33. A one liser solution contains 0.200 M CH COOH 40. An aqueous buffer contains

Question

33. A one liser solution contains 0.200 M CH COOH 40. An aqueous buffer contains acetic acid (CH,COOH) and (K 1.8x10) and 0.200 M CH,cOONa. The initial pH is 4.74, Calculate the pi when 0 0500 mole of HCI is sodium acetate (CH,COONa). Which reaction shows how the buffer minimizes the pH change when HC added to the solution. (A) 423 (B) 452 (C) 4.74 (D) 496 Lowry acid-base reaction? (A) H)+OH)H,O) (B) CH,COOH) OHaq) 34, which is a Lewis ucid-base reaction, but Bronsted. (A) CH,COOH(aq)+H,o) (C) CH,COO(aq) + H.(aq)=CH,COOH(aq) (D) NH,(g)+BF (p) H,NBFs) 41. Choose the correct ranking based oa acid strength for these three acids. Each picture is a representation of ar ionized acid that is dissol ved in water. The water molecules are not included in the pictures for the sake of clarity 35. Which statement is true about the pH of un aqueous (A) As pH increases, pkw increases (B) As pH increases.pkw decreases. (C) As pH increases, bydromium ion concentration (D) As pH increases, hydroxide ion concentration 36. The K, of a weak acid is 1.8x10. What is the K, of its conjagate base? (A) 5.6x10 (C) 5.6x10 (B) 1.8x10 (D) 1.8x10 (C) HZ> HY>HX 37. Which represents the titration of ammonia with HCI? What is the AG, in kJ for this reaction? 42. 395 (A) -2894 (B) -592 (C) +2850 (D) Not esough information given 43. For the reaction, H-2855.1 kJ, AS92.63 K Under standard conditions, this reaction is (A) non-spontaneous at all temperatures (B) spontancous at tow temperatures. (C) spontaneous at high temperatures (D) spontaneous at all temperatures mLofHCI 38. At50°C, p ,#1326, what is the pH ofpure water at this temperature? (A) 663 (B) 7.00 (C) 7.37 (D) 13.26 44. For this reaction, the system becomesdisordered and 39. What is the conjugate base of H,PO,? the entropy change isthan zero. (A) PO (B) HPO. (C) H,PO, (D) PO,2 (A) more, les (C) less, less (B) more, greater (D) less, grealer

Explanation / Answer

34)d because the BF2 is the acid and doesn't have protons to donate. 35) d because when the pH increases is lowering the concentration of H+ and increasing the concentration of OH- 36) Kw=Ka*Kb Kb= Kw/Ka = 5,6*10^-11 answer is A 37) d, because in a titration the curves changes drastically at the equivalence point, and because the NH3 is a base inicially has a basic pH 38) A 39) b 40) c 43) b 44)c 49)a

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