Key term
CCEA A-Level Chemistry 1110
Formulae, Equations and Amounts of Substance
Atomic Structure
Topic overviewProtons, neutrons and electronsAtomic number, mass number and the composition of ionsIsotopes and relative isotopic massRelative atomic, molecular and formula massMass spectra and relative atomic mass calculationsMass spectra of diatomic elementsElectronic configuration and the building up principleOrbitals, electron spin and orbital shapesThe s-, p-, d- and f-blocks of the Periodic TableIonisation energies and their equationsTrends in ionisation energy as evidence for shells and subshells
Bonding
Topic overviewIonic bonding and electron transferDot and cross diagrams for ionic compoundsCovalent bonding and the shared pairLone pairs and co-ordinate bondingDot and cross diagrams for covalent molecules and ionsThe octet rule and its limitationsElectronegativity and bond polarityMetallic bonding
Intermolecular Forces and Structure
Shapes of Molecules and Ions
Redox
The Halogens
Acid-Base Titrations
Qualitative Tests
Formulae and Amounts of a Substance
Nomenclature and Isomerism in Organic Chemistry
Alkanes
Topic overviewAlkanes as saturated hydrocarbonsBoiling points of alkanes and van der Waals' forcesBoiling points of branched isomersComplete and incomplete combustion of alkanesPollutants from alkane fuels and the atmosphereCatalytic convertersRadicals, homolytic fission and heterolytic fissionFree radical substitution of alkanes
Alkenes
Topic overviewUnsaturated hydrocarbons and the bromine water testSigma and pi bonds in the carbon–carbon double bondElectron density at C=C, reactivity and catalytic hydrogenationAddition of chlorine and bromine to alkenesAddition of hydrogen chloride and hydrogen bromideElectrophiles, heterolytic fission and the addition mechanismCarbocation stability and Markovnikov additionAddition polymerisation of alkenes
Halogenoalkanes
Topic overviewClassification and boiling points of halogenoalkanesLaboratory preparation of a halogenoalkane from an alcoholNucleophiles and hydrolysis with aqueous alkaliReactions with ammonia and with potassium cyanideRelative rates of hydrolysis and carbon–halogen bond enthalpyElimination using ethanolic potassium hydroxideCFCs and the ozone layer
Alcohols
Infrared Spectroscopy
Energetics
Topic overviewExothermic and endothermic changesStandard conditions and the standard enthalpy changeEnthalpy level diagramsStandard enthalpies of combustion and formationStandard enthalpy of neutralisationMeasuring enthalpy changes by experimentEnthalpy calculations using q = mcΔTHess's Law and enthalpy cyclesIndirect enthalpy calculations using Hess's LawAverage bond enthalpies and their limitations
Kinetics
Equilibrium
Group II Elements and Their Compounds
Topic overviews-block character and electronic configurationTrends in atomic radius and first ionisation energyReactions of the elements with oxygen, water and dilute acidsThe oxides and their reactions with water and dilute acidsThermal stability of the carbonates and hydroxidesUses of magnesium oxide, calcium carbonate and limeSolubility trends and solubility curves
Lattice Enthalpy, Entropy and Free Energy
Topic overviewLattice enthalpy and the factors that control itBorn–Haber cycles for Group I halidesBorn–Haber cycles for Group II halides and oxidesEnthalpy of hydration and enthalpy of solutionCalculations on dissolving ionic compoundsEntropy and the limits of enthalpy changeStandard entropy change calculationsFree energy and the temperature of feasibility
Rates of Reaction
Equilibrium and Acid-Base Equilibria
Topic overviewEquilibrium concentrations from initial amountsKc expressions, values and unitsBrønsted–Lowry acids, bases and conjugate pairsKw, pH and the pH of strong acids and basesKa, pKa and the pH of weak acidsBuffer solutions and how they resist pH changeCalculating the pH of a buffer solutionTitration curves, indicators and the pH of salt solutions
Isomerism
Aldehydes and Ketones
Topic overviewStructure and naming of aldehydes and ketonesBoiling points and solubility of carbonyl compoundsPreparation from primary and secondary alcoholsReaction with hydrogen cyanide and the nucleophilic addition mechanismRacemic mixtures from nucleophilic addition2,4-dinitrophenylhydrazine and the identification of carbonylsDistinguishing aldehydes from ketones, and reduction with lithal
Carboxylic Acids
Derivatives of Carboxylic Acids
Topic overviewEsters and acyl chlorides: structure and namingBoiling points and solubility of monoestersMaking esters from alcohols with carboxylic acids or acyl chloridesThe laboratory preparation of a liquid esterFats and oils as esters of glycerolTransesterification, biodiesel and margarineReactions of acyl chlorides with water and alcohols
Aromatic Chemistry
Spectroscopy and Chromatography
Topic overviewThe mass spectrum: molecular ion and base peakFragmentation and the formulae of fragment ionsHigh resolution mass spectrometryNuclear magnetic resonance and the TMS standardChemically equivalent hydrogens and chemical shiftIntegration curvesSpin–spin splitting and the n+1 ruleDeducing a structure from an nmr spectrumPaper and thin-layer chromatographyGas–liquid chromatography
Volumetric Analysis
Transition Metals
Topic overviewThe characteristic properties of the transition metalsElectronic configurations of the metals and their ionsComplexes, ligands and coordination numberOxidation number, redox and disproportionationMonodentate, bidentate and polydentate ligandsLigand strength and the entropy of ligand replacementLigand replacement in copper(II) complexesThe colours of the aqueous transition metal ionsHydroxide precipitates with sodium hydroxidePrecipitates with aqueous ammonia and their dissolutionVanadium and the interconversion of its oxidation states
Electrode Potentials
Amines
Amides and Polymers
Amino Acids and Proteins
Equilibrium and Acid-Base Equilibria
- 8 subtopics
- 24 things to know
- Unit A2 1
What Equilibrium and Acid-Base Equilibria covers
Equilibrium and Acid-Base Equilibria is examined in Unit A2 1, Further Physical and Organic Chemistry, and drawn on again in Unit A2 3, Further Practical Chemistry. It covers equilibrium concentrations from initial amounts, Kc expressions, values and units, Brønsted–Lowry acids, bases and conjugate pairs, Kw, pH and the pH of strong acids and bases, Ka, pKa and the pH of weak acids, buffer solutions and how they resist pH change, calculating the pH of a buffer solution and titration curves, indicators and the pH of salt solutions.
Where it is assessed
Unit A2 1
Further Physical and Organic Chemistry, and again in Unit A2 3, Further Practical Chemistry.
Check the CCEA specification ↗The 8 subtopics
Each one has its own page.
- Equilibrium concentrations from initial amountsRecall questions on the initial, change and equilibrium layout, why the changes follow the balancing numbers, worked examples on hydrogen with iodine, an esterification, the dissociation of dinitrogen tetroxide and of phosphorus pentachloride, converting moles to concentrations, and what a negative equilibrium amount shows.Open →
- Kc expressions, values and unitsRecall questions on writing the expression from the equation and the rule for which side goes on top, deducing units by cancelling, the units for four named equilibria, calculating Kc from given equilibrium concentrations for hydrogen iodide, dinitrogen tetroxide, an ester and phosphorus pentachloride, and the one condition that alters its value.Open →
- Brønsted–Lowry acids, bases and conjugate pairsBrønsted–Lowry acid, brønsted–Lowry base and conjugate acid-base pair.Open →
- Kw, pH and the pH of strong acids and basesIonic product of water, effect on pH of diluting a strong acid ten times and why the pH scale is logarithmic rather than linear.Open →
- Ka, pKa and the pH of weak acidsWeak acid and units of Ka for a weak monobasic acid.Open →
- Buffer solutions and how they resist pH changeBuffer solution and buffer capacity of a solution.Open →
- Calculating the pH of a buffer solutionRecall questions on the buffer expression and why it uses the ratio of acid to salt, calculating the pH of ethanoic acid and propanoic acid buffers, working from an acid partly neutralised by alkali, why pH equals pKa at half-neutralisation, finding the ratio needed for a target pH, and showing the effect of added alkali.Open →
- Titration curves, indicators and the pH of salt solutionsHow a titration curve is obtained experimentally and rule for choosing an indicator for a titration.Open →
What you need to know
Answer each one before you reveal it.
Your recallNot started
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Describe how a titration curve is obtained experimentally.
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Describe the layout used to work out equilibrium amounts from initial amounts.
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Write the expression for Kc for the equilibrium H₂(g) + I₂(g) ⇌ 2HI(g).
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Define the ionic product of water.
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Define a weak acid.
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State the two components of an acidic buffer solution.
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State the expression used to find the hydrogen ion concentration of an acidic buffer.
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Why must the change in moles for each species follow the balancing numbers in the equation?
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Write the expression for Kc for the equilibrium N₂(g) + 3H₂(g) ⇌ 2NH₃(g).
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Define a Brønsted–Lowry acid.
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State the value and units of Kw at 298 K.
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Write the expression for the acid dissociation constant of a weak monobasic acid HA.
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Name a pair of substances that could be mixed to make an acidic buffer.
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Explain why the pH at half-neutralisation of a weak acid equals its pKa.
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Why are additions made in smaller portions near the equivalence point when a titration curve is obtained?
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One mole of ethanoic acid and one mole of ethanol reach equilibrium with Kc = 4. State the amount of water present at equilibrium
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State the rule for the position of products and reactants in a Kc expression.
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Define a Brønsted–Lowry base.
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Define pH.
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State the units of Ka for a weak monobasic acid.
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Explain the role of the salt in a buffer solution.
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A buffer of pH 4.58 rises only to pH 4.76 when a quantity of alkali is added. Explain how this demonstrates buffering
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Why is a pH meter used rather than an indicator when a full titration curve is required?
Take Equilibrium and Acid-Base Equilibria further
The same content, four other ways.
Questions from this topic
Each one with the model answer underneath.
- 1
Describe the layout used to work out equilibrium amounts from initial amounts.
Model answer
A table is drawn with a row for the initial moles, a row for the change in moles, and a row for the equilibrium moles of each species.
- 2
Why must the change in moles for each species follow the balancing numbers in the equation?
Model answer
The stoichiometry fixes the ratio in which species are used up and formed, so if one mole of a reactant reacts the others change by the amounts the equation requires.
- 3
In the reaction H₂(g) + I₂(g) ⇌ 2HI(g), 1.00 mol of each reactant is placed in a 1.00 dm³ vessel and 1.56 mol of HI is present at equilibrium. Calculate the equilibrium moles of hydrogen.
Model answer
Forming 1.56 mol of HI uses 0.78 mol of hydrogen, so 1.00 − 0.78 = 0.22 mol of hydrogen remains.
- 4
1.00 mol of ethanoic acid and 1.00 mol of ethanol are mixed and 0.667 mol of ester is present at equilibrium. Calculate the equilibrium moles of ethanoic acid.
Model answer
Forming 0.667 mol of ester consumes 0.667 mol of acid, so 1.00 − 0.667 = 0.333 mol of ethanoic acid remains.
- 5
In that esterification mixture, state the amount of water present at equilibrium.
Model answer
Water is formed in a one to one ratio with the ester, so 0.667 mol of water is present.
- 6
1.00 mol of N₂O₄ is placed in a 2.00 dm³ vessel and 0.60 mol remains at equilibrium in the reaction N₂O₄(g) ⇌ 2NO₂(g). Calculate the equilibrium concentration of NO₂.
Model answer
0.40 mol of N₂O₄ has dissociated, producing 0.80 mol of NO₂, so the concentration is 0.80 ÷ 2.00 = 0.40 mol dm⁻³.
What is inside Levo
Six ways to work the same material.
Equilibrium and Acid-Base Equilibria revision questions
- What does Equilibrium and Acid-Base Equilibria cover in CCEA A-Level Chemistry?
- 8 subtopics: equilibrium concentrations from initial amounts, kc expressions, values and units, brønsted–lowry acids, bases and conjugate pairs, kw, ph and the ph of strong acids and bases, ka, pka and the ph of weak acids, buffer solutions and how they resist ph change, calculating the ph of a buffer solution and titration curves, indicators and the ph of salt solutions. Each one has its own page with questions and model answers.
- How is Equilibrium and Acid-Base Equilibria organised?
- By the CCEA 1110 specification, subtopic by subtopic, so it matches the order you are taught it in.
Every question in Equilibrium and Acid-Base Equilibria, on a schedule.
Attempt a question from memory, write the correct version, then attempt it again. Levo records the jump between your first attempt and your last, and brings each question back on the day you are due to forget it.
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