Problem: Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH  3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant:(c) 15.00 mL

FREE Expert Solution

Reaction:

(CH3CH2)3N(aq) + HCl(aq) → (CH3CH2)3NH+(aq) + Cl-(aq)


Step 1: Calculate the initial amount (in moles) of each species:

Given:

20.00 mL of 0.1000 M (CH3CH2)3N
15 mL of 0.1000 M HCl


molarity (M)=molL

moles (CH3CH2)3N=(0.1000mol (CH3CH2)3NL) (20.00 mL x 10-3 L1 mL)

(CH3CH2)3N = 0.002 mol NH3

98% (401 ratings)
View Complete Written Solution
Problem Details

Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH  3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant:

(c) 15.00 mL

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Base Strong Acid Titrations concept. You can view video lessons to learn Weak Base Strong Acid Titrations. Or if you need more Weak Base Strong Acid Titrations practice, you can also practice Weak Base Strong Acid Titrations practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Weems' class at Johnson County Community College.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.