OH + HCO3 Reactant Side Product Side (a) draw the conjugate acid and the conjugate base products of this reaction and include all lone pairs of electrons and all formal charges (if any) (b) using the Evans pka table and the internet: I. determine in which direction this reaction will proceed and explain your reasoning II. indicate the pKa value of the acid on the reactant side and of the acid on the product side of the reaction (c) using curved arrows indicate the direction of electron flow between the two reactants on the reactant side

OH + HCO3 Reactant Side Product Side (a) draw the conjugate acid and the conjugate base products of this reaction and include all lone pairs of electrons and all formal charges (if any) (b) using the Evans pka table and the internet: I. determine in which direction this reaction will proceed and explain your reasoning II. indicate the pKa value of the acid on the reactant side and of the acid on the product side of the reaction (c) using curved arrows indicate the direction of electron flow between the two reactants on the reactant side

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section: Chapter Questions

Problem 4.10P: Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow...

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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+
For each equation, label the Lewis acid and the Lewis base. In addition, show all unshared pairs of electrons on the reacting atoms and use curved arrows to show the flow of electrons in each reaction. (a) F + BF3 BF4
Complete the equation for the reaction between each Lewis acid-base pair. In each equation, label which starting material is the Lewis acid and which is the Lewis base; use curved arrows to show the flow of electrons in each reaction. In doing this problem, it is essential that you show valence electrons for all atoms participating in each reaction. (a) (b) (c) (d)
[References] Answer questions a-c about the Bronsted acid-base reaction below using the identifying letters A-D below each structure. The pka's for the acids of interest are: phenol (pka = 9.9), and carbonic acid (pKa = 6.4). OH A phenol B bicarbonate C phenoxide OH D carbonic acid a) The stronger acid is b) Its conjugate base is c) The species that predominate at equilibrium are (two letters, e.g. ac)
b Please help me answer all of this x O Dashboard ở Course: Chem 120 - Organic Che x O LOCAL clicker + A cpp.edu/~Isstarkey/local/clicker/bonding/acid-base.html Arrange the following hydrogens in the order of DECREASING pK, values (from least acidic to most acidic). Arrange the following compounds in order of INČREASING acid strength (from least acidic to most acidic). A)I> II > III -OH HCI CH;OH II III B) III> ||>1 0=C-C-CH2-CF3 OH I C) II > III >I A) III I> II II E) II>I> II C) I < III < II D) II < III < I E) I < II < III Which is the stronger base? Explain briefly. Draw the conjugate acid or conjugate base, as directed, for each. но CH3-C-o conjugate base of NH3 conjugate acid of HO conjugate acid of H:0 hydroxide acetate NH, H20 A) A) Because this is more stable: H-0-H hydroxide is the stronger base. NH. он о B) H20 B) Because this is more stable: H-o hydroxide is the weaker base. NH, OH H2 C) C) Because this is more stable: CH-8-OH acetate is the stronger base. NH, H2 D) D)…
I understand that Ka refers to the rate (constant) that HA acid dissociates into base A- and proton H+. I don't understand the pKa equation. What is the "p"? What does negative logarithm mean? Thank you.
Q8 (a) Based from the following reaction: H-ci: H. H. + (i) Determine the conjugate acid and conjugate base. (ii) Show the mechanism of the deprotonation reaction occurs using arrows.
2) For each of the following reactions below, predict the products and draw full Lewis structures for the products and reactants. Use curved arrows to show how the proton is transferred in each reaction. Use the table of pKa's given below to determine the position of the equilibrium (to the right or to the left). Acid a) C6H5OH + NaOCH3 pKa 0.18 CF3CO2H CH3CO2H 4.75 b) CH3CO2H + CF3CO2- НCN 9.31 c) HCEC?+ NH3 NH4* 9.25 C6H50H 10.0 CH3OH HCECH 15 25 NH3 39
2A. Rank the following compounds with increasing acidity: (1 = least acidic; 3 = most acidic) Me Me Mo Me (c) Se H. (d) H. .H H.
The following molecule (or ion) acts as a base: CH3 CH2 O Draw the structural formula of the conjugate acid formed in a reaction with HCI. • You do not have to explicitly draw H atoms. Do not include lone pairs in your answer. They will not be considered in the grading. • Do not include counter-ions, e.g., Na", I", in your answer. P opy aste CH4 ChemDoodle
Draw the organic product of the Lewis acid-base reaction shown below. Include all lone pairs and charges as appropriate. :0: NaBH4 (source of H-) H3C H :OH: CH3
Use the information in the pK table to rank the molecules in order of decreasing basicity. For example, select "1" in the second column for the strongest base a and "2" for the next strongest base and so on. CH3 HS F CH,CO, Molecules (Choose one) (Choose one) (Choose one) (Choose one) X Ś CHA 4 NH₂ H₂ CH3NH₂ 2 48 38 36 33 pk table pKa CH,NH, CH₂SH 10.4 H₂O* HCN + 10.6 9.4 NH H₂O 15.7 H₂S CH₂OH 15.5 CH,CO,H 4.76 9.2 7.00 HF CH₂OH₂ H₂SO4 HC1 HBr 3.17 -1.7 -2.2 -3.0 -7 -9