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Questions and Answers
What happens to the equilibrium constant when a reaction is reversed?
What happens to the equilibrium constant when a reaction is reversed?
In a precipitation reaction, what is the term used for the equilibrium constant that describes the solubility of a precipitate?
In a precipitation reaction, what is the term used for the equilibrium constant that describes the solubility of a precipitate?
When two reactions are added together, how is the equilibrium constant for the new reaction calculated?
When two reactions are added together, how is the equilibrium constant for the new reaction calculated?
Which type of reaction typically involves the formation of an insoluble precipitate?
Which type of reaction typically involves the formation of an insoluble precipitate?
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What is the correct formulation of the solubility product (Ksp) for a reaction where PbCl2(s) is in equilibrium with Pb2+ and Cl- ions?
What is the correct formulation of the solubility product (Ksp) for a reaction where PbCl2(s) is in equilibrium with Pb2+ and Cl- ions?
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If the concentration of a reactant in an equilibrium system is decreased, what effect does this have on the system according to Le Châtelier's Principle?
If the concentration of a reactant in an equilibrium system is decreased, what effect does this have on the system according to Le Châtelier's Principle?
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In the context of gas reactions at equilibrium, what effect does an increase in pressure have on the system?
In the context of gas reactions at equilibrium, what effect does an increase in pressure have on the system?
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What happens to the equilibrium when sodium acetate is added to a solution of acetic acid?
What happens to the equilibrium when sodium acetate is added to a solution of acetic acid?
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Under standard state conditions, how is the standard potential for a redox reaction calculated?
Under standard state conditions, how is the standard potential for a redox reaction calculated?
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Which statement regarding the equilibrium constant (Ka) for acetic acid is correct?
Which statement regarding the equilibrium constant (Ka) for acetic acid is correct?
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In Le Châtelier’s Principle, what effect does increasing the concentration of a reactant generally have on the equilibrium?
In Le Châtelier’s Principle, what effect does increasing the concentration of a reactant generally have on the equilibrium?
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When pressure is increased in a gaseous equilibrium involving more moles of gas on one side, what is the effect on the equilibrium?
When pressure is increased in a gaseous equilibrium involving more moles of gas on one side, what is the effect on the equilibrium?
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What is the implication of a more positive standard reduction potential in a redox reaction?
What is the implication of a more positive standard reduction potential in a redox reaction?
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If the equilibrium constant Ka for a weak acid is known, which of the following cannot be determined directly from it?
If the equilibrium constant Ka for a weak acid is known, which of the following cannot be determined directly from it?
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In a redox reaction where E°red is +0.3419 V for Cu2+ to Cu and E°ox is -0.7618 V for Zn2+ to Zn, what can be concluded about the reaction favorability?
In a redox reaction where E°red is +0.3419 V for Cu2+ to Cu and E°ox is -0.7618 V for Zn2+ to Zn, what can be concluded about the reaction favorability?
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How does the addition of Pb(NO3)2 affect the solubility of Pb(IO3)2?
How does the addition of Pb(NO3)2 affect the solubility of Pb(IO3)2?
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What principle explains why the solubility of Pb(IO3)2 decreases in the presence of Pb2+?
What principle explains why the solubility of Pb(IO3)2 decreases in the presence of Pb2+?
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What is the relationship between the solubility product (Ksp) and the molar solubility of Pb(IO3)2?
What is the relationship between the solubility product (Ksp) and the molar solubility of Pb(IO3)2?
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If the error in calculating concentrations due to approximation is 7.9 × 10–4%, is this error considered acceptable?
If the error in calculating concentrations due to approximation is 7.9 × 10–4%, is this error considered acceptable?
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What would happen to the equilibrium concentration of IO3- if the concentration of Pb2+ were to be significantly increased?
What would happen to the equilibrium concentration of IO3- if the concentration of Pb2+ were to be significantly increased?
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What happens to the solubility of an ionic compound in the presence of a gas that is part of its dissolution equilibrium?
What happens to the solubility of an ionic compound in the presence of a gas that is part of its dissolution equilibrium?
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Why is it important to consider the error introduced by approximations in solubility calculations?
Why is it important to consider the error introduced by approximations in solubility calculations?
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What best describes the common ion effect?
What best describes the common ion effect?
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Study Notes
Equilibrium Chemistry
- Students are expected to analyze reversible reactions, chemical equilibria, and thermodynamics.
- Students are expected to compute worded problems related to equilibrium chemistry.
- Students are expected to appreciate the importance of equilibrium chemistry.
Reversible Reactions and Chemical Equilibria
- In 1798, chemist Claude Berthollet accompanied Napoleon's military expedition to Egypt.
- Berthollet observed deposits of Na2CO3 at the Natron Lakes, which surprised him.
- This observation contributed to an important discovery about reversible chemical reactions.
- Chemical reactivity was once explained by the concept of "elective affinities".
- Berthollet's reasoning highlighted that reactions are reversible.
- Chemical reactions can move in both directions, determined by the relative amounts of reactants and products.
- The reversibility of a reaction is shown using a double arrow in an equation.
Thermodynamics and Equilibrium Chemistry
- Thermodynamics studies thermal, electrical, chemical, and mechanical forms of energy.
- The study of thermodynamics is important in chemistry.
- A reaction's free energy (∆G) is a function of its enthalpy (∆H), entropy (∆S), and temperature (T).
- The Gibb's free energy function (∆G = ∆H - T∆S) is used to determine if a reaction is thermodynamically favorable.
- A negative ∆G indicates a favorable reaction, while a positive ∆G indicates an unfavourable reaction.
Equilibrium Constants for Chemical Reactions
- Equilibrium constant (K) defines the reaction's equilibrium position.
- K is the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients.
- At equilibrium, the free energy (∆G) is zero.
- Thus, ∆G° = -RTlnK
Manipulating Equilibrium Constants
- Reversing a reaction reverses the equilibrium constant.
- Adding reactions multiplies their equilibrium constants.
Precipitation Reactions
- Precipitation reactions involve the formation of an insoluble precipitate from two soluble ions.
- The reaction is often a metathesis reaction.
- The equilibrium constant for precipitation reactions is the solubility product (Ksp).
Acid-base Reactions
- Acids donate protons, and bases accept protons.
- The most common strong acids are HCl, HI, HBr, HNO3, and HClO4, etc.
- The strongest acid in any given set is one that will readily donate its proton to the solvent or another molecule.
- Acids and bases can be strong or weak.
- Equilibrium constant expressions include concentrations of reactants and products in the reaction, each raised to their stoichiometric coefficients.
- Equilibrium constants are often called dissociation constants for the reactant-product reactions (Ka).
- The magnitude of Ka provides information about its relative strength.
Complexation Reactions
- In complexation reactions, metal ions act as electron acceptors, and a ligand acts as an electron donor.
- The equilibrium constant expresses the stability of the resulting metal-ligand complex, often called a formation constant (Kf).
- The reverse of a complexation reaction yields a dissociation constant (Kd).
- Kf and Kd are reciprocals of each other.
Redox Reactions
- Oxidation/Reduction Reactions involve electron transfer between reactants.
- A change in oxidation state indicates either oxidation or reduction.
- The species being oxidized is the reducing agent, and the species being reduced is the oxidizing agent.
- Equilibrium constants for redox reactions are often expressed as standard electrode potentials (E°).
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Description
Test your knowledge on reversible reactions, chemical equilibria, and thermodynamics in this Equilibrium Chemistry Quiz. Analyze different scenarios and compute worded problems to appreciate the significance of equilibrium in chemical reactions.
