Open Question
If the sodium concentration in blood plasma is 0.140 M, and Ksp for sodium urate is 5.76 * 10^-8, what minimum concentration of urate would result in precipitation?
Ch.17 - Aqueous Ionic Equilibrium
Chapter 17, Problem 129
Calculate the solubility of CuX in a solution that is 0.150 M in NaCN. Ksp for CuX is 1.27⨉10-36.
Verified step by step guidance1
Identify the relevant chemical equilibrium: CuX(s) ⇌ Cu⁺(aq) + X⁻(aq).
Write the expression for the solubility product constant (Ksp): Ksp = [Cu⁺][X⁻].
Recognize that NaCN provides CN⁻ ions, which can complex with Cu⁺ to form Cu(CN)₂⁻, affecting the solubility of CuX.
Write the equilibrium expression for the complexation reaction: Cu⁺ + 2CN⁻ ⇌ Cu(CN)₂⁻, and note that this will reduce the concentration of free Cu⁺ ions.
Use the Ksp expression and the complexation equilibrium to set up equations that relate the solubility of CuX to the concentration of CN⁻, and solve for the solubility of CuX.
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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 CuX, Ksp helps determine how much of the compound can dissolve in a solution before reaching saturation.
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Solubility Product Constant
Common Ion Effect
The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. In this case, the presence of NaCN introduces CN⁻ ions, which shifts the equilibrium of the dissolution of CuX, reducing its solubility. Understanding this effect is crucial for calculating the new solubility in the presence of a common ion.
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ICE Table (Initial, Change, Equilibrium)
An ICE table is a tool used to track the concentrations of reactants and products during a chemical reaction at different stages: Initial, Change, and Equilibrium. For solubility calculations, it helps organize the initial concentrations of ions, the changes that occur as the system reaches equilibrium, and the final concentrations. This systematic approach is essential for accurately determining the solubility of CuX in the given solution.
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Related Practice
Textbook Question
Pseudogout, a condition with symptoms similar to those of gout (see Problem 126), is caused by the formation of calcium diphosphate (Ca2P2O7) crystals within tendons, cartilage, and ligaments. Calcium diphosphate will precipitate out of blood plasma when diphosphate levels become abnormally high. If the calcium concentration in blood plasma is 9.2 mg/dL, and Ksp for calcium diphosphate is 8.64⨉10-13, what minimum concentration of diphosphate results in precipitation?
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Textbook Question
Calculate the solubility of silver chloride in a solution that is 0.100 M in NH3.
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Open Question
The Kb of hydroxylamine, NH2OH, is 1.10 * 10^-8. A buffer solution is prepared by mixing 100.0 mL of a 0.36 M hydroxylamine solution with 50.0 mL of a 0.26 M HCl solution. Determine the pH of the resulting solution.
Textbook Question
A 0.867-g sample of an unknown acid requires 32.2 mL of a 0.182 M barium hydroxide solution for neutralization. Assuming the acid is diprotic, calculate the molar mass of the acid.
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Textbook Question
A 25.0-mL volume of a sodium hydroxide solution requires 19.6 mL of a 0.189 M hydrochloric acid for neutralization. A 10.0-mL volume of a phosphoric acid solution requires 34.9 mL of the sodium hydroxide solution for complete neutralization. Calculate the concentration of the phosphoric acid solution.
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