Determine the pH of 0.250 M (CH3)3N Kb = 7.4 x10-5 for (CH3)3N
a. Determine the pH during the titration of 31.3 mL of 0.264 M trimethylamine ((CH3)3N, Kb = 6.3×10-5) by 0.264 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI ____ (b) After the addition of 12.6 mL of HI ____ (c) At the titration midpoint ____ (d) At the equivalence point ____ (e) After adding 43.8...
Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.400-05) with 0.100 M HBr. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL (b) 5.3 mL (c) 10.5 mL pH = pH = pH = (d) 15.8 ml (e) 21.0 mL (f) 27.3 mL pH = pH = pH =
Determine the pH of a 2.0 x10^-4 M solution of aniline hydrochloride (C6H5NH3Cl). Kb aniline (C6H5NH2) = 3.98 x10^-10
Calculate the pH during the titration of 20.00 mL of 0.1000 M trimethylamine, (CH3)3N(aq), with 0.1000 M HCl(aq) after 21 mL of the acid have been added. Kb of trimethylamine = 6.5 x 10-5.
Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.40e-05) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added:
Consider the titration of 60.0 mL of 0.0400 M (CH3)3N (a weak base; Kb = 6.40e-05) with 0.100 M HBr. 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) 38.4 mL pH =
Determine the pH during the titration of 39.9 mL of 0.349 M triethylamine ((C2H5)3N , Kb = 5.2×10-4) by 0.349 M HBr at the following points. (a) Before the addition of any HBr (b) After the addition of 17.7 mL of HBr (c) At the titration midpoint (d) At the equivalence point (e) After adding 61.0 mL of HBr
Calculate the PH of a 0.36 M aqueous solution of NH4NO3. Kb of NH3= 1.8 x10^-5. Please show your work; I know how to do a normal problem but I am confused because the Kb is only for NH3, not the whole thing. Thanks!
25.0 ml of a 0.100 M trimethylamine (CH3)3N (a base like ammonia) Kb = 6.3×10−5, are transferred in an Erlenmeyer flask and titrated with 0.100 M of HCl. Predict pH, pOH, concentration of trimethylamine, concentration of the conjugated acid (CH3)3NH+, and concentration of HCl in the Erlenmeyer flask when: (a) 0 mL of HCl solution are added to the Erlenmeyer flask (a) 12.5 mL of HCl solution are added to the Erlenmeyer flask (c) 25 mL of HCl solution are...
Determine the pH during the titration of 39.8 mL of 0.293 M triethylamine ((C2H5)3N, Kb = 5.2×10-4) by 0.293 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI (b) After the addition of 16.2 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 58.1 mL of HI