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Ch.16 - Chemical Equilibrium
All textbooksTro 5th EditionCh.16 - Chemical EquilibriumProblem 49
Chapter 16, Problem 49

Silver sulfate dissolves in water according to the reaction: Ag2SO4(s) ⇌ 2 Ag+(aq) + SO42-(aq) Kc = 1.1⨉10-5 at 298 K. A 1.5-L solution contains 6.55 g of dissolved silver sulfate. If additional solid silver sulfate is added to the solution, will it dissolve?

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1
Calculate the molar mass of silver sulfate (Ag2SO4) using the atomic masses of Ag, S, and O.
Determine the number of moles of silver sulfate in the solution by dividing the mass of silver sulfate (6.55 g) by its molar mass.
Calculate the initial concentration of silver sulfate in the solution by dividing the number of moles by the volume of the solution (1.5 L).
Use the stoichiometry of the dissolution reaction to find the equilibrium concentrations of Ag+ and SO4^2- ions in terms of the initial concentration of Ag2SO4.
Compare the reaction quotient (Q) with the equilibrium constant (Kc) to determine if additional solid silver sulfate will dissolve. If Q < Kc, more solid will dissolve; if Q > Kc, it will not.

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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 quantifies the extent to which a compound can dissolve in water, represented by the concentrations of its ions at equilibrium. For silver sulfate, Ksp = 1.1 x 10^-5 indicates that at 298 K, the product of the concentrations of Ag+ and SO4^2- ions in a saturated solution is equal to this value.
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Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium. In the context of the silver sulfate dissolution, adding more solid Ag2SO4 increases the concentration of Ag+ and SO4^2- ions in the solution, which can shift the equilibrium position according to this principle, potentially affecting the solubility of the compound.
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Saturation and Supersaturation

A solution is considered saturated when it contains the maximum concentration of solute that can dissolve at a given temperature. If additional solute is added to a saturated solution, it will not dissolve unless the solution becomes supersaturated, which occurs under specific conditions. In this case, understanding whether the current concentration of ions exceeds the Ksp value is crucial to determine if more silver sulfate can dissolve.
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Related Practice
Textbook Question

Consider the reaction: NH4HS(s) ⇌ NH3(g) + H2S(g) At a certain temperature, Kc = 8.5⨉10-3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

Textbook Question

Consider the reaction and the associated equilibrium constant: aA(g) ⇌ bB(g) Kc = 4.0 Find the equilibrium concentrations of A and B for each value of a and b. Assume that the initial concentration of A in each case is 1.0 M and that no B is present at the beginning of the reaction. c. a=1;b=2

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Textbook Question

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g) ⇌ 2 NO2(g) If a reaction vessel initially contains an N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?

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