Concept explainers
Interpretation:
An explanation regarding the differences in the first and second
Concept introduction:
The acidity depends on the ease with which the acidic hydrogen is removed and the relative stability of the conjugate base that results after hydrogen is lost. The acidic nature is governed by the electronic nature of the substituent.
Inductive effect is defined as the polarization that results when a shared pair of electrons is attracted by the more electronegative atom bonded in a single bond. It is of two types:
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Organic Chemistry
- Chitosan is derived from the shells of crustaceans. it is only soluble in an aqueous acidic medium but not in organic solvents. When reacted with phthalic anhydride, it forms an amide. The product is no longer soluble in the aqueous medium but now is soluble in organic solvents. a) Draw the product of the reaction between chitosan and phthalic anhydride. b) Briefly explain the behaviour change in solubility of the starting material and the final product.arrow_forwardmention the conjugate bases and use structures to explain the following: a. why is the alpha proton of a ketone (pKa ~ 16) is more acidic than the protons in CH3CH3? b. why is the alpha proton of a ketone (pKa ~ 16) is more acidic than the protons in a ester (pKa ~ 35)? c. why are the hydrogens in a C-H bond like CH3CH3 difficult to remove?arrow_forwardWill acetylene react with sodium hydride according to the following equation to form a salt and hydrogen, H2? Using pKa values given in Table 4.1, calculate Keq for this equilibrium.arrow_forward
- Low-molecular-weight dicarboxylic acids normally exhibit two different pKa values. Ionization of the first carboxyl group is easier than the second. This effect diminishes with molecular size, and for adipic acid and longer chain dicarboxylic acids, the two acid ionization constants differ by about one pK unit. Why do the two pKa values differ more for the shorter chain dicarboxylic acids than for the longer chain dicarboxylic acids?arrow_forwardThe pKa, of the conjugate acid of morpholine is 8.33. (a) Calculate the ratio of morpholine to morpholinium ion in aqueous solution at pH 7.0. (b) At what pH are the concentrations of morpholine and morpholinium ion equal?arrow_forwardWhat is the acid anhydride of phosphoric acid (H3PO4)?arrow_forward
- Can any functional groups on Risperidone ionize? If so, which ones? Under what conditions? What are the pKa values of these functional groups? Write the structures in their correct ionization state at physiological pH.arrow_forwardin the esterification of acetylsalicylic acid phosphoric acid was used as a catalyst. Hydrochloric acid is about as strong a mineral acid as sulfuric acid. Why would HCl be not a satisfactory catalyst in this reaction?arrow_forwardWhat is the pKa of Sylvianic Acid if it is 2.3% dissociated at pH = 10.26?arrow_forward
- Consider the following compounds that vary from nearly nonacidic to strongly acidic. Draw the conjugate bases of these compounds, and explain why the acidity increases so dramatically with substitution by nitro groups.CH4 CH3NO2 CH2(NO2)2 CH(NO2)3 pKa ≅ 50 pKa = 10.2 pKa = 3.6 pKa = 0.17arrow_forwardDraw the structure of chloric and chlorous acid and predict their pKa values using Pauling's rules.arrow_forwardWhat reagent serves as the source of ammonia to deprotonate oxalic acid in the production of calcium oxalate monohydrate? a. ammonium oxalate b. hydrochloric acid c. urea d. ammonium hydroxidearrow_forward
- Organic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning