Question

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. B) A proton acceptor. C) An electron pair donor. D) An electron pair acceptor. E) An anphoteric species. Q(35) What is the relationship between Ka and Kb for a conjugate acid base pair? A) Kw=Ka+Kb B) Kw=K.*Kb C) Kw=Ko-Kb. D) Kw=Ka/Kb. E) Kw=K? Q(36) What is the pH of a 0.02 M solution of HBr (a strong acid)? A) pH=1. . B) pH=1.2 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 B) pH=6.2 | C) pH=7 D) pH=9.3 . E) pH=12.6 Q(38) What is the pH of a 0.0200 M aqueous solution of HF (K. of HF is 6.8 * 10-4)? A) pH=1.4 | B) pH=2.4 C) pH=47 D) pH=9,3 E) pH=12.6 Q(39) What is the pH of a 0.1 M aqueous solution of NH3 (Kb of HF is 1.8 * 10-5)? A) pH=1.4 | C) pH=6.7 D) pH=11.3 . | E) pH=12.6 Q(40) 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 p orbitals. 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) electron pair acceptor

34. A) proton donor

35. B) K_w = K_{a *} K_b

36. C) pH = 1.7

37. E) pH = 12.6