Textbook Question
(a) I f t he molar solubility of CaF2 at 35°C i s 1.24 × 10–3 mol/L, what is Ksp at this temperature?
Ch.17 - Additional Aspects of Aqueous Equilibria
Chapter 17, Problem 54b
(b) If 0.0490 g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant.
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Identify the dissolution equation for silver iodate (AgIO3). When AgIO3 dissolves, it dissociates into silver ions (Ag+) and iodate ions (IO3-). The equation can be written as: \( AgIO3(s) \rightarrow Ag^+(aq) + IO3^-(aq) \).
Determine the molar mass of AgIO3 to convert grams per liter to moles per liter. The molar mass of AgIO3 is calculated by adding the atomic masses of silver (Ag), iodine (I), and three oxygen (O) atoms.
Convert the mass of AgIO3 given (0.0490 g) into moles using the molar mass calculated in the previous step. This will give you the concentration of AgIO3 in moles per liter, which is also the concentration of Ag+ and IO3- since each formula unit of AgIO3 produces one ion of each.
Write the expression for the solubility product constant (Ksp) of AgIO3. The Ksp expression for AgIO3 is given by: \( K_{sp} = [Ag^+][IO3^-] \), where [Ag+] and [IO3-] are the molar concentrations of the respective ions in a saturated solution.
Substitute the concentrations of Ag+ and IO3- obtained from the dissolution of AgIO3 into the Ksp expression to calculate the solubility-product constant.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced equation. For a compound like AgIO3, Ksp can be calculated from the concentrations of Ag+ and IO3- ions in a saturated solution.
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Solubility Product Constant
Dissociation of Ionic Compounds
When ionic compounds dissolve in water, they dissociate into their constituent ions. For AgIO3, it dissociates into Ag+ and IO3- ions. Understanding this dissociation is crucial for calculating Ksp, as the concentrations of these ions directly influence the solubility product constant.
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Molar Mass and Concentration Calculations
To calculate Ksp, it is essential to determine the molar mass of the compound and the concentration of ions in solution. The molar mass of AgIO3 is needed to convert the given mass (0.0490 g) into moles, which can then be used to find the molarity of the solution. This concentration is vital for accurately calculating the Ksp value.
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Related Practice
Textbook Question
(b) It is found that 1.1 × 10-2 g SrF2 dissolves per 100 mL of aqueous solution at 25°C. Calculate the solubility product for SrF2.
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A 1.00-L solution saturated at 25 C with calcium oxalate 1CaC2O42 contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 C.
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A 1.00-L solution saturated at 25 C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25 C.