Write an equation for each of the following equilibria, and use Table 3.1 to identify the pK
Question:
Write an equation for each of the following equilibria, and use Table 3.1 to identify the pKa value associated with the acidic species in each equilibrium.
(a) Ammonia acting as a base toward the acid water
(b) Ammonia acting as an acid toward the base water Which of these reactions has the larger Keq and therefore is more important in an aqueous solution of ammonia?
Transcribed Image Text:
GREATER ACIDITY TABLE 3.1 Relative Strengths of Some Acids and Bases Conjugate acid NH, (ammonia) RÖH (alcohol) HÖH (water) HPO (hydrogen phosphate) RSH (thiol) R,NH (trialkylammonium ion) NH, (ammonium ion) HCN (hydrocyanic acid) H₂PO, (dihydrogen phosphate) HSH (hydrosulfuric acid) R-C-OH (carboxylic acid) HE: (hydrofluoric acid) H₂PO (phosphoric acid) HNO, (nitric acid) H₂O* (hydronium ion) H₂C- -SO₂H (p-toluene- sulfonic acid) pK₂ ~35t 15-19 15.7 12.3 10-12* 9-11* 9.25 9.40 7.21 7.0 4-5* 3.2 2.2 -1.3 -1.7 -2.8+ Conjugate base -NH₂ (amide) RÖ:- (alkoxide) HÖ:- (hydroxide) PO (phosphate) RS (thiolate) R₂N: (trialkylamine) H₂N: (ammonia) -:CN (cyanide) HPO (hydrogen phosphate) HS:- (hydrosulfide) R-C-Ö: (carboxylate) F:-(fluoride) H₂PO (dihydrogen phosphate) NO; (nitrate) H₂O (water) H₂C- (p-toluene- -SO sulfonate, or "tosylate") GREATER BASI CITY
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