Ksp
Definition
Ksp stands for Solubility Product Constant. It represents how much an ionic compound can dissolve in water before it reaches saturation and starts forming precipitates.
Analogy
Consider your favorite soda drink; there's only so much gas (carbon dioxide) it can hold before it starts releasing bubbles (precipitating). That limit is similar to what Ksp represents for ionic compounds in water.
Related terms
Saturation: The state or process that occurs when no more of something can be absorbed, combined with, or added.
Ionic Compound: A compound composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal.
Precipitation Reaction: A reaction in which an insoluble substance forms and separates from the solution.
"Ksp" appears in:
Study guides (2)
Practice Questions (14)
What happens to Ksp if a substance is dissolved into a solvent other than water?
Consider a solution of 0.001M KI and 0.1M KCl. If Ag⁺ ions are added, what concentration is needed to begin causing AgI to form precipitate? (Ksp of 1.5 x 10⁻¹⁶)
Consider a solution of 0.001M KI and 0.1M KCl. If Ag⁺ ions are added, what concentration is needed to begin causing AgCl to form precipitate? (Ksp of 1.6 x 10⁻¹⁰)
Consider the solid AgCl with a certain Ksp. What is an expression, measured in M, for the solubility of AgCl?
Consider the solid Ca₃(PO₄)₂ with a certain Ksp. What is an expression comparing Ksp and its molar solubility (represented by x)?
Consider the equation PbCl₂ (s) ⇌ Pb²⁺ (aq) + 2Cl⁻ (aq), where saturation is reached at [Cl⁻] = 0.1M. What is the Ksp?
Consider the equation CaF₂ (s) ⇌ Ca²⁺ (aq) + 2F⁻ (aq), where saturation is reached at [Ca²⁺] = 0.1M. What is the Ksp?
What is the Ksp of nickel sulfide if its solubility is 2.97 x 10⁻⁹ grams per liter?
If the calculated Q for a reaction is greater than Ksp, what does this signify?
If the calculated Q for a reaction is less than Ksp, what does this signify?
A high Ksp is representative of what characteristic?
Per College Board, what is the Ksp required for a salt to be considered soluble?
What is the molar solubility of NaCl (Ksp 1.6x10⁻¹⁰) in pure water and in a 0.1M solution of AgCl?
What is the molar solubility of Ca₃(PO₄)₂ (Ksp 2.07 x 10⁻³³) in 0.5M CaCl₂ solution?
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