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Draw the structure of the product of the reaction between the compound shown below and H2SO4.
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- Which species is the stronger Lewis Acid? Why? (Use resonance structures to explain your answer.) BH3 or trimethoxyborateGive a complete curved arrow pushing mechanism for reactions A and B 1) Show ALL important resonance contributors for all intermediates. 2) Add non-bonding electrons and C−H bonds to the line-angle structures as required. 3) Indicate the Lewis acid/Lewis base (LA, LB) at each step as appropriate, and whether they are also Brønsted acids/bases (LA/BA, LB,BB) 4) GIVE THE NUMBER OF STEPS IN YOUR MECHANISMThe 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.
- S.2. List the following compounds by discussing their basicity.Please rank the following by increasing acidity: H2Se, H2O, CH4, H2Sexplain 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?
- One of the heptanedione isomers below has a pka of approximately 9 rather than 20. Which isomer? Why? Draw its conjugate base and offer a full explanation of its acidity.Rank the compounds shown in Image 27 in order of decreasing acidity.(i) Name the compounds participating in the following reactions as a Bronsted/Lewis acid and aBronsted/Lewis base and rewrite the reaction using the bond-line structure of reagents and products of the reaction. Supply the curved arrows explaining the mechanism of the reactions(arrows always originate at electron pair; if you have to use a couple of arrows pay attention that they have always to point the same direction). e. B(CH3)3 + H2O -> f. KH + (CH3)2CHCCH -> g. (CH3)3COH + NaH -> h. CH3CH(OH)COOH + HN(CH2CH3)2 -> i. H2SO4 + H3CCH2OH -> NOTE: PLEASE USE BOND-LINE STRUCTURE TO REPRESENT THE REACTANTS AND THE PRODUCTS
- NO2 being a deactivating group, increase the acidic nature of alcohol, by increasing the stability of the corresponding conjugate base. True FalseRank the following compounds in order of increasing acidity (1 = least acidic, 3 = most acidic) and in the space provided use resonance (of the conjugate base) to explain why the compound you have labelled “3” is the most acidic.Verify that the equilibrium position for the reaction between phenol and hydroxide ion is on the right by comparing the pKa value of the acid on the left with that of the acid on the right. Which acid is stronger? do the same for the reaction of phenol with hydrogen carbonate ion