acid and bases

Brønsted-Lowry Theory

A theory that extends the Arrhenius definition of acids and bases by defining acids as proton donors and bases as proton acceptors.

Brønsted-Lowry Acid

A species that donates a proton (hydrogen ion) in a chemical reaction.

Brønsted-Lowry Base

A species that accepts a proton (hydrogen ion) in a chemical reaction.

Arrhenius Theory

A theory of acids and bases focused on the behavior of hydrogen ions in aqueous solutions.

Ammonia Reaction with HCl

In this reaction, hydrogen chloride donates a proton to ammonia, making ammonia a Brønsted-Lowry base.

Conjugate Acid-Base Pair

A pair of species that transform into each other by the gain or loss of a proton.

Amphoteric Substance

A substance that can neutralize both acids and bases, such as aluminum oxide.

Amphiprotic Species

A species that can both donate and accept protons in chemical reactions.

pH Definition

The negative logarithm of the hydrogen ion concentration, measuring the acidity or basicity of a solution.

Strong Acid

An acid that completely dissociates in solution, producing a high concentration of hydrogen ions.

Weak Acid

An acid that only partially dissociates in solution, establishing an equilibrium with a high percentage of unreacted molecules.

Neutralization Reaction

A reaction in which an acid and a base react to form water and a salt, canceling out their ionic properties.

Dissociation of Water

The process by which water breaks into hydrogen and hydroxide ions; H2O ⇌ H+ + OH-.

Kw (Ionic Product of Water)

The equilibrium constant for the dissociation of water, value is 1.0 x 10^-14 mol^2 dm^-6 at 25ºC.

pH Scale range

A scale that ranges from 0 (strongly acidic) to 14 (strongly basic).

Hydronium Ion

The ion formed when a water molecule gains a proton, represented as H3O+.

Concentration

The amount of solute (in moles) per liter (mol dm^-3) of solution.

Strength of an Acid

Refers to the degree of ionization or dissociation of the acid in solution.

Metal Oxide Neutralization

Reaction between metal oxides and acids resulting in a salt and water.

Hydroxide Ion

The ion (OH-) produced when a base dissociates in solution.

Gas Evolution in Neutralization

Production of gases, such as CO2, in neutralization reactions with metal carbonates.

Endothermic Process

A process that requires the absorption of heat, like the dissociation of water.

pH Measurement Tools

Devices like pH meters and pH paper used to measure the acidity or basicity of a solution.

Reactivity Series

A ranking of metals based on their ability to displace hydrogen in reactions with acids.

Strong Base Example

Sodium hydroxide (NaOH), which dissociates 100% in solution.

Weak Base Example

Ammonia (NH3), which partially accepts protons from water.

Buffer Action

The ability of a conjugate acid-base pair to resist changes in pH upon addition of small amounts of acid or base.

Acid Strength Determination

Acids are strong if they are fully dissociated into ions in solution.

Chemical Properties of Bases

Substances that can neutralize acids, often containing hydroxide ions.

Equilibrium Constant

A constant that describes the ratio of products to reactants at equilibrium.

Sulfate Salt Formation

Reactions of sulfuric acid typically form sulfate salts.

Hydronium Ion Formation

The formation of H3O+ when acids dissociate in water.

pH Change in Dilution

Diluting a strong acid with water raises the pH, while concentrating it lowers the pH.

Titration Curve

A graph showing the pH of a solution as a function of the volume of a titrant added.

Indicator Function

A chemical that changes color to indicate the pH of a solution.

Hydrogen Ion Concentration

The concentration of H+ ions, essential for determining pH.

Lone Pair Electrons

Electrons that are not shared with another atom and can accept protons.

Chemical Opposites

Acids and bases are classified as chemical opposites due to their properties.

Stoichiometric Reactions

Reactions where reactants are consumed in fixed proportions.

Concentration Units

Measured in moles per liter (mol dm^-3), indicating solute amount.

Neutral Salt Formation

The result of neutralization by the reaction of an acid and a base.

Hydrochloric Acid Reactions

Typically produce chloride salts upon neutralization.

Organic Acids

Acids containing carbon; e.g., ethanoic acid.

Hydrogen Ion Transfer

The fundamental process in acid-base reactions.

Ionization Constant

The degree to which an acid or base dissociates in solution.

Sodium Hydroxide Properties

A strong base that dissociates completely to provide hydroxide ions.

Conductivity of Acids

Acids conduct electricity due to the presence of ions.

pOH Scale

A scale measuring the concentration of hydroxide ions in a solution.

Hydrochloric Acid Properties

A strong acid that ionizes completely in water.

Weak Base Behavior

Only partially accepts protons from acids, establishing an equilibrium.

Brønsted Acid Examples

Common examples include sulfuric acid and hydrochloric acid.

Reversible Reactions

Reactions where products can convert back to reactants.

Chemical Equilibrium

The state where the rates of forward and reverse reactions are equal.

Strong Base Characteristics

Dissociates completely in water producing high concentrations of OH-.

Amphoteric Example

Substances like zinc oxide that can act as both an acid and a base.

Hydrogen Bonding

Interactions between hydrogen and electronegative atoms, affecting acid-base behavior.

Acid-Base Definitions

Arrhenius, Brønsted-Lowry, and Lewis definitions provide different perspectives.

Elastic Collision in Reactions

Occurs in elastic interactions that conserve energy in chemical reactions.

Buffer Solution

A solution that resists changes in pH upon addition of acids or bases.

Avogadro's Law

The principle that equal volumes of gases contain equal numbers of molecules.

Calorimeter Use

A device to measure heat changes in chemical reactions.

Chemical Indicators

Substances that display color changes at specific pH levels.

Titration Endpoint

The stage in titration at which the reaction is complete, typically shown by an indicator.

Dilution Calculation

Determining concentrations based on the dilution factor used in solutions.

Reactivity of Metals with Acids

Dependent on their position in the reactivity series, influencing reaction ability.

Density and Concentration Correlation

Concentration can be related to the density of solutions for calculations.

Chemical Nomenclature

Naming conventions for acids, bases, and their corresponding salts.

Cation and Anion Interaction

The electrostatic attraction between oppositely charged ions in a compound.

Le Chatelier's Principle

Predicts how a system at equilibrium will respond to changes in concentration, temperature, or pressure.

Hydrolysis Reaction

The reaction of a compound with water, affecting solution properties.

Oxidation-Reduction Reaction

Reactions involving the transfer of electrons between species.

Equivalence Point

The point in a titration where equal amounts of acid and base have reacted.