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Questions and Answers
What type of materials are soluble in water but do not dissociate?
According to the Arrhenius theory, which is considered a base?
Which species have both acidic and basic properties?
In the Brønsted-Lowry theory, what is formed when an acid loses a proton?
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What type of electrolytes ionize almost completely when dissolved in water?
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Which of the following is an example of a non-electrolyte?
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According to the Lewis theory, which is considered an acid?
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What role does a base play in the Lewis theory?
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What is autoprotolysis in the context of solvents?
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Which of the following can be considered as an example of acid-base behavior?
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What does Kw represent in the context of aqueous solutions?
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What is the value of Kw at room temperature?
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Why can the concentration of water be considered constant in dilute aqueous solutions?
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Which statement correctly describes chemical equilibrium?
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What relationship can be discovered by taking the negative logarithm of Kw equation?
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Study Notes
Solubility and Dissociation
- Soluble materials that do not dissociate in water include sugar and alcohols that dissolve without breaking into ions.
- Non-dissociating solutes retain their molecular structure when in solution.
Arrhenius Theory
- According to the Arrhenius theory, bases are substances that yield hydroxide ions (OH⁻) when dissolved in water.
Amphovert Properties
- Amphoteric species can behave as either acids or bases, depending on the circumstances; examples include water (H₂O) and bicarbonate (HCO₃⁻).
Brønsted-Lowry Theory
- In the Brønsted-Lowry framework, an acid, upon losing a proton (H⁺), forms a conjugate base.
Electrolytes
- Strong electrolytes are substances that ionize almost completely in solution, such as sodium chloride (NaCl) and hydrochloric acid (HCl).
Non-Electrolytes
- Non-electrolytes are substances that do not conduct electricity when dissolved, with examples like glucose and ethanol.
Lewis Theory
- In the Lewis acid-base theory, acids are defined as electron pair acceptors, while bases are electron pair donors.
Autoprotolysis
- Autoprotolysis refers to the self-ionization of solvents, such as water, where two molecules interact to form hydronium (H₃O⁺) and hydroxide (OH⁻) ions.
Acid-Base Behavior
- Acid-base behavior can be exemplified by the reaction between an acid and a base, resulting in the formation of water and a salt.
Ion Product of Water
- Kw represents the ion product of water at a specific temperature, symbolizing the equilibrium constant for the autoprotolysis of water.
Value of Kw
- At room temperature (25°C), the value of Kw is 1.0 × 10⁻¹⁴.
Concentration of Water
- The concentration of water in dilute aqueous solutions remains effectively constant due to its high concentration relative to solutes.
Chemical Equilibrium
- Chemical equilibrium is a state where the concentrations of reactants and products remain constant over time, indicating a balance in chemical reactions.
Logarithmic Relationship
- Taking the negative logarithm of the Kw equation reveals the relationship to pH, illustrating how concentration of H⁺ and OH⁻ ions affect acidity and basicity.
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Description
Learn about the chemical composition of aqueous solutions and the classification of electrolytes. Understand the difference between strong electrolytes, weak electrolytes, and non-electrolytes. Explore how water serves as a versatile solvent in chemical analyses.
