Question

Part A Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2 Express your answer numerically using two decimal places. View Available Hint(s) 20 A20 0 2 ? pH Submit Part B Calculate the pH of a 0.10 M solution of NaOH Express your answer numerically using two decimal places. View Available Hint(s) VO ALDO ? Submit Part

Answer 1

Date Page Solution 1) part A The value provided in the Molarity of BalO4) = 0.10m question are, we have to find the pH. we have, Ba (Ohla - Bat+200 45 .. the equation to find the patis рен - - log Гон) s-log (Qx0.1) - poh = 0.6989 pH = 14-pon = '14-0.6989 -= 13.301 Hence pH of 0.1M of Ba(OH)2 is 13. 301.

2) part B question are The value provided in the Molarity of NaOH = 0.10m we have to find the oilm solution of Naon we have, NaOH Nat +[04] The equation to find the plot is OH = -log [ort = -log (180.1) pH = 14 - poH = 14-1= 13 = 13.00 Hence the pH of is 13.00 oilM Solution of NaOH

Date Page part c The value provided in the question are, Molarity of Hydrazine solution = 0.1M kb of Hydroazine = 1.3810-6 we have to find the pH of Hydrazine Hydrazine Reaction with water H₂ NN He can t How H₂NNH3 + cas) to HER ky sur bydrazine, kb = [H₂NNH₂] [ou] H₂NNH2 Noto - Toril Assouman A * my kb = [ougat [Nata] [on] = kb x [Notta = 1.3 X 166 Xoil [on] - J 1.3x107

[ori] = 3.6058104 equation to find the pon of the solution рона — log Гон) = 3.443 pH of Hydrazine, pH = 14 - pon - 14 – 3.443 = 10.556 solution. Hence, pH os o. lm by desazine with kh al-3x10-6 is 10.556