Redox Chemistry & Acid-Base Titrations

A comprehensive set of flashcards focused on redox chemistry and acid-base titrations, including key terms and definitions.

Oxidation

A process involving the loss of electrons or an increase in oxidation state.

Reduction

A process involving the gain of electrons or a decrease in oxidation state.

Redox Reaction

A chemical reaction that involves both oxidation and reduction processes.

Oxidation Number

The charge that would exist on an atom if the bonding were completely ionic.

Disproportionation Reaction

A reaction where the same species is both oxidised and reduced.

Oxidising Agent

A substance that oxidises another atom by causing it to lose electrons.

Reducing Agent

A substance that reduces another atom by causing it to gain electrons.

Half Equation

An equation showing either the oxidation or reduction process in a redox reaction.

Ionic Equation

An equation that shows the species involved in a chemical reaction in ionic form.

Manganate(VII) Ion

MnO4-; a common oxidising agent in redox reactions.

Amber

A color change observed in acid-base titrations that indicates a transition point.

Titration

A technique to determine the concentration of a solution by reacting it with a standard solution.

Indicator

A substance that changes color at a specific pH level.

Conjugate Acid-Base Pair

A pair of compounds that differ by a single proton.

Equivalence Point

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

Concentration (mol/dm³)

The amount of solute (in moles) per volume of solution (in dm³).

Dilute Solution

A solution with a low concentration of solute.

Concentrated Solution

A solution with a high concentration of solute.

Roman Numeral Notation

A method of indicating the oxidation state of elements in compounds.

Alfred Stock

A German chemist known for the Stock notation of oxidation states.

Hydroxide Ion

OH-; often involved in acid-base reactions.

Neutralization Reaction

A reaction where an acid and a base react to form water and a salt.

Charge Balance

A principle used in balancing redox equations ensuring that both sides have equal charges.

Oxidation State of Oxygen

Generally -2 except in peroxides and superoxides.

Loss of Electrons

Occurs during oxidation, resulting in an increase in oxidation state.

Gain of Electrons

Occurs during reduction, resulting in a decrease in oxidation state.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Half Cell Reaction

The reduction or oxidation component of a full redox reaction.

H₂O as a Solvent

Frequently used in reactions and titrations for dissolving solutes.

Experimental Uncertainty

The doubt that exists regarding the result of any measurement.

Percentage Uncertainty

A measure of the uncertainty of a measurement relative to its size.

Volumetric Flask

A piece of laboratory glassware used to prepare solutions at a precise volume.

Burette

A graduated glass tube used to measure and deliver variable amounts of a liquid.

Volumetric Pipette

A pipette used to measure a precise volume of liquid.

Indicators in Titration

Substances that provide a color change to signal the end point of a titration.

Electron Transfer

The movement of electrons from one atom or molecule to another.

Chemical Environment

The local environment around an atom or molecule that influences its chemical behavior.

Hydride Ion

H-; the form of hydrogen with an oxidation state of -1.

Acid-Base Indicator

A substance that changes color depending on the acidity or basicity of a solution.

Chromate Ion

CrO₄²-; can appear in different oxidation states.

Lithium Carbonate

A common compound that can be involved in acid-base reactions.

Sulfur Dioxide

SO₂; an example of a compound that involves variable oxidation states.

Acid-Base Neutralization

The reaction between an acid and a base to yield salt and water.

Iron(II) Ion

Fe²+; known for its role in various redox reactions.

Titration Curve

A graphical representation of the pH change during a titration.

Equivalence Point vs Endpoint

The equivalence point is where the exact reaction occurs; endpoint is where the indicator changes.

Standard Solution

A solution of known concentration used for titrations.

Dissociation in Water

The process by which a compound breaks into its ions in solution.

Flame Test

A qualitative analysis technique to identify metal ions based on the color of flame.

Spectrophotometry

A method for measuring the intensity of light absorbed by a sample.

Gas Chromatography

A method for separating and analyzing compounds that can be vaporized.

Molar Mass

The mass of one mole of a given substance; used in calculations.

Dimensional Analysis

A technique used for converting one unit of measurement to another.

Chemical Reaction Rate

The speed at which reactants are converted into products.

Pathway of Electrons

The route taken by electrons during oxidation and reduction reactions.

Acid-Base Pairs

Conjugate acid-base pairs that exist in equilibrium.

End Point in Titration

The stage in titration where the indicator shows a definitive change.