Podcast
Questions and Answers
Which statement best defines a strong acid?
Which statement best defines a strong acid?
- A strong acid can only be an Arrhenius acid.
- A strong acid ionizes partially in water.
- A strong acid does not produce H+ ions in water.
- A strong acid ionizes completely in water. (correct)
According to the Brønsted-Lowry concept, what role does a base play in a proton-transfer reaction?
According to the Brønsted-Lowry concept, what role does a base play in a proton-transfer reaction?
- It donates a proton.
- It produces hydroxide ions.
- It accepts a proton. (correct)
- It acts as a buffer solution.
What characterizes a heterogeneous reaction?
What characterizes a heterogeneous reaction?
- At least two different phases are involved. (correct)
- Reactants and products are in the same physical state.
- It proceeds in both forward and reverse directions.
- It does not reach an equilibrium state.
Which of the following pairs represents a weak acid and a weak base?
Which of the following pairs represents a weak acid and a weak base?
What theory describes acids as electron pair acceptors and bases as electron pair donors?
What theory describes acids as electron pair acceptors and bases as electron pair donors?
What is the primary limitation of the Arrhenius concept of acids and bases?
What is the primary limitation of the Arrhenius concept of acids and bases?
Which of the following reactions is classified as an acid-base reaction?
Which of the following reactions is classified as an acid-base reaction?
What is the ionization constant a measure of?
What is the ionization constant a measure of?
What is the expression for the ionization constant of acetic acid (Ka)?
What is the expression for the ionization constant of acetic acid (Ka)?
In the self-ionization of water, what ions are produced?
In the self-ionization of water, what ions are produced?
Which statement correctly describes the equilibrium constant (Kw) for water?
Which statement correctly describes the equilibrium constant (Kw) for water?
According to Le Chatelier’s principle, what occurs when pressure is increased in a reaction with more gaseous products than reactants?
According to Le Chatelier’s principle, what occurs when pressure is increased in a reaction with more gaseous products than reactants?
What is the effect of increasing the temperature on an endothermic reaction?
What is the effect of increasing the temperature on an endothermic reaction?
If more O2 is added to the equilibrium reaction 2 SO3(g) ⇌ 2 SO2(g) + O2(g), what will be the effect?
If more O2 is added to the equilibrium reaction 2 SO3(g) ⇌ 2 SO2(g) + O2(g), what will be the effect?
What happens when O2 is removed from the system in the equilibrium 2 SO3(g) ⇌ 2 SO2(g) + O2(g)?
What happens when O2 is removed from the system in the equilibrium 2 SO3(g) ⇌ 2 SO2(g) + O2(g)?
What is the equilibrium constant expression for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g)?
What is the equilibrium constant expression for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g)?
Flashcards
Acid-Base Reaction
Acid-Base Reaction
A chemical reaction between an acid and a base, producing a salt and water.
Arrhenius Acid
Arrhenius Acid
A compound that releases H+ ions in water.
Brønsted-Lowry Acid
Brønsted-Lowry Acid
A molecule or ion capable of donating a proton (H+).
Strong Acid
Strong Acid
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Equilibrium Constant
Equilibrium Constant
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Homogeneous Reaction
Homogeneous Reaction
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Weak Acid
Weak Acid
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Reversible Reaction
Reversible Reaction
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Ka
Ka
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Kb
Kb
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Kw
Kw
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Acidic Solution
Acidic Solution
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Neutral Solution
Neutral Solution
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Basic Solution
Basic Solution
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Equilibrium Constant (Kc)
Equilibrium Constant (Kc)
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Le Chatelier's Principle
Le Chatelier's Principle
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Study Notes
Chemical Equilibrium
- Chemical equilibrium is a state where the forward and reverse reactions occur at the same rate.
- The concentrations of reactants and products remain constant.
- A reversible reaction involves the simultaneous conversion of reactants to products and products to reactants.
- An irreversible reaction proceeds in one direction only.
Types of Chemical Reactions in Aqueous Solutions
- Acid-base reactions: acid + base → salt + water
- Example: HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
- Oxidation-reduction reactions (Redox reactions): involve electron transfer
- Precipitation reactions: result in the formation of a solid precipitate
Acids and Bases
-
Arrhenius concept:
- An acid releases H⁺ ions in water.
- A base releases OH⁻ ions in water.
- Example: HCl(aq) → H⁺(aq) + Cl⁻(aq)
- Example: NaOH(aq) → Na⁺(aq) + OH⁻(aq)
- Limitation: Some bases do not contain OH⁻.
-
Brønsted-Lowry concept:
- An acid is a proton (H⁺) donor.
- A base is a proton acceptor.
-
Lewis concept:
- An acid is an electron pair acceptor.
- A base is an electron pair donor.
Strength of Acids and Bases
- Strong acids and bases ionize completely in water.
- Examples of strong acids: HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄
- Examples of strong bases: LiOH, NaOH, KOH, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂
Equilibrium Constant Law
- Equilibrium constant (Kc) is a measure of the ratio of products to reactants at equilibrium.
- A homogeneous reaction involves all reactants and products in the same phase.
- A heterogeneous reaction involves reactants and products in at least two different phases.
Weak Acids and Bases
- Weak acids and bases ionize to a limited extent in water.
- Examples: CH₃COOH, NH₃
- Acid or base ionization constant (Ka or Kb) measures the strength of the acid or base.
- The ionization constant is given by the equilibrium expression.
Self-Ionization of Water
- Water can act as both an acid and a base (self-ionization).
- Water dissociates into H₃O⁺ and OH⁻ ions.
- The equilibrium constant for the self-ionization of water is Kw.
- Kw = [H₃O⁺][OH⁻]
Equilibrium Constant Equation
- Example: 2 SO₂(g) + O₂(g) ↔ 2 SO₃(g)
- Kc = [SO₃]² / [SO₂]²[O₂]
Le Chatelier's Principle
- A change in conditions of a system at equilibrium shifts the equilibrium to counteract the change.
- Change in concentration of a reactant or product
- Change in temperature
- Change in pressure (for gaseous reactions)
Predict the effect of the changes
- Increasing the temperature: shifts the equilibrium towards the products in endothermic reactions.
- Increasing the pressure: shifts the equilibrium towards the side with fewer moles of gas.
- Adding more O₂: shifts the equilibrium towards the reactants.
- Removing O₂: shifts the equilibrium towards the products.
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