Questions and Answers
What are the two main types of substances?
What is an example of a non-electrolyte?
Sugar solution
Which of the following is a strong electrolyte?
What does the term 'ionization constant' (K) refer to?
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Electrolytes do not conduct electricity in molten state.
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The degree of ionization is denoted by ______.
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What does the Ostwald Dilution Law relate to?
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What is an example of a weak electrolyte?
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Ions obey Ohm's law.
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The process of ionization is ______ for weak electrolytes.
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Study Notes
Types of Substances
- Substances classified as non-electrolytes do not conduct electricity in molten states or aqueous solutions; examples include sugar, urea, glucose, and glycerine.
- Electrolytes conduct electricity in molten states or aqueous solutions; an example is NaCl.
- In solid form, electrolytes are poor conductors of electricity but become good conductors when molten or dissolved.
Types of Electrolytes
- Strong Electrolytes: Completely ionize in water, allowing high electrical conduction. Examples include strong acids (HCl, H₂SO₄, HNO₃) and strong bases (KOH, NaOH).
- Weak Electrolytes: Partially ionize in water, resulting in lower electrical conduction. Examples include weak acids (HCN, CH₃COOH, H₃PO₄, H₂CO₃) and weak bases (NH₄OH).
Arrhenius Theory
- Also known as the dissociation or ionic theory, it posits that electrolytes ionize in solvents.
- The ionization process is reversible, with the ionization constant (K) represented by the formula:
- K = [A⁺][B⁻] / [AB]
- The discharge of ions during electrolysis occurs in equivalent amounts, independent of their relative speeds.
Properties and Evidence of Ionic Theory
- Ions affect physical properties like freezing point depression, boiling point elevation, osmotic pressure, and vapor pressure.
- X-ray diffraction can confirm the presence of ions in solid electrolytes.
- Ions conform to Ohm’s law, where I (current) = E (voltage) / R (resistance).
- Ionic reactions can be observed, as shown in the reaction: AgNO₃ + NaCl → Ag + Cl⁻ + Na + NO₃⁻.
- The color of solutions, such as CuSO₄ appearing blue, is due to the presence of specific ions like Cu²⁺.
Degree of Ionization
- Represented by α, it defines how well an electrolyte ionizes in a solvent.
- α = Number of molecules dissociated / Total number of molecules.
- Degree of ionization depends on:
- Nature of solute and solvent; weak electrolytes have lower α than strong electrolytes.
- Dielectric constant of the solvent, which is directly proportional to ionization.
- Dilution; weak electrolyte degree of dissociation increases with dilution, reaching maximum at infinite dilution (α = 1).
- Concentration and temperature also affect α.
Ostwald Dilution Law
- This law describes the mass action principle for dilute solutions and weak electrolytes, relating to their dissociation behavior.
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Description
Test your knowledge on ionic equilibrium and the classification of substances. This quiz covers the key differences between non-electrolytes and electrolytes, along with their behavior in different states. Dive into the concepts of conductivity and the types of ionic compounds in this engaging quiz.
