a. Calculate the pH of a 0.205 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10) and the equilibrium concentrations of the weak base and its conjugate acid.
pH | = | |
[C6H5NH2]equilibrium | = | M |
[C6H5NH3+]equilibrium | = | M |
b. Calculate the pH of a 0.0555 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3) and the equilibrium concentrations of the weak base and its conjugate acid.
pH | = | |
[C5H11N]equilibrium | = | M |
[C5H11NH+ ]equilibrium | = | M |
a. Calculate the pH of a 0.205 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10)...
1. Calculate the pH of a 0.447 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10). 2. Calculate the pH of a 0.0590 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb = 4.10×10-4). 3. Calculate the percent ionization of a 0.545 M solution of hydrocyanic acid.
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
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 = ...
Calculate the pH of a 0.0410 M aqueous solution of ethylamine (C2HsNH2, Kb 4.3x10) and the equilibrium concentrations of the weak base and its conjugate acid pH [C2HsNH2]equilibrium C2H5NH3 lequilibrium
1. Calculate the pH of a 0.543 M aqueous solution of codeine (C18H21O3N, Kb = 8.9×10-7). pH = 2. Calculate the pH of a 0.1250 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3). pH = 3. Calculate the pH of a 0.0774 M aqueous solution of the weak base triethylamine ((C2H5)3N, Kb = 5.20×10-4). pH =
What is the pH of a 0.15 M solution of the weak base aniline (C6H5NH2; Kb = 3.8 x 10-10) A) 5.12 B) 8.88 C) 13.18 D) 9.42 E) 10.24
a) Kb for aniline (C6H5NH2) is 4.3×10−10. Calculate KaKa for the C6H5NH3+C6H5NH3+ cation.. b) Calculate the pH of 0.40 MNH3 (Kb=1.8×10−5).
1)In the laboratory, a general chemistry student measured the pH of a 0.405 M aqueous solution of aniline, C6H5NH2 to be 9.254. Use the information she obtained to determine the Kb for this base. Kb(experiment) = 2) In the laboratory, a general chemistry student measured the pH of a 0.405 M aqueous solution of codeine, C18H21O3N to be 10.793. Use the information she obtained to determine the Kb for this base. Kb(experiment) = 3) The hydroxide ion concentration, [OH-], of...
Calculate the pH of a 0.10 M solution of aniline(C6H5NH2, Kb=3.8 x 10-10.) A. 11.21 B.5.21 C. 9.42 D.2.79 E. 8.79
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M