Consider a 0.84 M solution of (CH3)2NH (Kb = 1.3x10-3). Mark the major species found in...
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 =
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 = ...
Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 6.0 mL pH = (c) 12.0 mL pH = (d) 18.0 mL pH = (e) 24.0 mL pH = (f) 40.8 mL pH =
Consider the titration of 80.0 mL of 0.0200 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 4.0 mL pH = (c) 8.0 mL pH = (d) 12.0 mL pH = (e) 16.0 mL pH = (f) 30.4 mL pH = please help :) I'm super confused
Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL (b) 6.0 mL (c) 12.0 mL (d) 18.0 mL
Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb=0.000540) with 0.100M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 ml (b) 6,0 ml. (c) 12.0 mL (d) 18.0 mL (e) 24.0 ml (f) 38.4ml
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
Consider a solution of 0.31 M C5H5N (Kb = 1.7×10-9). Decide if each of the following is a major or minor species in the solution. Calculate the pH of this solution.
What is the pH of a 0.00391 M solution of NH(CH3)3Cl? The Kb of N(CH3)3 is 6.3×10^–5.