4.A student has prepared 0.05 M solution of CH3-C=CH and has added to it 0.05 M solution ofpotassium tert-butoxide (K" O-C(CH3)3).(i) Write the equation for the acid-base reaction that might occur.(ii) With curved arrows track the movements of electron pairs.(iii) Assign Base, Acid, Conjugate acid for the base, Conjugate base for the acid.(iv) Calculate the percentage of deprotonated methyl acetylene taking into account that pKa ofthe conjugate acid of potassium tert-butoxide equals 18 and pKa of methyl acetylene equals 24.

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Answered: 4. A student has prepared 0.05 M…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section14.6: Molecular Structure And Acid Strength

Problem 14.14CE

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Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO,H, pK = 5.0]. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right? %3D The pKa values in Table 2.1 span a large range (-7 to 50). The pK, scale is logarithmic. small difference in pK, translates into a large numerical difference, For example, the diffe between the pK, of NH3 (38) and CH2=CH, (44) is six pKa units. This means that NH, is one million times more acidic than CH,=CH,.
3. For the following acid - base reaction, (a) predict the products; (b) identify the Bronsted acid, Bronsted base, conjugate acid, and conjugate base; (c) use curved arrows to show the flow of electron pairs in the reaction. CH3 CH2C-OH + NaNHa
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
Ammonia can react as an acid or a base. a) What is the conjugate acid of ammonia? b) What is the conjugate base of ammonia? c) arist dit ons servbed as Complete the following acid-base reaction in which NH3(e) acts as both an acid and a base: OcH 6 HOONH3() + NH3() = OOH (d FOZH (s *АНИ (1 sqz ions to biosqu adtavið
A student has prepared a 0.05 M solution of C6H5-OH and has added to it a 0.05 M solution of di-iso-propylamine (HN(CH(CH3)2)2. Concentrations are given only to emphasize they are equal, you do not need the value itself. (i) Write the equation for the acid-base reaction that might occur. (ii) With curved arrows track the movements of electron pairs. (iii) Assign Base, Acid, Conjugate acid for the base, Conjugate base for the acid. (iv) Calculate the percentage of phenolate (C6H5O-) that forms in this acid-base reaction taking into account that pKa of the conjugate acid of di-iso-propylamine equals 11 and pKa of phenol (C6H5OH) equals 10.
For each conjugate acid-base pair, identify the first species as an acid or a base and the second species as its conjugate acid or base. In addition, draw Lewis structures for each species, showing all valence electrons and any formal charge. (a) CH3CH2O- CH3CH2OH
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)
Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2O
Consider the acid-base nature of the salt NH4[C6H5COO], when it is dissolved in water. (1) What are the acid-base properties of the cation, NH4+? (2) What are the acid-base properties of the anion, C6H5COO™? (3) Would an aqueous solution of NH4[C6H5COO] be acidic, basic or neutral? C ◊
Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO2H, pKa = 5.0]. (a) Which acid has the larger Ka? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?
For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36
3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.

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