Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: The Ksp of AgCl at 25 °C is 1.6 x 10-10. Consider a solution that is 1.0 x 10-2 M CaCl2 and 1.0 x 10-8 M AgNO3.

Problem

The Ksp of AgCl at 25 °C is 1.6 x 10-10. Consider a solution that is 1.0 x 10-2 M CaCl2 and 1.0 x 10-8 M AgNO3.

Solution

We’re being asked to determine if a precipitate will form when 1.0 x 10-2 M CaCl2 and 1.0 x 10-8 M AgNO3. are mixed.


For this, we need to compare the reaction quotient (Q) vs. the solubility product constant (Ksp)

Recall that when:

• Q > Ksp: the solution is supersaturated and a precipitate will form. Reactants are favored.

• Q = Ksp: the solution is at equilibrium and no precipitate will form.

• Q < Ksp: the solution is unsaturated and no precipitate will form. Products are favored.


The expected precipitate is AgCl. The chloride ion, Cl, has a charge of –1. Ag then has a charge of +1. 

The dissociation of AgCl in water is as follows:

AgCl(s)  Ag+(aq) + Cl(aq)


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