a) Given 20.00 mL of 0.2000 M diethylamine (CH3CH2)2NH (Kb = 3.1 x 10-4), determine the pH for the titration against 0.1000 M Hal at the following HCl volumes: i) 0.0 mL, ii) 1/4 eq pt, iii) 15.00 mL, iv) 20.00 mL, v) 3/4 eq pt, vi) 35.00 mL, vii) at the eq pt, viii) 50.00 mL, ix) 20.00 mL beyond the eq point.
b) Use the results of part 'a' to sketch the titration curve. Make the line as smooth as possible.
a) Given 20.00 mL of 0.2000 M diethylamine (CH3CH2)2NH (Kb = 3.1 x 10-4), determine the...
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) 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
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...
Determine the pH during the titration of 31.1 mL of 0.259 M diethylamine ((C2H5)2NH, Kb 6.9x10) by 0.259 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 12.9 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 48.5 mL of HI Determine the pH...
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
(1) Given the following information: hydrocyanic acid HCN Ka = 4.0×10-10 diethylamine (C2H5)2NH Kb = 6.9×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium will the reactants or products be favored? (3) Will the pH of the resulting solution be greater than, less than, or roughly equal to 7?...
Consider the titration of 145 mL of 1.45 M triethylamine, (CH3CH2)3N (Kb = 4.0 x 10-4) with 0.25 M HCI. How many mL of HCI will need to be added to the triethylamine, (CH3CH2)3N solution to reach a pH of 10.60? A: 311 B: 374 OC: 395 OD: 420. OE: 542
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...
2. 20.00 mL of 0.270 M HA (K. = 7.2 x 10-4) was titrated with 0.300 M sodium hydroxide (3 + 3 + 2 + 3 + 3 + 3 + 12 = 29 points) a) Write the titration equation and calculate volume of NaOH needed to reach the equivalence point. ml b) At what volume of the titrant would pH=pKa? Why? c) pH at the equivalence point when the acid and base are neutralized will be ..choose one of...