Please name the structure, thanks Vanillylmandelic acid (pK, 3.42) is a metabolite found in urine, the pH of which is normally in the range from 4.8 to 8.4. Provide thestructure of vanillylmandelic acid that you would expect to find in urine with pH 5.8?онOHНОVanillylmandelic acid

IUPAC naming of vanilylmandelic acid.

Answered: Please name the structure, thanks

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.135QE

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Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity, resonance, induction, hybridization, aromaticity, and atomic size, all play a role. In the following comparisons, you are asked to identify the factor(s) that would be most important to analyze when predicting relative acidity, and then to predict the trend in acidity and pKa values. For each of the following pairs of compounds answer the following two multiple-choice questions. 1. What factor(s) are the most important to consider when predicting the relative acidity of the two compounds? a. Electronegativity of the atom possessing the hydrogen. b. Resonance stabilization of the anionic conjugate base. c. Inductive stabilization of the anionic conjugate base. d. Hybridization of the atom possessing the hydrogen. e. The atomic size of the atom possessing the hydrogen.
Find the value of Kb for the conjugate base of the following organic acids. (a) picric acid used in the manufacture of explosives; Ka = 0.16 (b) trichloroacetic acid used in the treatment of warts; Ka = 0.20
Benzoic acid (C6H5COOH) and aniline (C6H5NH2) areboth derivatives of benzene. Benzoic acid is an acid withKa = 6.3 x10-5 and aniline is a base with Ka = 4.3 x10-10. (a) What are the conjugate base of benzoic acid andthe conjugate acid of aniline? (b) Anilinium chloride(C6H5NH3Cl) is a strong electrolyte that dissociates intoanilinium ions (C6H5NH3+) and chloride ions. Which willbe more acidic, a 0.10 M solution of benzoic acid or a 0.10M solution of anilinium chloride? (c) What is the value ofthe equilibrium constant for the following equilibrium?C6H5COOH(aq) + C6H5NH2(aq) ⇌ C6H5COO-(aq) + C6H5NH3+(aq)
The pKa value of CH3COOH/CH3COO- is 4.75. At what pH value are the concentration of CH3COO- and CH3COOH the same?
Assuming only the neutral form of the compound significantly "bioconcentrates" in fish, Estimate the equilibrium concentration (ug chemical/kg wet fish) of the acid pentachlorophenol (PCP) in a rainbow trout swimming in water (pH =7) having a total concentration of 10 ug/L PCP (both neutral and negatively charged forms. The log Kow for the neutral form of pentachlorophenol is 5.0 and the pKa is 5.
The structure of benzene-1,2,3-tricarboxylic acid (pKa1 =2.88, pKa2 4.76, pKa3 = 7.13) can be seen on the right. What is the predominate form of benzene-1,2,3-tricarboxylic acid in a solution that has a pH of 6.0?
Please answer all as soon as possibleeee
Quinine (C20 H24 N2O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pKb, = 5.1 and pK, = 9.7 (pK, = - log Kp). Only 1 g quinine will dissolve in 1930.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction Q+ H20 = QH+ + OH° described by pK,, where Q = quinine. pH =
Please don't provide handwritten solution
The following aqueous species constitute two conjugate acid-base pairs. Use them to write one acid-base reaction with Kc > 1 and another with Kc < 1: HS-, Cl-, HCl, H2S.
pKa values are different in different solvents. For example, the pKa of hydrofluoric acid (HF) in water is 3.45, but the pKa of hydrofluoric acid in DMSO (dimethyl sulfoxide) is 15.0. Choose the best explanation for the difference
An analytical chemist is titrating 211.2 mL of a 0.5700M solution of aniline (C6H5NH₂) with a 0.7200M solution of HNO3. The pK, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 140.1 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 P X S

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