Calculate the pH at the equivalence point when 75.0 mL of 0.250 M HCl is mixed with 0.350 M of CH3NH2. Kb = 4.4 x 10-4 Y
Posted: Wed May 18, 2022 10:28 am
Calculate the pH at the equivalence point when 75.0 mL of 0.250
M HCl is mixed with 0.350 M of CH3NH2. Kb = 4.4 x 10-4
Your answer must include a balanced equation for the new
equilibrium established, completed ICE box and assumption
check.
M HCl is mixed with 0.350 M of CH3NH2. Kb = 4.4 x 10-4
Your answer must include a balanced equation for the new
equilibrium established, completed ICE box and assumption
check.