Question

D) An electron pair acceptor. E) An anphoteric species Q/33) A Lewis acid is? A)A proton donor B)A proton acceptor. C) An electron pair donor D) An electron pair acceptor E) An anphoteric species. Q(34) A Brønsted-Lowry acid is? A) A proton donor D) An electron pair acceptor. B)A proton acceptor. C) An electron pair donor E) An anphoteric species. Q(35) What is the relationship between Ka and Ko for a conjugate acid base pair? A) Kw=Ka+Kb B) Kw=Ka*Kb C) Kw=Ka-Ko. D) Kw=KaJKb. E) K-K2 Q(36) What is the pH of a 0.02 M solution of HBr (a strong acid)? B) pH=1.2 A) PH=1 C) pH=1.7 D) pH=2.3 E) pH-12.3 Q(37) What is the pH of a 0.04 M solution of KOH (a strong base)? A) pH-1.4 D) pH=9.3 B) pH-6.2 C) pH=7.7 E) pH=12.6 Q(38) What is the pH of a 0.0200 M aqueous solution of HF (Ka of HF is 6.8 * 10-4)? A) pH=1.4 D) pH-9.3 B) pH-2.4 C) pH-4.7 E) pH-12.6 Q(39) What is the pH of a 0.1 M aqueous solution of NH3 (Ko of HF is 1.8 * 10-)? A) pH=1.4 B) pH-2.4 C) pH-6.7 D) pH=11.3 E) pH-12.6 9140) Aqueous metal ions behave as Lewis acids because they A) can readily accept electrons in their vacant d orbitals. B) can readily donate electron pairs from their outermost porbitals. C) attract electrons from the water molecules they are dissolved in. D)are attracted to the electronegative oxygen atoms in the solvent. E) they are also a little amphoter

Answer 1

33. D ( Lewis acid is electron pair acceptor and lewis base is electron paorn donar )

34 A ( bronsted acid is proton donar and base is proton acceptor )

35. B ( ka * kb = kw = 10 ^ -14 )

36. Answer = C

pH = - log ( H+ ) = - log ( 0.02 ) = 2 - log 2 = 2 - 0.3 = 1.7