The dissociation of lactic acid to lactate is shown in the reaction. Lactic acid has a pk, of 3.86. + H* HO. OH OH Lactic acid Lactate A solution containing a mixture of lactic acid and lactate was found to have a pH of 3.32. Calculate the ratio of the lactate concentration to the lactic acid concentration in this solution. [lactate] 0.301 [lactic acid] What fraction of the lactic acid/lactate mixture is lactic acid? fraction lactic acid =

The dissociation of lactic acid to lactate is shown in the reaction. Lactic acid has a pk, of 3.86. + H* HO. OH OH Lactic acid Lactate A solution containing a mixture of lactic acid and lactate was found to have a pH of 3.32. Calculate the ratio of the lactate concentration to the lactic acid concentration in this solution. [lactate] 0.301 [lactic acid] What fraction of the lactic acid/lactate mixture is lactic acid? fraction lactic acid =

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section: Chapter Questions

Problem 4.18P: If the G for a reaction is 4.5 kcal/mol at 298 K, what is the Keq for this reaction? What is the...

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If the G for a reaction is 4.5 kcal/mol at 298 K, what is the Keq for this reaction? What is the change in entropy of this reaction if H = 3.2 kcal/mol?
3. The pH of the given solution of lactic acid and lactate is 4.30. Calculate the pKa of lactic acid, when the concentration of lactic acid and lactate are 0.020 M and 0.073 M respectively.
You are going to be using Isoleucine in a buffer. The pKa of the carboxylate group of Isoleucine is 2.36 If you have a 0.1 M solution of Isoleucine at pH 3.22, what fraction (or percent) of the solution is in the deprotonated (COO- ) form?
Alcohols are weak organic acids, pKa 15–18. The pKa of ethanol, CH3CH2OH, is 15.9. Write equations for the equilibrium reactions of ethanol with each base. Which equilibria lie considerably toward the right? Which lie considerably toward the left? Q.) NaOH
Oxacarbazepine ( C15H12N2O) is used to treat epilepsy. What would happen to the equilibrium of oxacarbazepine in water when more oxacarbazepine is added to the system? a.) Ratef < Rateb and the equilibrium would shift to reactants (to the left) b.) Ratef > Rateb and the equilibrium would shift to reactants (to the left) c.) Ratef < Rateb and the equilibrium would shift to products (to the right) d.) Ratef > Rateb and the equilibrium would shift to products (to the right)
The value of K, for ethylamine, C,H;NH, is 4.30×104. Write the equation for the reaction that goes with this equilibrium constant. + It is not necessary to include states such as (ag) or (1). +
Carbonic acid is a weak di-protic acid, which constitutes an important buffer system in the blood. There, it can dissociate two different protons at two different pka’s. These pka values are 6.4 and 10.2 a) Research the chemistry of this system in your textbook and provide the balanced equilibrium reactions. Start with the formation of carbonic acid from carbondioxide and water and show the reactions where protons dissociate. For each step provide both the chemical formulas and the names of the chemical components. Indicate the above pka values for the appropriate equilibrium reactions b) Provide both the chemical formulas and the names of all molecules shown in a) that can act as i) weak acid and ii) conjugate base at the respective pka values
Ethylenediamine has pK, values of 4.072 (pKb) and 7.152 (pKb2). What is the predominant form of ethylenediamine at pH 6.077? O) HẸNCH,CH,NH H₂NCH₂CH₂NH₂ H₂NCH₂CH₂NH What is the predominant form of ethylenediamine at pH 9.332? O H₂NCH₂CH₂NH₂ O H₂NCH₂CH₂NH O H₂NCH₂CH₂NH3 What is the second most abundant species of ethylenediamine at pH 6.077? O H₂NCH₂CH₂NH₂ O HẸNCH,CH,NH O H₂NCH₂CH₂NH What is the second most abundant species of ethylenediamine at pH 9.332? O H₂NCH₂CH₂NH₂ ( HẸNCH,CH,NH H₂NCH₂CH₂NH Calculate the percentage of ethylenediamine in the predominant form at each pH. pH 6.077: pH 9.332: % %
Ammonia (NH3) is a weak base that under acidic conditions becomes protonated to the ammonium ion in thefollowing reaction:NH3 + H+ → NH4 +NH3 freely permeates biological membranes, including thoseof lysosomes. The lysosome is a subcellular organelle witha pH of about 4.5–5.0; the pH of cytoplasm is about 7.0.What is the effect on the pH of the fluid content of lysosomes when cells are exposed to ammonia? Note: Ammonium (NH4 +) does not diffuse freely across membranes.
The following reactions all have K > 1.1) HF (aq) + C6H5O- (aq) F- (aq) + C6H5OH (aq)2) CH3COOH (aq) + C6H5O- (aq) C6H5OH (aq) + CH3COO- (aq)3) HF (aq) + CH3COO- (aq) F- (aq) + CH3COOH (aq)Arrange the substances based on their relative acid strength. Strongest acid, intermediate acid, weak acid, not a Bronsted-Lowry acid. CH3COOH HF C6H5OH CH3COO- F- C6H5O-
The pKb for the propanoate ion, CH3CH2CO3 , is 9.126. What is the value of Ka (NOT the pKa) for propanoic acid, CH3CH2CO3H?
For an acid with a pKa of 5.00, what is the pKb of its conjugate base?