A) ammonia acting as a base toward the acid water B) ammonia acting as an acid t

Question

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 k(eq) and therefore is more important in an aqueous solution of ammonia? Relative Strengths of some Acids and Bases Relative Strengths of Some Acids and Bases Conjugate acid NH, (ammonia) ROH (alcohol HOH (water) RSH (thiol) R,NH (trialkylammonium ion) NH4 (ammonium ion) HCN (hydrocyanic acid) H (hydrosulfuric acid) TABLE 3.1 Conjugate base NH2 (amide) RO (alkoxide) HO (hydroxide R$ (thiolate) R,N: (trialkylamine) H,N: (ammonia) CN (cyanide) Hs (hydrosulfide) pk, -35 15-19 15.7 10-12* 9-11 9.25 9.40 7.0 R-C-OH (carboxylic acid) HF: (hydrofluoric acid) 0 R-- (carboxylate) F:(fluoride) 4-5 3.2 (p-toluene- soi sulfonate, or "tosylate") (p-toluene- so,H sulfonic acid) SO,H Hö (hydronium ion) ,so, (sulfuric acid) HCl: (hydrochloric acid) HBr: (hydrobromic acid) HI: (hydroiodic acid) HCIO, (perchloric acid Precise value varies with the structure of R 1.7 3t -6 to-7 -8 to-9.5 9.5 to-10 H,0 (water) HSO2 (bisulfate Ci:- (chloride (bromide) :-(lodide CIO; (perchlorate) -10( Estimates; exact measurement is not possible.

Explanation / Answer

A) ammonia acting as a base toward the acid water

NH3 + H2O <--> NH4+ + OH-

Kb = 1.8*10^-5

B) ammonia acting as an acid toward the base water.

NH3 + H2O <--> NH2- + H3O+

ka = kw/Kb = (10^-14)/(1.8*10^-5= 5.555*10^-10

Which of these reactions has the larger k(eq) and therefore is more important in an aqueous solution of ammonia?

K eq = Kb

since KA is too low, wont probably happen

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.