Consider the titration of 145 mL of 1.45 M triethylamine, (CH3CH2)3N (Kb = 4.0 x 10-4)...
Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant. (a) 15.00 mL: pH = (b) 20.40 mL: pH = (c) 29.00 mL: pH =
Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant. a) 12.00 mL b) 20.70 mL c) 30.00 mL
Find the pH during the titration of 20.00mL of 0.1000 M triethylamine, (CH3CH2)3N, (Kb = 5.2x10^-4) with 0.1000 M HCl solution after the following additions of titrant. 1.) 0 mL 2.) 10.00 mL 3.) 20.00 mL 4.) 25.00 mL
Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant. (a) 15.00 mL: pH = (b) 20.40 mL: pH = (c) 29.00 mL: pH =
A 25.0 mL aqueous sample of 0.220 M triethylamine, (CH3CH2)3N, where Kb = 5.2*10^-4 is titrated with 0.500 M HCl(aq). 1) What is the pH before any titrant has been added? (Show all work.) 2) What is the pH at the midpoint of the titration? (Show all work.) 3) What is the pH after a total of 8.0 mL of HCl has been added? (Show all work) 4) What is the pH at the equivalence point of the titration? (Show...
A 25.0 mL aqueous sample of 0.220 M triethylamine, (CH3CH2)3N, where Kb = 5.2x10^-4 is titrated with 0.500 M HCl(aq). 1) What is the pH before any titrant has been added? (Show all work.) 2) What is the pH at the midpoint of the titration? (Show all work.) 3) What is the pH after a total of 8.0 mL of HCl has been added? (Show all work) 4) What is the pH at the equivalence point of the titration? (Show...
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
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
1- Determine the pH during the titration of 39.4 mL of 0.374 M triethylamine ((C2H5)3N , Kb = 5.2×10-4) by 0.374 M HClO4 at the following points. (a) Before the addition of any HClO4 (b) After the addition of 16.2 mL of HClO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 55.6 mL of HClO4
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 =