The concept used in this problem is based on the solubility product.
Solubility product comes into action when the sparingly soluble (not totally dissolved) ionic compound dissociates into its constituent ions in water.
Solubility product:
The solubility product helps to determine the solubility of the compound in water.
Higher the value of solubility product, higher will be the solubility of that compound in water.
Example-
The expression for the solubility product will be shown below.
…… (1)
Here, is the concentration of andis the Concentration of , a and b are the coefficients of the respective ion.
The reaction of silver sulfate in water is shown below.
Let the value of solubility of silver sulfate be
Similar to the solubility product expressed in equation (1), the expression for solubility product for silver sulfate will be shown below.
Substitute as the value of and as the value of and as the value of .
Conversion of the unit of solubility from mol per liter to gram per liter is as shown below.
…… (2)
Substitute as the value of and as the value of the molar mass of silver nitrate (M) in equation (2)
Ans:The solubility of silver sulfate in gram per liter is.
The value of Ksp for silver sulfate, Ag2SO4, is 1.20x10-5 . Calculate the solubility of Ag2SO4 in grams per liter. Exp...
The solubility of silver sulfate (Ag2SO4), in moles per liter, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?
Calculate the molar solubility of Ag2SO4 in each solution below. The Ksp of silver sulfate is 1.5x10-5 a) 0.19 M AgNO3 b) 0.19 M Na2SO4
Silver sulfate has Ksp = 9.0 × 10−5. What mass (g) of Ag2SO4 will dissolve per liter of water? Enter your answer to 1 decimal place.
Ch19-22. Calculate the molar solubility of Ag2SO4 in each solution below. The Ksp of silver sulfate is 1.5x10^-5. a) 0.17 M AgNO3: ________ b) 0.17 M Na2SO4: ________
Calculate the solubility (g/L) of calcium sulfate, CaSO4 in units of grams per liter. Ksp(CaSO4) = 2.4E-5
Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution: CaF2(s)⇌Ca2+(aq)+2F−(aq) At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystallization. The equilibrium constant for the dissolution reaction is Ksp=[Ca2+][F−]2 Ksp is called the solubility product and can be determined experimentally by measuring thesolubility, which is the amount...
What is the minimum concentration of sulfate ion, SO4 2- that must be present in a 0.050 M solution of Ca2+ to cause a precipitate to form? The K sp for calcium sulfate, CaSO4, is 7.10 × 10-5. The value of Ksp for silver sulfate, Ag2SO4, is 1.20×10−5. Calculate the solubility of Ag2SO4 in grams per litre. Express your answer numerically in grams per litre. A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water....
Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) = 1.1x10-10 solubility = AL The equilibrium concentration of chloride ion in a saturated lead chloride solution is M. In the presence of excess OH, the Ar+ (aq) ion forms a hydroxide complex ion. Al(OH)4 Calculate the concentration of free Ap+ ion when 1.56x10-mol Al(CH2C00)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For Al(OH)4, Ke=...
please show work 4) (24 points) What is the solubility of Ag2SO4 (silver sulfate) in... a) ...pure water? b) ...1.5 M AgNO3?
a) Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its molar solubility. b) If Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its mass solubility in g solute/100g of water. Please answer a & b