🔋 Acids, Bases & Electrochemistry
105 chemistry topics in Acids, Bases & Electrochemistry, from beginner to intermediate to advanced level. Each topic has a clear explanation, a worked example, frequently asked questions and an interactive lesson.
Beginner topics in Acids, Bases & Electrochemistry (23)
- Arrhenius Acids and BasesAcids produce H+ in water while bases produce OH- ions.
- Bronsted-Lowry TheoryAcids donate protons and bases accept protons.
- Conjugate Acid-Base PairsSpecies differing by one proton, such as NH4+ and NH3.
- pH ScaleA logarithmic measure of acidity, pH equals minus log of hydrogen ion concentration.
- pOH and pKwpOH equals minus log of hydroxide concentration, and pH plus pOH equals 14 at 25 C.
- Strong AcidsAcids that ionize completely in water, such as HCl, HBr, HI, HNO3, H2SO4 and HClO4.
- Strong BasesBases that dissociate completely, such as group 1 hydroxides and Ba(OH)2.
- Acid-Base NeutralizationAcid and base react to form salt and water.
- Acid-Base IndicatorsWeak acids or bases whose color differs between protonated and deprotonated forms.
- Universal IndicatorA mixture of indicators giving a range of colors across the pH scale.
- Oxidation NumberThe hypothetical charge of an atom if bonds were fully ionic.
- OxidationLoss of electrons, increase in oxidation number.
- ReductionGain of electrons, decrease in oxidation number.
- Redox ReactionsReactions involving transfer of electrons between species.
- Oxidizing AgentThe species that gains electrons and is reduced.
- Reducing AgentThe species that loses electrons and is oxidized.
- Anode and CathodeOxidation occurs at the anode and reduction at the cathode.
- Dry CellA zinc-carbon battery with a paste electrolyte, used in torches and remotes.
- CorrosionGradual destruction of metals by electrochemical reaction with the environment.
- Rusting of IronIron oxidizes in the presence of oxygen and water to form hydrated iron(III) oxide.
- Strong and Weak ElectrolytesStrong electrolytes dissociate fully while weak electrolytes dissociate partially.
- Acid RainRain acidified by sulfur and nitrogen oxides forming sulfuric and nitric acids.
- AntacidsWeak bases that neutralize excess stomach acid.
Intermediate topics in Acids, Bases & Electrochemistry (48)
- Lewis Acids and BasesLewis acids accept electron pairs and Lewis bases donate them.
- Amphoteric SubstancesSpecies that can act as either acid or base, such as water and bicarbonate.
- Autoionization of WaterWater molecules transfer protons to form H3O+ and OH-, with Kw of 1e-14 at 25 C.
- Weak AcidsAcids that only partially ionize in water, described by Ka.
- Weak BasesBases that partially react with water, described by Kb.
- Acid Dissociation ConstantKa measures the extent of acid ionization; larger Ka means a stronger acid.
- Ka and Kb RelationshipFor a conjugate pair, Ka times Kb equals Kw.
- Percent IonizationThe fraction of acid molecules ionized, which increases with dilution.
- pH of Weak Acid SolutionsCalculated using an ICE table and Ka, often with the small-x approximation.
- Polyprotic AcidsAcids with more than one ionizable proton, each step having a smaller Ka.
- Hydrolysis of SaltsIons of weak acids or bases react with water, making salt solutions acidic or basic.
- pH of Salt SolutionsSalts of strong acid with weak base are acidic, strong base with weak acid are basic.
- TitrationA procedure that determines unknown concentration by adding a standard solution until the…
- Equivalence PointThe point at which stoichiometrically equal amounts of acid and base have reacted.
- End PointThe point at which the indicator changes color, ideally close to equivalence.
- Titration CurveA plot of pH versus titrant volume showing a steep rise at equivalence.
- Strong Acid Strong Base TitrationThe equivalence point is at pH 7.
- Buffer SolutionsMixtures of weak acid and conjugate base that resist pH change.
- Henderson-Hasselbalch EquationpH equals pKa plus log of base over acid concentration ratio.
- DisproportionationA species is simultaneously oxidized and reduced, such as H2O2 forming water and oxygen.
- Balancing Redox: Half-Reaction MethodSplit the reaction into oxidation and reduction halves, balance atoms and charge, then…
- Balancing in Acidic and Basic MediumBalance O with H2O and H with H+, then add OH- to convert to basic solution.
- Electrochemical CellA device that converts chemical energy to electrical energy or vice versa.
- Galvanic CellA spontaneous redox reaction produces electric current.
- Electrolytic CellElectrical energy drives a nonspontaneous reaction.
- Salt BridgeAllows ion flow to maintain charge neutrality between half-cells.
- Cell NotationShorthand like Zn|Zn2+||Cu2+|Cu representing anode, cathode and salt bridge.
- Standard Electrode PotentialThe voltage of a half-cell relative to the standard hydrogen electrode under standard…
- Standard Hydrogen ElectrodeThe reference electrode defined as 0.00 V, with hydrogen gas at 1 bar over platinum in 1…
- Cell PotentialThe voltage of a cell equals cathode potential minus anode potential.
- Electrochemical SeriesSpecies ranked by reduction potential, predicting oxidizing and reducing strength.
- Spontaneity from Cell PotentialA positive standard cell potential indicates a spontaneous reaction.
- Faraday's ConstantThe charge on one mole of electrons, 96485 coulombs.
- Faraday's First LawMass deposited during electrolysis is proportional to the charge passed.
- Electrolysis of Molten SaltsPassing current through molten NaCl yields sodium at the cathode and chlorine at the…
- ElectroplatingCoating an object with a metal layer by electrolysis.
- Alkaline BatteryZinc and manganese dioxide cell with potassium hydroxide electrolyte providing long life.
- Lead-Acid BatteryA rechargeable battery with lead and lead dioxide plates in sulfuric acid, used in…
- Lithium-Ion BatteryLithium ions shuttle between graphite anode and metal oxide cathode, giving high energy…
- Fuel CellsCells that convert fuel such as hydrogen directly into electricity with water as the…
- Prevention of CorrosionPainting, galvanizing, alloying and cathodic protection prevent corrosion.
- GalvanizationCoating iron with zinc, which protects both by barrier and sacrificial action.
- pH MeterMeasures potential across a glass electrode to give pH.
- Hydrogen Production by ElectrolysisSplitting water into hydrogen and oxygen using electricity, possibly from renewable…
- Ocean AcidificationAbsorbed CO2 forms carbonic acid, lowering ocean pH and harming shell-forming organisms.
- Acid AnhydridesOxides that form acids with water, such as SO3 giving sulfuric acid.
- Basic AnhydridesMetal oxides that form bases with water, such as CaO giving calcium hydroxide.
- Water HardnessDissolved calcium and magnesium ions that form scum with soap and scale in kettles.
Advanced topics in Acids, Bases & Electrochemistry (34)
- Acid Strength and StructureAcidity increases with bond polarity and weaker H-X bonds, and with more oxygen atoms on…
- Weak Acid Strong Base TitrationEquivalence point is above pH 7 and the half-equivalence pH equals pKa.
- Choosing IndicatorsThe indicator's pKa range should lie within the steep section of the titration curve.
- Buffer CapacityThe amount of acid or base a buffer can neutralize before pH changes significantly.
- Blood Buffer SystemCarbonic acid and bicarbonate keep blood pH near 7.4.
- Nernst EquationCalculates cell potential under nonstandard conditions from the reaction quotient.
- Cell Potential and Free EnergyDelta G equals minus n F E, linking voltage to Gibbs energy.
- Cell Potential and EquilibriumE standard equals RT over nF times ln K, giving equilibrium constants from voltages.
- Concentration CellsCells with identical electrodes differing only in concentration, producing voltage from…
- Faraday's Second LawMasses deposited by the same charge are proportional to equivalent weights.
- Electrolysis of Aqueous SolutionsWater may be oxidized or reduced instead of ions, depending on potentials.
- ElectrorefiningPurifying metals such as copper by anodic dissolution and cathodic deposition.
- Hall-Heroult ProcessAluminium is produced by electrolysis of alumina dissolved in molten cryolite.
- Chlor-Alkali ProcessElectrolysis of brine produces chlorine, hydrogen and sodium hydroxide.
- Nickel-Metal Hydride BatteryA rechargeable battery using a hydrogen-absorbing alloy anode and nickel oxyhydroxide…
- Solid-State BatteriesBatteries using solid electrolytes for greater safety and energy density.
- Sacrificial AnodeA more reactive metal such as zinc or magnesium corrodes in place of iron.
- Conductance and ConductivityConductance is the ease of current flow; conductivity is conductance per unit geometry.
- Molar ConductivityConductivity divided by electrolyte concentration, rising on dilution.
- Kohlrausch's LawLimiting molar conductivity of an electrolyte is the sum of contributions of its…
- Ionic MobilitySpeed of an ion in an electric field, high for H+ because of proton hopping.
- Transport NumberFraction of total current carried by a particular ion.
- Debye-Huckel TheoryDescribes how ionic atmospheres affect activity coefficients in electrolyte solutions.
- Ionic StrengthA measure of total ion concentration weighted by charge squared.
- Activity and Activity CoefficientsEffective concentrations accounting for interactions among ions.
- OverpotentialThe extra voltage needed beyond the thermodynamic value to drive an electrode reaction at…
- Pourbaix DiagramPlots stable species of an element against pH and potential.
- Latimer and Frost DiagramsGraphical summaries of reduction potentials across oxidation states.
- Ion-Selective ElectrodesSensors such as the glass pH electrode that respond to a specific ion.
- Leveling EffectIn a given solvent, no acid stronger than the solvent's conjugate acid can exist.
- Nonaqueous Acids and BasesAcid-base behavior in solvents such as liquid ammonia follows solvent-system definitions.
- SuperacidsAcids stronger than 100 percent sulfuric acid, such as fluoroantimonic acid.
- Hard and Soft Acids and BasesHard acids prefer hard bases and soft acids prefer soft bases, guiding stability of…
- AlkalinityThe capacity of water to neutralize acid, mainly from bicarbonate, carbonate and…
Frequently asked questions about Acids, Bases & Electrochemistry
How many topics are in Acids, Bases & Electrochemistry?
Acids, Bases & Electrochemistry has 105 topics, from beginner to intermediate to advanced level.
Where should I start in Acids, Bases & Electrochemistry?
Start with Arrhenius Acids and Bases at the beginner level, then work through the topics in order.
Does every topic have an explanation and an example?
Yes. Each topic page has an in-depth explanation, a worked example, FAQs and links to related topics.