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Question 17 5 pts What is the pH of a 1.113 M aminomethyl propanol solution? Aminomethyl...
Question 17 5 pts What is the (OH) of a solution with a pH of 5.8. 6.33x 10°M 07.6 x 101 M. 1.58 x 10-6M 1x 10-'M
a)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH of a 0.289 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H15O3N]equilibrium = M [C6H15O3NH+]equilibrium = M b) Calculate the pH of a 0.0338 M aqueous solution of dimethylamine ((CH3)2NH, Kb = 5.9×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ...
a)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH of a 0.289 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H15O3N]equilibrium = M [C6H15O3NH+]equilibrium = M b) Calculate the pH of a 0.0338 M aqueous solution of dimethylamine ((CH3)2NH, Kb = 5.9×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH =...
QUESTION 4 What is the pH of 31.56 mL of a 0.1528 M solution of a weak monoprotic basic base (B:, Kb = 2.41 x 10-0) @ the midway point of a titration with 0.1236 M HCIO3? %3D Your answer must have 2 decimal places. QUESTION 5 What is the pH of 37.88 mL of a 0.1142 M solution of a weak basic base (B:, Kp = 7.95 x 10-4) that has been titrated with 18.45 mL of 0.1831 M...
A 0.297-M aqueous solution of (CH3)2NH (dimethylamine) has a pH of 12.1. Calculate the pH of a buffer solution that is 0.297 M in (CH3)2NH and 0.236 M in (CH3)2NH2+. pH =
Question 48 5 pts What is the pH of a 2.2 M solution of HOBr (K, - 2.0 x 10°)? Report your answer to the nearest whole number.
A solution contains 0.327 M ammonium iodide and 9.45×10-2 M ammonia. The pH of this solution is . The compound dimethylamine is a weak base like ammonia. A solution contains 0.306 M (CH3)2NH2+ and 0.185 M dimethylamine, (CH3)2NH. The pH of this solution is .
What is the pH of a 0.00831 M solution of NH(CH3)3Cl? The Kb of N(CH3)3 is 6.3×10–5.
D Question 7 10 pts It is desired to buffer a solution at pH - 4.30. What molar ratio of CH3COOH to NaCH3COO should be used? The Ka for CH3COOH is 1.8 x 10-5. 10 pts D | Question 8 How much NH4CI must be added to 2.00 liters of 0.26 M aqueous ammonia to give a solution with pH 8.55? Assume no volume change due to the addition of NH4CI. The Kb of ammonia is 1.8 x 105, and...
Consider a 0.84 M solution of (CH3)2NH (Kb = 1.3x10-3). Mark the major species found in the solution. -(CAH)2NH AOH H2O (CH3)2NH2 Calculate the pH of this solution. pH =