Ask Question
7 September, 07:22

Be sure to answer all parts. 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) 11.00 mL: pH = (b) 20.60 mL: pH = (c) 25.00 mL:

+3
Answers (1)
  1. 7 September, 08:25
    0
    (a) 10.62

    (b) 2.82

    (c) 1.95

    Explanation:

    The neutralization reaction in this question is

    (CH3CH2) 3N + HCl ⇒ (CH3CH2) 3NH⁺ + Cl⁻

    The problem can be solved by calculating the number of moles of triethylamine after addition of the portions of HCl. Since it is a weak base if it is not consumed completely, that is in excess we will have a buffer of a waek base. If its consumed completely the pH will be determined by the strong acid HCl.

    The pOH for a buffer of a weak base is gven by

    pOH = pKb + log [ (CH3CH2) 3NH⁺] / [ (CH3CH2) 3N]

    (a) 11 mL of 0.100 M HCl

    mol HCl = 0.011 L x 0.100 mol/L = 0.0011 mol HCl

    mol (CH3CH2) 3N reacted = 0.0011 mol

    mol (CH3CH2) 3NH⁺ produced = 0.0011 mol

    mol (CH3CH2) 3N initially = 0.020 L x 0.1000 mol/L 0.0020 mol

    mol (CH3CH2) 3N left = 0.0020 mol - 0.0011 = 0.0009 mol

    pKb = - log Kb = - log (5.2 x 10⁻⁴) = 3.284

    Now we can compute pOH,

    pOH = 3.284 + log (0.0011 / 0.0009) = 3.37

    pH = 14 - pOH = 14 - 3.37 = 10.62

    (b) 20.60 mL HCl

    mol HCl = 0.0206 L x 0.100 mol/L = 0.00206

    mol (CH3CH2) 3N consumed = 0.0020 mol

    This is so because the acid will consume completely the 0.0020 mol of the weak base we had originally present.

    Now the problem circumscribes to that of calculating the pH of the unreacted HCl

    Total Vol = 0.0206 L + 0.02 L = 0.0406 L

    mol HCl = 0.0206 L x. 100 = 0.00206 mol

    mol HCl left = 0.00206 mol - 0.0020 mol = 0.00006 mol

    [HCl] = 0.00006 mol / 0.0406 L = 0.0015 M

    Since HCl is a strong acid (100 % ionization):

    pH = - log [H⁺] = - log (0.0015) = 2.82

    (c) We will compute the pH in the same way we did for part (b)

    mol HCl = 0.025 L x 0.100 mol/L = 0.0025 mol

    mol HCl left = 0.0025 mol - 0.0020 mol = 0.0005

    Total Volume = 0.020 L + 0.025 L = 0.045 L

    [HCl] = 0.0005 mol / 0.045 L = 0.111

    pH = - log (0.111) = 1.95
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2) 3N (Kb = 5.2 * 10-4), with ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers