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- What is the pH of a 0.05M solution of diethylamine? ((CH3CH2)2NH)? (Ignore activities) 10. What...
9. What is the pH of a 0.05M solution of diethylamine? (ICH,CH), NH)? ilgnore activities) 10. What is the pH of a solution which contains 0.05 moles benzoic acid and 0.075 moles sodium benzoate dissolved to make 0.5000 L of solution? (Ignore Activities)
10. What is the pH of a solution which contains 0.05 moles benzoic acid and 0.075 moles sodium benzoate dissolved to make 0.5000 L of solution? (Ignore Activities)
10. What is the pH of a solution which contains 0.05 moles benzoic acid and 0.075 moles sodium benzoate dissolved to make 0.5000 L of solution? (Ignore Activities)
10. What is the pH of a solution which contains 0.05 moles benzoic acid and 0.075 moles sodium benzoate dissolved to make 0.5000 L of solution? (Ignore Activities)
9. What is the pH of a 0.05M solution of diethylamine? -? (CH,CH2)2NH)? (Ignore activities)
What is the pH of a solution that is 0.456 M in diethylamine (CH3CH2)2NH and 0.547 M in diethylamine chloride (CH3CH2)2NH2Cl? The Kb for diethylamine is 6.9 x 10-4.
a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...
a) Given 20.00 mL of 0.2000 M diethylamine (CH3CH2)2NH (Kb = 3.1 x 10-4), determine the pH for the titration against 0.1000 M Hal at the following HCl volumes: i) 0.0 mL, ii) 1/4 eq pt, iii) 15.00 mL, iv) 20.00 mL, v) 3/4 eq pt, vi) 35.00 mL, vii) at the eq pt, viii) 50.00 mL, ix) 20.00 mL beyond the eq point. b) Use the results of part 'a' to sketch the titration curve. Make the line as...
(1) Given the following information: hydrocyanic acid HCN Ka = 4.0×10-10 diethylamine (C2H5)2NH Kb = 6.9×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium will the reactants or products be favored? (3) Will the pH of the resulting solution be greater than, less than, or roughly equal to 7?...
[References) A 0.079 M solution of diethylamine has a pH of 12.00. What is the value of Ky for this weak base? (C2H6)2NH(aq) + H2O(l) = (C2H6)2NH2+ (aq) + OH(aq) K- Submit Answer Try Another Version 10 item attempts remaining