3. Draw the acid-base reaction products of sodium hydride and ethanol. Show using a curved arrow notation how the products are generated. Given the pKa values below, show using the equilibrium arrow where the reaction will proceed (forward or backward process). Justify your answer. (7 PTS) Na* :H + CH3CH₂-O-H Sodium hydride Ethanol Selected pK, Values Acid H-CI CH₂COO-H HO-H CHỊCH,O-H HCE CH H-H H₂N-H CH₂=CH₂ CH₂-H pk₂ -7 4.8 15.7 16 25 35 38 44 50 Conjugate base cr CH₂COO™ HO™ CH,CH,O HCEC H H₂N™ CH₂=CH CH₂

3. Draw the acid-base reaction products of sodium hydride and ethanol. Show using a curved arrow notation how the products are generated. Given the pKa values below, show using the equilibrium arrow where the reaction will proceed (forward or backward process). Justify your answer. (7 PTS) Na* :H + CH3CH₂-O-H Sodium hydride Ethanol Selected pK, Values Acid H-CI CH₂COO-H HO-H CHỊCH,O-H HCE CH H-H H₂N-H CH₂=CH₂ CH₂-H pk₂ -7 4.8 15.7 16 25 35 38 44 50 Conjugate base cr CH₂COO™ HO™ CH,CH,O HCEC H H₂N™ CH₂=CH CH₂

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter27: Amines

Section: Chapter Questions

Problem 7E

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Similar questions

Treatment of indene with NaNH2 forms its conjugate base in a Brønsted– Lowry acid–base reaction. Draw all reasonable resonance structures for indene's conjugate base, and explain why the pKa of indene is lower than the pKa of most hydrocarbons.
Treatment of indene with NaNH2 forms its conjugate base in a Brønsted–Lowry acid–base reaction. Draw all reasonable resonance structures for indene’s conjugate base, and explain why the pKa of indene is lower than the pKa of most hydrocarbons.
The Ka of acetic acid (CH3CO2H) is 1.8x10-5 and the Kb of methylamine (CH3NH2) is 4.4x10-4. Complete the following equilibrium reaction (acid-base reaction) equation and predict the side of the equilibrium that is favored. Explain. Show all your work.
Phthalic acid and isophthalic acid have protons on two carboxy groupsthat can be removed with base. (a) Explain why the pKa for loss of thefirst proton (pKa1) is lower for phthalic acid than isophthalic acid. (b)Explain why the pKa for loss of the second proton (pKa2) is higher forphthalic acid than isophthalic acid.
According to the Evan's pKa table, phenol has a pKa of 9.95. p-Nitro and m-nitrophenol have pKas of 7.14 and 8.35 respectively. Using resonance structures, explain the observed trends in the acidity of these molecules.
explain in great detail why the pKa values are what they are and compare them among the three compounds. The conjugate acids that are protonated are drawn in red for each compound. Which one based on the pKa is most acidic and what does that tell you about how basic their lone pairs are?
5) Ethyne (CH≡CH) has a pKa of 25 and water has pKa of 15.7 and ammonia (NH3) has a pKa of 36. Write equilibrium reactions showing arrows that indicate whether the reactants or products are the favored for reaction of Ethyne with a. HO- , and b. with NH2 - and indicate which one is better for removing proton from Ethyne. Then calculate the equilibrium constants, Ke, for each equilibrium reaction. Are calculated Ke values match the expected results from prediction you made .
Taking Ka for acidic acid as 1.8 x 10-5, calculate H3O+ , using the known concentraions of acidic acid and soudium acecate contained in reaction mixtures 1 and 4. Reaction mixture time (s) Acidic acid concentration (mol/L) sodium acetate concentration (mol/L) calculated H3O+ concentration 1 237 0 1 x 10 -5 4 236 1 x 10 -4 1 x 10 -5
Nitric acid (HNO3) is a strong acid that completely ionizes when dissolved in water (pKa = -1.30). Calculate the pH of 10 mg/L HNO3. a. Unlike nitric acid, butyric acid (CH3CH2CH2COOH) is a weak acid (pKa = 4.8). Calculate the pH of a solution when 90% of the CH3CH2CH2COOH is dissociated. b. Briefly explain how you can use the pKa values of these two molecules to determine that nitric acid is a strong acid, while butyric acid is a weak acid.
Histidine is an important catalytic residue found at the active sites of many enzymes. In many cases, histidine appears toremove protons or to transfer protons from one location to another.(a) Show which nitrogen atom of the histidine heterocycle is basic and which is not.(b) Use resonance forms to show why the protonated form of histidine is a particularly stable cation.(c) Show the structure that results when histidine accepts a proton on the basic nitrogen of the heterocycle and then isdeprotonated on the other heterocyclic nitrogen. Explain how histidine might function as a pipeline to transfer protonsbetween sites within an enzyme and its substrate
Phthalic acid and isophthalic acid have protons on two carboxy groups that can be removed with base. (a) Explain why the pKa for loss of the rst proton (pKa1) is lower for phthalic acid than isophthalic acid. (b) Explain why the pKa for loss of the second proton (pKa2) is higher for phthalic acid than isophthalic acid.
Label the most acidic hydrogen in each molecule and justify your choice by using appropriate pKa values