Fundamentals of Analytical Chemistry¶
Skoog, D. A. (2014). Fundamentals of Analytical Chemistry.
Cited by¶
2 citations across 2 artifacts.
Each citation links to the sentence it supports in the citing article.
Domain-specific¶
- Precipitation
- The solubility product Ksp, a thermodynamic equilibrium constant for the dissolution-precipitation equilibrium of a sparingly soluble salt (e.g., BaSO₄ ⇌ Ba²⁺ + SO₄²⁻, Ksp = [Ba²⁺][SO₄²⁻] = 1.1 × 10⁻¹⁰ at 25°C)
This sourceSkoog and colleagues' analytical-chemistry text, which defines the solubility-product constant and works the barium sulfate dissolution equilibrium as its example. Skoog and colleagues' analytical-chemistry text, which covers gravimetric analysis and its precipitates.
Supported in partVerified against the work's full text
“OSH. One Ohm Heterogeneous equilibrium [Solubility] product, K,, [BaSO],(s) = Ba2* + SOZ- between a slightly”
- The solubility product Ksp, a thermodynamic equilibrium constant for the dissolution-precipitation equilibrium of a sparingly soluble salt (e.g., BaSO₄ ⇌ Ba²⁺ + SO₄²⁻, Ksp = [Ba²⁺][SO₄²⁻] = 1.1 × 10⁻¹⁰ at 25°C)
- Solubility
- The common-ion effect — addition of a soluble salt sharing an ion with the sparingly soluble compound depresses solubility further, as required by the Ksp equilibrium — is the inorganic-chemistry instance of Le Chatelier's principle applied to dissolution equilibria
This sourceSkoog's analytical-chemistry text presents the common-ion effect as a mass-action consequence of the solubility equilibrium, predicted from Le Chatelier's principle, and shows a common ion lowering the formal solubility of Ba(IO3)2. Skoog and colleagues' worked example of silver chloride dissolving through the AgCl(s)/AgCl(aq) and Ag+/Cl- equilibria.
SupportedVerified against the work's full text
“the presence of a small concentration of the [common ion] has lowered the formal solubility of Ba(lO3)2”
- The common-ion effect — addition of a soluble salt sharing an ion with the sparingly soluble compound depresses solubility further, as required by the Ksp equilibrium — is the inorganic-chemistry instance of Le Chatelier's principle applied to dissolution equilibria
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