Solved Examples on Solubility Product Constant
Calculate the solubility product constant for silver chloride (AgCl) given that the concentration of Ag+ ions is 1.5×10 −5M and Cl− ions is 2.0×10−5M.
Ksp = [Ag+]×[Cl–]
Ksp = (1.5×10−5)×(2.0×10−5)
Ksp = 3.0×10 −10
Calculate the Molar Solubility for calcium hydroxide (Ca(OH)2) given that the solubility product constant for calcium hydroxide is 6.7 X 10-6
Ca(OH)2 = Ca2 + 2OH
Ksp = Ca2+OH2
Let x be molar solubility and Ca2+ = x and OH = 2x
6.7 × 10-7 = 4x 3
Now substitute x
x3= 6.7 × 10 -7
Calculate the solubility product constant for silver chloride (AgCl) given that the concentration of Ag+ ions is 0.5×10 −6M and Cl− ions is 3.0×10−9M.
Ksp =[Ag+]×[Cl–]
Ksp =( 0.5×10 −6M)×(3.0×10−9M)
How to Calculate Solubility Product Constant? Demystify the calculation of Ksp with an example. Consider silver chloride (AgCl) with [Ag+]=2.4×10−5M and [Cl-]=1.0×10−5M.
Ksp = Ag+ × Cl–
Ksp = (2.4×10−5)×(1.0×10−5)
Ksp = 2.4×10−10
Solubility Product – Definition, Formula, Significance
Solubility Product Constant, denoted as Ksp is an equilibrium constant which quantifies how much of a solute substance can dissolve in water. Solubility Product (Ksp) aims to explain the maximum amount of substances (solutes) that can dissolve in water (solvents) at a given temperature. it depends on the temperature, its value increases with the increase in temperature, which increases solubility. This article aims to learn Ksp, exploring its principles, formulas, constants, and practical applications.
Table of Content
- What is Solubility Product?
- Formula for Solubility Product
- Solubility Product Constant
- How to Calculate Solubility Product Constant?
- Solubility Product and Ionic Product
- Significance of the Solubility Product:
Contact Us