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10 Nov 2019
A 1.0-liter solution contains 0.25 M HF and 0.83 M NaF (K_a for HF is 7.2 times 10^-4). What is the pH of this solution? A) 3.14 B) 3.66 C) 2.62 D) 0.52 E) 10.34 What is the pH of a solution that results when 0.010 mol HNO_3 is added to 500. mL of a solution that is 0.10 M in aqueous ammonia and 0.55 M in ammonium nitrate. Assume no volume change. (The K_b for NH_3 = 1.8 times 10^-5.) A) 9.26 B) 5.05 C) 10.11 D) 8.40 E) 8.71 Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH_3 (K_b for NH_3 = 1.8 times 10^-5). A) 2.87 B) 4.98 C) 5.12 D) 7.00 E) 11.12 50.00 mL of 0.10 M HNO_2 (nitrous acid, K_a = 4.5 times 10^-4) is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, the pH in the titration flask will be A) 2.17 B) 3.35 C) 2.41 D) 1.48 E) 7.00
A 1.0-liter solution contains 0.25 M HF and 0.83 M NaF (K_a for HF is 7.2 times 10^-4). What is the pH of this solution? A) 3.14 B) 3.66 C) 2.62 D) 0.52 E) 10.34 What is the pH of a solution that results when 0.010 mol HNO_3 is added to 500. mL of a solution that is 0.10 M in aqueous ammonia and 0.55 M in ammonium nitrate. Assume no volume change. (The K_b for NH_3 = 1.8 times 10^-5.) A) 9.26 B) 5.05 C) 10.11 D) 8.40 E) 8.71 Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH_3 (K_b for NH_3 = 1.8 times 10^-5). A) 2.87 B) 4.98 C) 5.12 D) 7.00 E) 11.12 50.00 mL of 0.10 M HNO_2 (nitrous acid, K_a = 4.5 times 10^-4) is titrated with a 0.10 M KOH solution. After 25.00 mL of the KOH solution is added, the pH in the titration flask will be A) 2.17 B) 3.35 C) 2.41 D) 1.48 E) 7.00
Trinidad TremblayLv2
12 May 2019