Can someone please thoroughly explain titrations and their graphs? Thank you!

What is the purpose of a titration? What/where is the equivalence point? Half-equivalence point? Where are those points located on a titration graph? And is there any other information that you think is helpful/important?

2 Answers
Apr 23, 2017

Answer:

Please see explanation. I don't know about half-equivilance points / graphs though.

Explanation:

A titration can be performed in order to determine the concentration of an acid or a base by neutralizing it with another acid or base which you know the concentration of.

This is useful because, if you had HCl with an unknown concentration, it can either scar you for life when you touch it, or irritate you for a while. To be safe, we can use titration to determine its concentration.

If you are doing a lab with titration, it must be very precise. In general, you place acid-base indicator such as phenolphthalein to find out when the equivalence point is reached. This is the point where the indicator has switched colours, indicating the volume of the acid or base that was used to neutralize the acid or base in question. Using the equation #c_1V_1 = c_2V_2# you can find the concentration of the acid or base in question.

Apr 23, 2017

Take the titration curve for #"NaOH"# added to acetic acid as an example:

https://www.researchgate.net/

The rest of this answer will assume strong base is added to weak acid. However, strong acid could just as easily be added to weak base, and the above graph would be flipped horizontally.

Let's say you know what your acid is already. Then the point of a titration is to:

  • verify the concentration of your base (whose concentration might be hard to determine if the solid used to make it is hygroscopic---that is, if it absorbs moisture in the air).
  • to check the #"pKa"# of your acid.

That is done by knowing the mass you used to make your acid solution, so that you can calculate its starting concentration with a good amount of certainty.

If you do NOT know what your acid is, then the titration is done to determine its #"pKa"# and thus, possibly its identity.

A common lab procedure is to first use a known acid (your primary standard) that you've prepared to determine the concentration of your secondary standard (in this case, #"NaOH"#). Then, the secondary standard can be used to determine the concentration of an unknown acid.


BUFFER REGION

The side of the graph before the steep rise is the buffer region. It is where your weak acid, while being neutralized, is in the presence of its conjugate weak base (which is being produced as the weak acid is being neutralized).

It is here that the Henderson-Hasselbalch equation can be used.

EQUIVALENCE POINT

The equivalence point is the spot indicated on the graph by #V_e#, the volume used to reach it. It is where a steep rise in the #"pH"# occurs, which is called an inflection point. This volume is the volume of titrant (e.g. #"NaOH"# from a burette) you added in order to neutralize all of the substance being titrated exactly.

(That is, it is the volume of titrant that contains the exact number of mols you need to react with all of what you are titrating.)

Once you make it past here, you're at a part of the titration where you have only the weak conjugate base and any extra #"NaOH"# you add. Thus, the #"pH"# becomes higher than #7#, and peaks off at the #"pH"# of your #"NaOH"#.

HALF-EQUIVALENCE POINT

The half-equivalence point is what you'll need to locate to find the #"pKa"# of the titrated weak acid. It is quite easy to find once you have identified your equivalence point; simply halve the volume you needed to get to the equivalence point.

In other words, it is at #V_e/2#. On the above graph, it's at about #"42 mL"#, and it is in the buffer region. It is where the #bb("pH" = "pKa")# since the concentration of weak acid and its conjugate weak base are equal:

#"pH" = "pKa" + log\frac(["A"^(-)])(["HA"])#

Of course, the Henderson-Hasselbalch equation only works in the BUFFER REGION... at the equivalence point, the logarithm tends to infinity... #["HA"] -> 0#, and thus, #log(["A"^(-)]/0) -> oo#.