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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 90b,c
Capitolo 17, Problema 90b,c

Use the given molar solubilities in pure water to calculate Ksp for each compound. b. Ag2SO3; molar solubility = 1.55⨉10-5 M c. Pd(SCN)2; molar solubility = 2.22⨉10-8 M

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1
Identify the dissolution equation for Ag_2SO_3: Ag_2SO_3(s) \(\rightleftharpoons\) 2Ag^+(aq) + SO_3^{2-}(aq).
Determine the relationship between molar solubility and ion concentrations: If the molar solubility of Ag_2SO_3 is s, then [Ag^+] = 2s and [SO_3^{2-}] = s.
Substitute the given molar solubility into the expressions for ion concentrations: [Ag^+] = 2(1.55 \(\times\) 10^{-5}) M and [SO_3^{2-}] = 1.55 \(\times\) 10^{-5} M.
Write the expression for the solubility product constant, K_{sp}: K_{sp} = [Ag^+]^2[SO_3^{2-}].
Substitute the ion concentrations into the K_{sp} expression and simplify: K_{sp} = (2 \(\times\) 1.55 \(\times\) 10^{-5})^2 \(\times\) (1.55 \(\times\) 10^{-5}).

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Molar Solubility

Molar solubility is the number of moles of a solute that can dissolve in one liter of solution at a given temperature. It is a crucial measure in determining how much of a compound can be present in a saturated solution. In this context, the molar solubility of Ag₂SO₃ is given as 1.55×10⁻⁵ M, which indicates the maximum concentration of the compound that can dissolve in water.
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Molar Solubility Example

Solubility Product Constant (Ksp)

The solubility product constant, Ksp, is an equilibrium constant that applies to the solubility of 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 Ag₂SO₃, Ksp can be calculated using the molar solubility to find the concentrations of Ag⁺ and SO₃²⁻ 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 Ag₂SO₃, the dissociation can be represented as Ag₂SO₃(s) ⇌ 2Ag⁺(aq) + SO₃²⁻(aq). Understanding this dissociation is essential for calculating Ksp, as it allows us to relate the molar solubility to the concentrations of the ions produced in solution.
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Ionic Compounds Naming
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