What is Ksp in chemistry?
We can represent its solubility in water in the following way:
As for any equilibrium, we can write (and quantify) this equilibrium:
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Ksp, or the solubility product constant, is a measure of the extent to which a sparingly soluble salt dissolves in water. It represents the equilibrium constant for the dissolution reaction of a solid salt into its respective ions in a saturated solution.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- Calculate the equilibrium concentration of #"NO"# if the equilibrium concentration of #"N"_2# is #"0.036mol L"^(-1)# and that of #"O"_2# is #"0.0089 mol L"^(-1)# ?
- Suppose #"2.83 g"# of ammonium chloride solid is placed into a closed, evacuated rigid container, and allowed to decompose at a certain temperature. If 40% of it decomposed into ammonia and hydrogen chloride gas, what is #K_c# for this reaction?
- What happens to the color of the #Fe^(2+)# when the equivalence point is reached?
- What is Le Chatelier's principle and why is it important?
- For complex formation of iron(III) thiocyanate at a certain ionic strength, #K_f = 1099#. If its initial concentration is #"4.0 M"#, determine the equilibrium concentration of all species in solution for the dissociation of iron(III) thiocyanate in water?

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