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11.2 Electrolytes

2 min read•june 25, 2024

are substances that conduct electricity when dissolved in water. They dissociate into ions, with fully breaking apart and weak ones only partially. This process is crucial for understanding how chemicals behave in solution.

The strength of an electrolyte depends on its interactions with water molecules. Ionic compounds split into separate ions, while react with water. These processes are key to grasping how different substances dissolve and conduct electricity in aqueous solutions.

Electrolytes

Concept and examples of electrolytes

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  • Electrolytes dissociate into ions when dissolved in water, allowing the solution to conduct electricity ()
    • Strong electrolytes completely dissociate into ions (, , )
    • only partially dissociate into ions (, )
  • do not dissociate into ions and do not conduct electricity when dissolved (, )

Dissolution of ionic vs covalent electrolytes

  • (salts) dissociate into separate cations and anions when dissolved in water driven by the strong attraction between ions and water molecules
    • NaCl(s)→Na+(aq)+Cl−(aq)NaCl(s) \rightarrow Na^+(aq) + Cl^-(aq)
  • Covalent electrolytes (acids and bases) undergo a reaction with water to form ions
    • Strong acids and bases completely react with water to form ions
      • HCl(g)+H2O(l)→H3O+(aq)+Cl−(aq)HCl(g) + H2O(l) \rightarrow H3O^+(aq) + Cl^-(aq)
    • Weak acids and bases only partially react with water to form ions and undissociated molecules
      • CH3COOH(l)+H2O(l)⇌CH3COO−(aq)+H3O+(aq)CH3COOH(l) + H2O(l) \rightleftharpoons CH3COO^-(aq) + H3O^+(aq)

Solute-solvent interactions in electrolyte strength

  • Electrolyte strength depends on the extent of its or ionization in water
  • , such as , determine electrolyte strength
    • Strong ion-dipole interactions between ions and water molecules lead to complete and behavior
      • Ions with high (small size and high charge) interact strongly with water and are strong electrolytes
    • Weak ion-dipole interactions result in partial dissociation and behavior
      • Ions with low charge density (large size and low charge) interact weakly with water and are weak electrolytes
  • affects electrolyte strength
    • Polar solvents (water) promote dissociation and ionization due to their ability to solvate ions
    • Non-polar solvents (hexane) do not effectively solvate ions, leading to minimal dissociation and weak electrolyte behavior

Processes in electrolyte solutions

  • Dissociation: The process by which ionic compounds separate into individual ions in solution
  • : The surrounding of dissolved ions by solvent molecules, stabilizing them in solution
  • Ionization: The process by which neutral molecules form ions in solution, often through reaction with the solvent
  • : The specific form of where water molecules surround and interact with dissolved ions

Key Terms to Review (33)

Acid ionization: Acid ionization is the process by which an acid releases protons ($H^+$) into solution, forming its conjugate base. This process is quantified by the acid dissociation constant, $K_a$.
C12H22O11: C12H22O11 is the molecular formula for sucrose, a common disaccharide found in many foods. Sucrose is an important carbohydrate that serves as a primary source of energy for the body and plays a key role in various electrolyte-related processes.
C2H5OH: C2H5OH, also known as ethanol, is a simple organic compound composed of two carbon atoms, five hydrogen atoms, and one oxygen atom. It is a colorless, volatile, and flammable liquid that is widely used as a solvent, fuel, and in the production of various chemicals.
CH3COO-: CH3COO- is the acetate ion, which is the conjugate base of acetic acid. It plays a significant role in various chemical reactions, particularly as an electrolyte in solution and in the hydrolysis of salts formed from weak acids and strong bases. Understanding acetate’s behavior helps explain its interactions in biochemical processes and its applications in various fields.
CH3COOH: CH3COOH, also known as acetic acid, is a weak organic acid that plays a crucial role in the context of electrolytes and the hydrolysis of salts. It is a common compound found in various chemical and biological processes.
Charge Density: Charge density is a measure of the amount of electric charge per unit volume or unit area of a material or system. It is an important concept in the study of electrolytes, as it describes the distribution and concentration of charged particles within a solution or medium.
Cl-: Cl- is the chemical symbol for the chloride ion, which is a negatively charged ion consisting of a chlorine atom that has gained an extra electron. This ion is an important component in various chemical processes and contexts, including writing and balancing chemical equations, ionic bonding, electrolytes, and precipitation and dissolution.
Conductivity: Conductivity is a measure of a material's ability to allow the flow of electric charge or the movement of ions through it. It is a fundamental property that is closely related to the concept of electrical resistance and is an important consideration in various fields, including chemistry, physics, and engineering.
Covalent Electrolytes: Covalent electrolytes are substances that can conduct electricity when dissolved in water or melted, but consist of molecules held together by covalent bonds rather than ionic bonds. These compounds typically do not dissociate into ions but may still allow for the movement of charged particles in a solution, contributing to their electrical conductivity under certain conditions. Understanding covalent electrolytes helps in grasping how different substances behave in solution and their role in various chemical processes.
Dissociation: Dissociation is the process by which an ionic compound separates into its individual ions when dissolved in a solvent, typically water. This process is crucial for understanding how electrolytes conduct electricity in solution.
Dissociation: Dissociation is the process by which an ionic compound separates into its individual ions when dissolved in a solvent, usually water. This phenomenon is crucial for understanding how electrolytes function, as it allows for the conduction of electricity through the solution. Dissociation is key to the behavior of acids, bases, and salts in solution, influencing their chemical reactions and interactions with other substances.
Electrolytes: Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They play crucial roles in various biological and chemical processes, including maintaining fluid balance, transmitting nerve impulses, and regulating muscle function. Understanding electrolytes is essential for grasping concepts related to solutions and conductivity in chemistry.
H3O+: H3O+ is the hydronium ion, a positively charged species formed when a proton (H+) interacts with a water molecule (H2O). It is a crucial concept in understanding the behavior of acids, bases, and the pH of aqueous solutions.
HCl: HCl, or hydrogen chloride, is a chemical compound consisting of one hydrogen atom and one chlorine atom. It is a colorless, corrosive gas that has a wide range of applications and plays a crucial role in various chemical processes and reactions.
Hydration: Hydration refers to the process of adding water or other liquid to a substance, resulting in the formation of a hydrated compound or solution. This term is particularly relevant in the context of dissolution, electrolytes, and hydrocarbon chemistry.
Ion-dipole attraction: Ion-dipole attraction is the electrostatic force between an ion and a polar molecule. It is a key interaction in dissolving ionic compounds in polar solvents.
Ion-Dipole Interactions: Ion-dipole interactions are attractive forces that occur between an ion (a charged particle) and a polar molecule (a molecule with an unequal distribution of electrons). These interactions are important in various chemical and biological processes, including the solubility of ionic compounds and the functioning of biological membranes.
Ionic Electrolytes: Ionic electrolytes are charged particles that can conduct electricity when dissolved in water or another solvent. They are formed when ionic compounds, such as salts, dissociate into positively and negatively charged ions, which are able to move freely and carry an electric current.
Ionization: Ionization is the process by which an atom or molecule loses or gains one or more electrons, resulting in the formation of ions. This fundamental chemical process is crucial in understanding the Bohr model, the strengths of ionic and covalent bonds, and the behavior of electrolytes.
Na+: Na+ is the chemical symbol for the sodium ion, a positively charged particle that plays a crucial role in various chemical processes and biological functions. This term is particularly important in the context of writing and balancing chemical equations, ionic bonding, and the behavior of electrolytes.
NaCl: NaCl, commonly known as sodium chloride, is a chemical compound that consists of one sodium atom (Na) and one chlorine atom (Cl) bonded together. It is an ionic compound that is essential for various biological and industrial processes, and it is the primary component of table salt.
NaOH: NaOH, or sodium hydroxide, is a strong base that plays a crucial role in various chemical processes, including electrolytes, buffers, and the occurrence, preparation, and compounds of oxygen. It is a highly reactive and corrosive chemical with a wide range of applications in industry, science, and everyday life.
NH3: NH3, also known as ammonia, is a colorless, pungent-smelling gas that is composed of one nitrogen atom and three hydrogen atoms. This simple inorganic compound is an important chemical in various contexts, including molecular structure, acid-base chemistry, and the nitrogen cycle.
Non-Electrolytes: Non-electrolytes are substances that do not dissociate into ions when dissolved in water or other solvents. They are molecules that do not conduct electricity in aqueous solutions, in contrast to electrolytes which do dissociate into charged particles.
Nonelectrolytes: Nonelectrolytes are substances that, when dissolved in water, do not dissociate into ions and therefore do not conduct electricity. Typically, these are covalent compounds such as sugars and alcohols.
Solute-Solvent Interactions: Solute-solvent interactions refer to the attractive and repulsive forces that exist between a dissolved substance (solute) and the surrounding liquid medium (solvent). These interactions determine the solubility and behavior of the solute in the solvent, which is a crucial concept in the study of electrolytes.
Solvation: Solvation is the process of surrounding solute particles with solvent molecules to form a solution. It involves interactions between the solute and solvent molecules.
Solvation: Solvation is the process by which solute particles or ions become surrounded by solvent molecules, forming a solvated species. This interaction between the solute and solvent is a critical aspect of the dissolution process, the behavior of electrolytes, and the solubility of substances.
Solvent Polarity: Solvent polarity refers to the degree of polarity or charge distribution within a solvent molecule, which determines its ability to dissolve and interact with other polar or non-polar substances. The polarity of a solvent is a crucial factor in determining the solubility and behavior of solutes in chemical reactions and processes.
Strong electrolyte: A strong electrolyte is a substance that completely dissociates into ions when dissolved in water, resulting in high electrical conductivity. Examples include most salts, strong acids, and strong bases.
Strong Electrolytes: Strong electrolytes are substances that completely dissociate into ions when dissolved in water, producing a high concentration of free-moving charged particles. These substances readily conduct electricity due to the high mobility of their ions.
Weak electrolyte: A weak electrolyte is a substance that partially dissociates into ions when dissolved in water, resulting in a solution that conducts electricity poorly. Common examples include weak acids and weak bases.
Weak Electrolytes: Weak electrolytes are substances that partially dissociate into ions when dissolved in water or other solvents. Unlike strong electrolytes, which completely dissociate, weak electrolytes maintain a balance between their molecular and ionic forms in solution.
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11.3 Solubility