Using the pK a values in Table 3.1, calculate the equilibrium constant for each of the following
Question:
Using the pKa values in Table 3.1, calculate the equilibrium constant for each of the following reactions.
(a) NH3 acting as a base toward the acid HCN
(b) F– acting as a base toward the acid HCN
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GREATER ACIDITY TABLE 3.1 Relative Strengths of Some Acids and Bases Conjugate acid pk NH, (ammonia) RÖH (alcohol) HÖH (water) HPO (hydrogen phosphate) RSH (thiol) R₂NH (trialkylammonium ion) NH, (ammonium ion) HCN (hydrocyanic acid) H₂PO, (dihydrogen phosphate) HSH (hydrosulfuric acid) R-C-OH (carboxylic acid) HF: (hydrofluoric acid) H₂PO4 (phosphoric acid) HNO, (nitric acid) H₂O* (hydronium ion) H₂C- -SO₂H (p-toluene- sulfonic acid) ~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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