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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Explain how isoelectric focusing works.

CO2(g)𝆏CO2(aq)KH=[CO2aq]PCO2=10-1.2073molkg-1bar-1at0C=10-1.6048molkg-1bar-1at30CCO2(aq)+H2O𝆏HCO3-+H+Ka1=[HCO3-][H+][CO2aq]=10-6.1004molkg-1at0C=10-5.8008molkg-1bar-1at30CHCO3-𝆏CO32-+H+CaCO3(S,aragonite)𝆏Ca2++CO3-2Ksparg=[Ca2+][CO32-]=10-6.1113mol2kg-2bar-2at0C=10-6.1391mol2kg-2bar-2at30CCaCO3(s,calcite)𝆏Ca2++CO3-2kspcal=[Ca2+][CO32-]=10-6.3652mol2kg-2bar-2at0C=10-6.3713mol2kg-2bar-2at30CEffect of temperature on carbonic acid acidity and the solubility of localid="1654949830957" CaCO3×14Box10-1states that marine life withlocalid="1654949841354" CaCO3shells and skeletons will be threatened with extinction in cold polar waters

before that will happen in warm tropical waters. The following equilibrium constants apply to seawater at0ndlocalid="1654949866125" 30C, when concentrations are measured in moles per kilogram of seawater and pressure is in bars:

localid="1654951136007" CO2g𝆏CO2aqKH=CO2aqPCO2=10-1.2073molkg-1bar-1at0C=10-1.6048molkg-1bar-1at30CCO2aq+H2O𝆏HCO3-+H+Ka1=HCO3-H+CO2aq=10-6.1004molkg-1at0C=10-5.8008molkg-1bar-1at30CHCO3-𝆏CO32-+H+CaCO3S,aragonite𝆏Ca2++CO3-2Ksparg=Ca2+CO32-=10-6.1113mol2kg-2bar-2at0C=10-6.1391mol2kg-2bar-2at30CCaCO3s,calcite𝆏Ca2++CO3-2kspcal=Ca2+CO32-=10-6.3652mol2kg-2bar-2at0C=10-6.3713mol2kg-2bar-2at30C

The first equilibrium constant is calledlocalid="1654949908801" KHfor Henry's law (Problem 10-10). Units are given to remind you what units you must use.

(a) Combine the expressions forlocalid="1654949922835" KH,K21, andlocalid="1654949935065" K22to find an expression forlocalid="1654949944862" [CO3-2]in terms oflocalid="1654949958224" PCO2andlocalid="1654949971486" [H+].

(b) From the result of (a), calculatelocalid="1654949980228" [CO32-](molkg-1)atlocalid="1654950000228" pCO2=800μbar and pH=7.8 at temperatures oflocalid="1654950013597" 0(polar ocean) andlocalid="1654950030147" 30C(tropical ocean). These are conditions that could possibly be reached around the year 2100 .

(c) The concentration oflocalid="1654950042348" Ca2+in the ocean islocalid="1654950053646" 0.010M. Predict whether aragonite and calcite will dissolve under the conditions in (b).

Calculate the pH of a0.010Msolution of each amino acid in the form drawn here


A solution containing acetic acid, oxalic acid, ammonia, and pyridine has a pHof 9.00. What fraction of ammonia is not protonated?

Heterogeneous equilibrium.CO2dissolves in water to give "carbonic acid" (which is mostly dissolvedCO2, as described in Box 6-4).

CO2(g)𝆏CO2(aq)K=10-1.5

(The equilibrium constant is called the Henry's law constant for carbon dioxide, because Henry's law states that the solubility of a gas in a liquid is proportional to the pressure of the gas.) The acid dissociation constants listed for "carbonic acid" in Appendix G apply toCO2(aq). Given thatPCO2in the atmosphere is 10-3.4atm, find the pHof water in equilibrium with the atmosphere.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free