Organic Chemistry Acidity Problem: Explain the pKa Difference Acetic Acid & Chloroacetic acid

In this video I will explain the difference in pka between acetic acid (carboxylic acid) and chloroacetic acid (carboxylic acid). It is critical that an organic chemistry student is able to not only predict what protons on a molecule are acidic but why they are the most acidic. In this video I will demonstrate the steps that a student should use to explain the differences in pka (ka). pka = -log ka.

In general when examining conjugate bases and attempting to determine which one is more basic it is resonance we turn to for the answer. However, if both conjugate bases have equal resonance forms then we must turn to induction for the answer. Induction or the inductive effect is the pulling of electron density through the sigma bonds. Induction is the result of an electronegative atom being bonded to carbon thus making the carbon more positive (delta positive, partial positive). Consider that if a negatively charged atom is attached to a carbon with a greater delta positive charge than typical the more attracted the anion will be to that carbon and the less attractive other cations (protons) will be to the anion.

The large the ka the more acidic a molecule is. The lower the pka the more acidic a molecule is.

Consider the following reaction:

HA + H2O - H3O+ + A-

The ka expression for the above reaction would be: ka = [H3O+][A-]/[HA].

To achieved a large ka using the above expression the concentration of H3O+ and the conjugate base(A-) must be large and the concentration of the parent acid must be low. In other words the more the reaction favors the right side of the reaction the more acidic it is. When comparing two different molecules it is important to understand that acidity is referring to the ka and ka is referring to the concentration of H3O+ and the conjugate base (A-). The higher the concentration of conjugate base at equilibrium the more to the right the reaction is. It stands to reason that if we can predict the relative basicity of two conjugate bases we can predict how far to the right a reaction goes and therefore predict which parent acid is more acidic.

In organic chemistry I (Intro to organic chemistry) it is important to be able to identify the acidic protons (hydrogens) and be able to predict how strong or weak the conjugate base will be. An important factor that effects the conjugate base is resonance. If a conjugate base resonances it is likely to be less basic and therefore more stable in water. Remember the stronger the acid the weaker the conjugate base. Strong acids have weak conjugate bases. Strong bases have weak conjugate acids. Acids and bases are important. I wish you all success in organic chemistry.

Being able to push arrows and draw resonance forms is a critical skill that you must learn to be successful in organic chemistry. Performing acidity practice problems will help you be successful in organic chemistry.

This video is part of a series called How to be Successful in Organic Chemistry. It this series I go over numerous problems that a student could expect to see in there organic chemistry 1 course. Doing organic chemistry practice problems will make you more successful in organic chemistry and biochemistry.

I recommend that you download the problem from the link below and attempt the problem yourself and use this video to correct your work.

Download the problem from this video at the following link:

https://www.dropbox.com/s/i2n5d4byaru8zsc/compare%20pka%20acetic%20acid%20cl%20acetic%20acid%20watermark.pdf?dl=0

Good Luck and Good Chemistry!

Please subscribe to my channel by clicking the link below!
https://www.youtube.com/c/AllInwithDrBetts?sub_conformation=1

Like this video and leave a comment below!

#induction #resonance #acids #bases
#organicchemistry
#organiccompounds
#organicproblems
#organictutor
#simpleresonance
00:00 Introduction
00:29 reacting each acid with water
01:58 Why is one more acidic than the other?
02:35 Induction to stabilize conjugate bases
06:50 Conclusion