Deciding whether a precipitate will form
We can cause a sparingly soluble salt to precipitate out of solution if the product of the concentration of the
Author: Sarah Parkes
The common ion effect
Silver chloride is a sparingly soluble salt. AgCl(s) ⇌ Ag+(aq) + Cl–(aq) Ksp = [Ag+(aq)] [Cl–(aq)] = 2.0 x 10-10
What is the solubility product?
Many ionic compounds are sparingly soluble – a good example is barium sulphate which has a solubility of 1.05 x
Understanding the relationship between Kc and Kp
We can derive a value for the equilibrium constant in a gaseous equilibrium system either using partial pressures, Kp, or
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Calculating Kp, the equilibrium constant, for a gaseous system.
For reversible reactions taking place in the gaseous phase it is more straightforward to think in terms of pressure rather
Continue readingCalculating Kp, the equilibrium constant, for a gaseous system.
Why don’t reactions at equilibrium go to completion?
To complete our understanding of systems that have achieved equilibrium, we need to look at the position of equilibrium through
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Equilibrium constants and equilibrium concentrations
Now it is time to introduce the concept of the equilibrium constant, Kc. Kc is basically a ratio – the
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Le Chatelier’s Principle
When we have a chemical reaction that has reached a state of dynamic equilibrium, there will be one particular set
What is position of equilibrium?
I’m sure you will all have seen a strip of magnesium burning in a Bunsen burner flame. It is a
Elimination reactions – dehydrating an alcohol
If we dehydrate an alcohol, we are essentially removing a water molecule and the product will be an alkene. The
Continue readingElimination reactions – dehydrating an alcohol