Friday, 9 September 2016
STEP ONE: Write a balanced equation for what has happened at the equivalence point. This is not an equilibrium reaction, it is neutralisation.
STEP TWO: Use the n, c, V relationship to calculate the concentration of the conjugate being formed in the neutralisation reaction.
STEP THREE: Write an equation for the dissociation of the conjugate with water.
STEP FOUR: Use the weak base (or weak acid) calculations, as appropriate, to find the concentration of hydronium ions.
STEP FIVE: Use this concentration to calculate pH.
The first things we need to master about buffers:
- Define a buffer
- Explain how a buffer works
- Calculate the pH of buffer solutions
On Mondays lesson, we can use our workbooks (Continuing Chemistry), and the internet as our resources, as well as the following videos:
Our next step is to work out how to make a buffer of a desired pH...
Tuesday, 6 September 2016
During a titration, the pH does not change uniformly. There are key points that can be calculated, and the remainder of the curve can be sketched from these:
This example starts with a weak acid in the conical flask. If it were a weak base, the calculations are a lot harder, but you can refer to THIS for how to do that calculation.
Equivalence Volume and Half-Equivalence Point
This relies on a good memory of the titration topic from last year. Once you know the equivalence volume, you are ready to mark the pH of the half-equivalence volume (pKa = pH).
This is very easy if you remember how to calculate the pH of a strong base (in this example). Put all of these points together to sketch the shape of the curve.
Weak Acid vs. Strong Base
Weak Base vs. Strong Acid
Wednesday, 31 August 2016
Whenever these questions are asked, they are worth Excellence. This is because there are six key steps to remember, and they need to be remembered in order!
- Write out the equation for the base acting as a an alkaline solution.
- Write a Kb expression.
- Calculate Kb from Ka
- Calculate [OH-] from the Kb expression (assuming [HB+] = [OH-]
- Calculate [H3O+] from [OH-], using KW
- Calculate pH