If you wanted to prepare 1.00Lof buffer with a total phosphate concentration of 0.0500M, 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.

In this problem, we calculate the pH of the intermediate form of a diprotic acid, taking activities into account.

(a) Including activity coefficients, derive Equation 10 - 11 for potassium hydrogen phthalate (K+HP- in the example following Equation 10 - 12 ).

(b) Calculate the pH of 0.050MKHP , using the results in part (a). Assume that the sizes of both HP- and P2- are 600pm . For comparison, Equation 10 - 11 gives pH=4.18.

  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?

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