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Organic Chemistry (6th Edition)
- For each of the following reactions predict whether the equilibrium lies predominantly to the left or to the right. Explain your prediction briefly. (a) HCO3(aq) + SO42(aq) CO32(aq) + HSO4(aq) (b) HSO4(aq) + CH3CO2(aq) SO42(aq) + CH3CO2H(aq) (c) [Co(H2O)6]2+(aq) + CH3CO2(aq) [Co(H2O)5(OH)]+(aq) + CH3CO2H(aq)arrow_forwardFor each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) H2S(aq) + CO32(aq) HS(aq) + HCO3(aq) (b) HCN(aq) + SO42(aq) CN(aq) + HSO4(aq) (c) SO42(aq) + CH3CO2H(aq) HSO4(aq) + CH3CO2(aq)arrow_forwardBased on this acid-base reaction as written below, which of the following is correct about the roles of the species in the reaction? + NH2 H-C=C-H H-C=C? :NH3 K L M N O a. Mis the stronger acid than K O b. Nis the weaker base than L O c. Lis the weaker base than M O d. Kis the stronger acid than Narrow_forward
- 1. For each acid-base reaction, label the acid, the base, the conjugate acid, and the conjugate base, and determine whether the equilibrium lies toward reactants (to the left) or toward products (to the right) ' a) b) d) H₂O OH + IZ Br Хон NH₂ H₂O OH HBr Xo NH3arrow_forward2 What is the pH of a solution of 0.1M Acetic Acid with 0.01 M HCl added. The Ka for acetic acid is 1.8 x 10-5? What is the pH of a solution of 0.1M acetic acid with 0.01 M sodium acetate added. The Ka for acetic acid is 1.8 x 10-5arrow_forwardAbout this time, you may be wishing you had an aspirin. Aspirin is an organic acid with a Ka of 3.27 104 for the reaction. HC9H7O4(aq) + H2O() C9H7O4(aq) + H3O+(aq) If you have two tablets, each contains 0.325 g of aspirin (mixed with a neutral binder to hold the tablet together), and you dissolve then in a glass of water to give 225 mL of solution, what is the pH of the solution.arrow_forward
- For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid? (a) Acetic add, Ka = 1.74 105 (b) Chloroacetic acid, Ka= 1.38 103arrow_forwardWhat are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. HC1O4+ H2O — NH/ + H2O -» HCOr + OH" —arrow_forward8-15 Write an equation for the reaction that takes place when each base is added to water. (a) LiOH (b) (CH3)2NH (c) Sr(OH)2 (d) CH3CH2NH2arrow_forward
- Which of the following will increase the percent of NH3 that is converted to the ammonium ion in water (Hint: Use LeChatelier’s principle.)? (a) addition of NaOH. (b) addition of HCl. (c) addition of NH4Clarrow_forwardBarbituric acid, HC4H3N2O3, is used to prepare barbiturates, a class of drugs used as sedatives. Its Ka is 9.8105. Calculate [H+] in solutions prepared by adding enough water to the following to make 1.45 L. (a) 0.344 mol (b) 28.9 garrow_forwardCalculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+, in a 0.10-M aqueous solution of pyridine (Kb = 1.7 109).arrow_forward
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