A 0.297-M aqueous solution of (CH3)2NH (dimethylamine) has a pH of 12.1. Calculate the pH of...
Calculate the pH of a 0.0198 M aqueous solution of dimethylamine ((CH),NH, Kn=5.9x104) and the equilibrium concentrations of the weak base and its conjugate acid. PH M [(CH3)2NH)equilibrium [(CH3)2NH2 Lequilibrium = C =
An aqueous solution contains 0.449 M dimethylamine ((CH3)2NH). How many mL of 0.249 M perchloric acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.500? _________mL
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 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 .
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 =
The pOH of an aqueous solution of 0.355 M dimethylamine (a weak base with the formula (CH3)2NH) is .
Three organic amines ( trimethylamines (ch3)2NH+ pka=9,8, dimethylamine (ch3)2NH2+ pka=10.78, monomethylamine (ch3)2Nh2+ pka=10.64 and one inorganic cation (NH4+) aka= 9.24 was achieved using a ion-exchange column containing sulfonate (SO3-) group attached to polystyrene divinylbenzene backbone. What is the best elution from least to most retained of these four catonic compounds on this stationary using a mobile phase ph of 10.2?
The pH of a 0.164 M aqueous solution of (CH3)2NH is 11.98. What is the value of Kb? A. 6.10 * 10-14 B. 5.84 * 10-4 C. 5.80 * 10-2 D. 6.70 * 10-24 E. 1.86
The pH of a 0.164 M aqueous solution of (CH3)2NH is 11.98. What is the value of Kb? A. 5.84 * 10-4 B. 6.10 * 10-14 C. 6.70 * 10-24 D. 5.80 * 10-2 E. 1.86
A 23.4 mL sample of 0.250 M dimethylamine, (CH3)2NH, is titrated with 0.224 M hydrochloric acid. At the titration midpoint, the pH is?