It means, . In other words, the molar solubility of a given compound represents the highest molarity solution that is possible for that compound. However, solubility can also be expressed as the moles per liter. Problem : Silver Chromate (Ag2CrO4, 331.73 g/mol) has a Ksp of 1.12 x 10 -12.a) Calculate the solubility (in g/L) of silver chromate in water.b) Calculate the solubility (in g/L) of silver chromate in 0.110 M AgNO 3 solution. Solubility is normally expressed in g/L of saturated solution. Solubility is the amount of reagent that will be consumed to saturate the solution or reach the equilibrium of the dissociation reaction. Recall that the definition of solubility is the maximum possible concentration of a solute in a solution at a given temperature and pressure. Problem : Silver Chromate, Ag2CrO4, has a Ksp of 9.0 x 10 -12. Solubility product constants are used to describe saturated solutions of ionic compounds of relatively low solubility. Saturated solution - Contains the maximum concentration of ions that can exist in equilibrium with the solid salt at a given temperature. Molar solubility is the number of moles of solute in one liter of saturated solution. Use information of the solubility of a compound to calculate the Ksp value. Solubility Product: The equilibrium existing between a soluble chemical compound and its solution is known as dynamic equilibrium. Introduction. The solution must be saturated in nature. So, The solubility product, Ksp expression for this compound is written as: Let's plug in the values in it: So, the solubility product(Ksp) of is . Ag2CrO4 = 2Ag + CrO4. What is the ionic concentrations of Ag+ and CrO4^-2 in a saturated solution of Ag2CrO4 at 25C? Ksp = [Ag]2 [CrO4] = 9 x 10-12 so (2x)2 (x) = 9 x 10-12. Example: The solubility of silver sulfate, Ag2SO4, is 0.025 M at 25oC. Ag2CrO4 = 332 g/mole x 1.31 x 10-4 moles = 4.35 g/liter Solutions . And 4x3 = 9 x 10-12 x = 1.31 x 10-4 Since x moles of Ag2CrO4 had to dissolve to give us 2x Ag ions and x CrO4 ions, then x moles of Ag2CrO4 dissolved. A saturated solution is in a state of dynamic equilibrium between the dissolved, dissociated, ionic compound and the undissolved solid. Which is the Ksp of Ag2CrO4? If the molar solubility of is s then is 2s and is s. (It's because there is 2:1 ration between ions) Silver ion concentration in saturated solution is given as . The equilibrium reaction for the dissociation of AgCl is: Solubility product equilibrium constant (K sp) - The product of the equilibrium concentrations of the ions in a saturated solution of a salt. Calculate its solubility product constant, Ksp. The key to solving solubility problems is to properly set up your dissociation reactions and define solubility. M x A y (s) - … For Ag2CrO4, the solubility equilibrium isThus, For AgBr, the solubility equilibrium is Let the solubility of AgBr be S mol L-1The ratio of molarities of their saturated solutions Since the solubility of Ag2CrO4 is more than that of AgBr, so the former is more soluble. A saturated solution of Ag2CrO4 has a silver-ion concentration of 1.3 * 10^-4M. Calculate its solubility product constant, Ksp. Solubility Product Constants, K sp. Chemistry Chemical Reactions Chemical Equations Ksp of Ag2CrO4 is 1.9x10^-12 mole^3/dm^9?