Consider the structures below to answer the following questions.A. Indicate the most acidic hydrogens in each of the molecules.OHCH-HCH₂C-HH&CམིངྒཱའིB. Rank the molecules above in order of increasing acidity (least acidic to most acidic).a.III, II, Ib. II, III, IC.I, II, IIId. II, I, III

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Answered: Consider the structures below to answer…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 45E: Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4

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The following are equivalent ways of asking about the acidity of an H atom: • What is the most acidic H on the molecule? • Which H is associated with the published pKa value? • Which H on the molecule is easiest to remove? • Which H on the molecule takes the least energy to remove? • Which bond to an H is most polarized? • For which H atom is removal least uphill in energy? • Which bond to an H atom, when broken, results in the lowest PE conjugate base? We will often find the last of these questions is easiest to answer. To do this, find all the different Hatoms on the molecule, and draw all possible conjugate bases.Only the lowest-energy one is the “real” conjugate base. Identify this structure, and you have found the most acidic H. Use this strategy to find the most acidic H on each of the following molecules. Note: Each structure hasat least three different kinds of H’s, so draw at least three unique conjugate bases for each.
Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize-excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid—base pairs.
Use Table 13-2 to order the following from the strongest to the weakest base. ClO2,H2O,NH3,ClO4
Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838. (a) Bath functional groups of salicylic acid ionize in water, with Ka=1.0103 for the—CO2H group and 4.201013 for the -OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L).. (b) Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H. The -CO2H functional group is still present, but its acidity is reduced, Ka=3.0104. What is the pH of a solution of aspirin with the same concentration as a saturated solution of salicylic acid (See Part a). (c) Under some conditions, aspirin reacts with water and forms a solution of salicylic acid and acetic acid: CH3CO2C6H4CO2H(aq)+H2O(l)HOC6H4CO2H(aq)+CH3CO2H(aq) i. Which of the acids, salicylic acid or acetic acid, produces more hydronium ions in such a solution? ii. What are the concentrations of molecules and ions in a solution produced by the hydrolysis of 0.50 g of aspirin dissolved in enough water to give 75 mL of solution?
Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+
I need help solving questions 5 and 6
s) For each of the following pairs of compounds indicate which is more acidic and why? Draw equations showing the dissociation into the anion and H*. он ČI A. HO, Br S-H C. D. H H H. H- -- E. B.
Indicate the order of acid strength of these compounds by ranking them, strongest to weakest. Select one: O a. IV, II, III, I O b. I, II, II, IV Oc. I, IV, II, III O d. IV, III, II, I e. III, IV, II, IX I O-H II H O-H CI III O-H IV O-H CI
Arrange the compounds in order of increasing acidity (least first). OH OH OCH3 OH I II III IV а. IV, II, I, II b. I, II, III, IV С. IV, II, III I d. II, I, II, IV
Arrange the following in terms of increasing stability in section IV, acidity in section V, and basicity in section VI using the less than (<) inequality.
Which of the following is the correct order of decreasing acid strength of the following compounds (more acidic > less acidic)? Explain. of + of "NH₂ H₂C- -NH₂ ΝΗ 3 a. 1>2>3 b. 2>3>1 c. 1>3>2 d. 3>2>1
Rank the indicated protons from least to most acidic: O MeO I. II. O I. < II. < III. III. < II.

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