Consider the titration of 30.0 mL of 0.0700 M
(CH3)3N (a weak base; Kb =
6.40e-05) with...
90.2K
Verified Solution
Link Copied!
Question
Chemistry
Consider the titration of 30.0 mL of 0.0700 M(CH3)3N (a weak base; Kb =6.40e-05) with 0.100 M HCl. Calculate the pH after the followingvolumes of titrant have been added:
(a) 0.0 mL
pH = _________
(b) 5.3 mL
pH = __________
(c) 10.5 mL
pH = ____________
(d) 15.8 mL
pH = _____________
(e) 21.0 mL
pH =___________
(f) 39.9 mL
pH = __________
Answer & Explanation
Solved by verified expert
4.0 Ratings (798 Votes)
For CH33N let us assume CH33N B for simplicity so CH33N H2O CH33NH OH becomes B H2O HB OH Kb HBOHB so a no volume of acid B H2O HB OH Kb HBOHB in equilibrium for 1 mol of OH we hava always 1 mol of HB HB OH x the dissociation fraction of acid B Mx 007x Account for dissociation 64105 xx007x solve with quadratic formula x OH 0002084 pOH logOh log0002084 268110 pH 14pOH 14268110 113189 b 53 mL
See Answer
Get Answers to Unlimited Questions
Join us to gain access to millions of questions and expert answers. Enjoy exclusive benefits tailored just for you!
Membership Benefits:
Unlimited Question Access with detailed Answers
Zin AI - 3 Million Words
10 Dall-E 3 Images
20 Plot Generations
Conversation with Dialogue Memory
No Ads, Ever!
Access to Our Best AI Platform: Flex AI - Your personal assistant for all your inquiries!
