Molar Solubility solubility is the amount of solute that will dissolve in a given amount of solution at a particular temperature the molar solubility is the number of moles of solute that will dissolve in a liter of solution the molarity of the dissolved solute in a saturated solution for the general reaction: MnXm(s) nMm+(aq) + mXn−(aq) 6 6
Molar Solubility: (n solute/L saturated solution) 5 (g/L) Ksp: The equilibrium between the ionic solid and the saturated solution. Solubility: The quantity of solute that dissolves to form a saturated solution. In a particular sample, the concentration of silver ions was 1.2 x10-6 M and the concentration of bromide was 1.7x10-6 M. Write the solubility product expression for each of the following:Ī) Ca3(PO4)2 b) Hg2Cl2 c) HgCl2.
Name, Formula Ksp Aluminum hydroxide, Al(OH)3 3 x 10-34 Cobalt (II) carbonate, CoCO3 1.0 x 10-10 Iron (II) hydroxide, Fe(OH)2 4.1 x 10-15 Lead (II) fluoride, PbF2 3.6 x 10-8 Lead (II) sulfate, PbSO4 1.6 x 10-8 Mercury (I) iodide, Hg2I2 4.7 x 10-29 Silver sulfide, Ag2S 8 x 10-48 Zinc iodate, Zn(IO3)2 3.9 x 10-6 3Ĥ 1. 2ģ Table 1 Solubility-Product Constants (Ksp) of Selected Ionic Compounds at 250C Ksp = solubility product constant Ksp = Keq (s) Ksp = 1.1 x 10-10 Ksp represents the amount of dissolution (how much solid dissolved into ions), the smaller the Ksp value, the smaller the amount of ions in solution (more solid is present). SOLUBILITY Saturated Solution BaSO4(s) Ba2+(aq) + SO42-(aq) Equilibrium expresses the degree of solubility of solid in water.
Presentation on theme: "Solubility Equilibria"- Presentation transcript:Īll ionic compounds dissolve in water to some degree however, many compounds have such low solubility in water that we classify them as insoluble we can apply the concepts of equilibrium to salts dissolving, and use the equilibrium constant for the process to measure relative solubilities in water 1 1