Question

What is meant by a strong base? Are the strong bases also strong electrolytes? Explain.

Short answer

A strong base is a chemical compound that fully dissociates in a solution, releasing a high concentration of hydroxide ions (OH⁻) and rapidly increasing the solution's pH. Examples include sodium hydroxide (NaOH) and calcium hydroxide (Ca(OH)₂). Strong electrolytes are compounds that completely dissociate in a solution, producing a high concentration of charged ions, thereby increasing the solution's electrical conductivity. Since strong bases fully dissociate into ions in a solution, they act as strong electrolytes, efficiently conducting electricity.

Step-by-step solution

Definition of strong base

A strong base is a chemical compound that can fully dissociate, or ionize, in a solution and release a high concentration of hydroxide ions (OH⁻), causing a rapid increase in the solution's pH. This complete dissociation gives strong bases the ability to neutralize acids in a neutralization reaction effectively. Examples of strong bases are the alkali metal hydroxides, such as sodium hydroxide (NaOH), and the alkaline earth metal hydroxides, like calcium hydroxide (Ca(OH)₂).

Definition of strong electrolytes

Electrolytes are substances that, when dissolved in a solvent (usually water), disassociate into positively and negatively charged ions and can conduct electricity. A strong electrolyte is a compound that completely dissociates in a solution, producing a high concentration of charged ions that can move freely and increase the solution's electrical conductivity.

Relation between strong bases and strong electrolytes

Since strong bases are compounds that fully dissociate into their constituent ions when dissolved in water, they also fit the definition of strong electrolytes. By releasing their positive (e.g., Na⁺, Ca²⁺) and negative (OH⁻) ions into the solution, strong bases contribute to the solution's electrical conductivity, acting as strong electrolytes. In conclusion, strong bases are indeed strong electrolytes due to their complete dissociation into ions in a solution, making them efficient in conducting electricity.

Key concepts

Electrolytes

Imagine a charged particle that travels in a solution, helping it conduct electricity. That's essentially what an electrolyte is. When substances, such as salts or strong acids and bases, dissolve in water, they dissociate into ions and these ions make the solution capable of conducting electricity.

• Electrolytes in Solutions: In water, these dissolved substances break apart and produce positive and negative ions.
• Conductivity: If a solution can conduct electricity, it likely contains electrolytes.

Electrolytes are divided into strong and weak, based on how well they dissociate into ions. Strong electrolytes, like all strong bases, completely dissociate, ensuring plenty of ions to carry out electrical current.

Dissociation

Dissociation is like the process of untying a knot. In chemistry, when a compound dissolves in water and separates into its individual ions, it is dissociating.
Full Dissociation: This is what strong bases do. They dissociate completely in water. This means they release not just some, but all of their ions into the solution, making it highly alkaline.
Importance for Conductivity: More ions mean more conductivity. Full dissociation is why strong bases also act as strong electrolytes. By dissociating fully, they ensure the solution is filled with ions that help conduct electricity.

Neutralization Reaction

Neutralization is the chemical process where an acid and a base react to form water and a salt. This reaction helps balance out extremes in acidity or alkalinity.

• Acid-Base Reaction: When a strong base meets an acid, they undergo a neutralization reaction, neutralizing each other's properties.
• Equation: The general equation for this reaction is:
  \[ ext{Acid} + ext{Base} ightarrow ext{Water} + ext{Salt} \]

During this reaction, the hydroxide ions ( ext{OH}⁻ from the base) and hydrogen ions ( ext{H}⁺ from the acid) combine to form water, effectively neutralizing the acid and base effects.

Hydroxide Ions

Hydroxide ions are like tiny bouncers that can drastically change a solution's environment. They are negatively charged ions, denoted as \( ext{OH}^- \), that increase the alkalinity of a solution.

• Role in Solutions: By adding hydroxide ions to a solution, bases can push pH levels up, making the solution more basic or alkaline.
• Result of Dissociation: In strong bases, their hallmark is their ability to thoroughly dissociate and release hydroxide ions, thereby raising the pH level significantly.

These ions are central to many reactions, especially neutralization, where they pair up with hydrogen ions to form water, mitigating acidity.