Textbook Question
Consider the titration of 50.0 mL of 1.00 M H3PO4 with 1.00 M KOH. Calculate the pH after the addition of each of the following volumes of base. (a) 25.0 mL
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Ch.17 - Applications of Aqueous Equilibria
Chapter 17, Problem 99
For each of the following compounds, write a balanced net ionic equation for the dissolution of the compound in water, and write the equilibrium-constant expression for Ksp. (d) Hg2Cl2
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Net Ionic Equations
A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions that do not participate in the reaction. In the context of dissolution, it shows the ions that form when a compound dissolves in water, highlighting the actual chemical change occurring in the solution.
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Net Ionic Equations
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It quantifies the extent to which a compound can dissolve in water, expressed as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation.
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Dissociation of Ionic Compounds
Dissociation refers to the process by which an ionic compound separates into its constituent ions when dissolved in water. For example, when mercurous chloride (Hg2Cl2) dissolves, it dissociates into mercury (I) ions and chloride ions, which is essential for writing the net ionic equation and determining the Ksp expression.
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Related Practice
Textbook Question
Consider the titration of 50.0 mL of 1.00 M H3PO4 with 1.00 M KOH. Calculate the pH after the addition of each of the following volumes of base. (d) 100.0 mL
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Textbook Question
The titration of 0.02500 L of a diprotic acid solution with 0.1000 M NaOH requires 34.72 mL of titrant to reach the second equivalence point. The pH is 3.95 at the first equiva-lence point and 9.27 at the second equivalence point. If the acid solution contained 0.2015 g of the acid, what is the molar mass, pKa1, and pKa2 of the acid?
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Textbook Question
A particular saturated solution of Ca3(PO4)2 has [Ca2+] = [PO43-] = 2.9 x 10^-7 M.
(c) What is [PO43-] in a saturated solution that has [Ca2+] = 0.010 M?
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Textbook Question
Use the following solubility data to calculate a value of Ksp for each compound. (a) SrF2: 1.03 x 10^-3 M
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Textbook Question
Use the following solubility data to calculate a value of Ksp for each compound. (d) Zn(CN)2; 4.95 x 10^-4 g/L
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