1
answer
1
watching
728
views
10 Nov 2019
For nitrous acid, HNO_2, K_a = 4.0 times 10^-4. Calculate the pH of 0.27 M HNO_2. A) 1.98 B) 0.57 C) 3.97 D) 12.02 E) none of these The pH of a 0.118 M solution of an aqueous weak acid (HA) is 3.20. The K_b for the weak acid is A) 5.4 times 10^-3 B) 4.0 times 10^-7 C) 3.4 times 10^-4 D) 3.2 E) none of these Calculate the pH of a 0.59 M solution of NH_4Cl. (K_b for NH_3 = 1.8 times 10^-5) A) 9.26 B) 4.74 C) 9.48 D) 4.52 E) 0.23 Calculate the K_a for an unknown monoprotic acid HX, given that a solution of 0.28 M LiX has a pH of 8.90. A) 2.3 times 10^-10 B) 3.5 times 10^-10 C) 1.8 times 10^3 D) 8.9 times 10^-5 E) 4.4 times 10^-5
For nitrous acid, HNO_2, K_a = 4.0 times 10^-4. Calculate the pH of 0.27 M HNO_2. A) 1.98 B) 0.57 C) 3.97 D) 12.02 E) none of these The pH of a 0.118 M solution of an aqueous weak acid (HA) is 3.20. The K_b for the weak acid is A) 5.4 times 10^-3 B) 4.0 times 10^-7 C) 3.4 times 10^-4 D) 3.2 E) none of these Calculate the pH of a 0.59 M solution of NH_4Cl. (K_b for NH_3 = 1.8 times 10^-5) A) 9.26 B) 4.74 C) 9.48 D) 4.52 E) 0.23 Calculate the K_a for an unknown monoprotic acid HX, given that a solution of 0.28 M LiX has a pH of 8.90. A) 2.3 times 10^-10 B) 3.5 times 10^-10 C) 1.8 times 10^3 D) 8.9 times 10^-5 E) 4.4 times 10^-5
Reid WolffLv2
30 Jan 2019