How to Calculate Solubility from Solubility Product
In this JC2 webinar we want to learn how to calculate solubility from solubility product.
Let's take a look at this exercise.
When an amount of salt that corresponds to its solubility (x) dissolves, a saturated solution is formed.
A saturated solution is at equilibrium since the concentration of its ions are maximum and constant.
Therefore it is relevant to use solubility product (Ksp), the equilibrium constant for the dissociation of sparingly soluble salts.
This means that solubility and solubility product are related to each other.
Check out the following video for an in-depth discussion of the relationship between solubility and solubility product.
Let's turn our focus back on the dissociation of AgBr.
From the mole ratio we can deduce that x moldm-3 of AgBr (which corresponds to its solubility) will give x moldm-3 of Ag+ and x moldm-3 of Br-.
Therefore we can write down the Ksp and work out its relationship with solubility x.
We can then express solubility in terms of Ksp and calculate its value.
Let's look at another example Ag2CO3.
The method is essentially the same as the previous example.
We can write down its dissociation and figure out the concentration of Ag+ and CO32- in terms of solubility x.
We can then have a relationship between Ksp and x, and solve for x given Ksp.
Topic: Solubility Product, Physical Chemistry, A Level Chemistry, Singapore
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