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1000","correct":false,"explanation":"Multiplying would convert dm³ to cm³, making the volume 1000 times too large for $n=cV$. The required conversion from cm³ to dm³ is dividing by 1000."},{"text":"dividing by 100","correct":false,"explanation":"The conversion factor is 1000, not 100, because $1\\,\\mathrm{dm^3}=1000\\,\\mathrm{cm^3}$. Dividing by 100 leaves the volume ten times too large for calculating moles."},{"text":"multiplying by 100","correct":false,"explanation":"This reverses the required direction and uses the wrong conversion factor. To change cm³ into dm³, divide by 1000 before substituting the volume into $n=cV$."}]},{"id":"7d7c1014-a529-4a60-aaae-ee4c8b022269","cardType":"cloze","points":null,"front":"The volume delivered from the burette is the [ ]; the observed indicator colour change is the [ ].","back":"The volume delivered from the burette is the titre; the observed indicator colour change is the end point.","mcqOptions":[{"text":"The volume delivered from the burette is the titre; the observed indicator colour change is the end point.","correct":true,"explanation":"The titre is the volume delivered from the burette, while the end point is identified experimentally by the indicator’s observed colour change."},{"text":"The volume delivered from the burette is the end point; the observed indicator colour change is the titre.","correct":false,"explanation":"These terms have been reversed: the titre is a volume measured from the burette, whereas the end point is the observed indicator colour change used to stop the titration."},{"text":"The volume delivered from the burette is the equivalence point; the observed indicator colour change is the titre.","correct":false,"explanation":"The equivalence point is the theoretical stoichiometric condition, not a measured volume. The measured volume is the titre, and the visible indicator change marks the end point."},{"text":"The volume delivered from the burette is the titre; the observed indicator colour change is the equivalence point.","correct":false,"explanation":"Although the titre is correctly identified, the visible colour change is the end point. The equivalence point is where stoichiometric amounts have reacted and may not exactly match the indicator end point."}]},{"id":"2eaa0ecb-22af-4f62-b96a-011a2f1bf486","cardType":"cloze","points":null,"front":"The point where reactants are mixed in the exact stoichiometric ratio is the [ ].","back":"The point where reactants are mixed in the exact stoichiometric ratio is the equivalence point.","mcqOptions":[{"text":"equivalence point","correct":true,"explanation":"At the equivalence point, the reactants have been mixed in the exact stoichiometric ratio required by the balanced chemical equation."},{"text":"end point","correct":false,"explanation":"The end point is the experimentally observed indicator colour change. The exact stoichiometric ratio is reached at the equivalence point, which may differ slightly from the end point."},{"text":"titre","correct":false,"explanation":"A titre is the volume of solution delivered from the burette, not the stoichiometric condition. The exact reactant ratio defines the equivalence point."},{"text":"buffer point","correct":false,"explanation":"A buffer point describes a region where a solution resists pH change, not exact stoichiometric mixing. The point defined by the required reactant ratio is the equivalence point."}]},{"id":"88921bbe-fe8d-4970-b6ce-a6b5bf954dac","cardType":"basic","points":1,"front":"Which apparatus measures a fixed volume into the conical flask?","back":"A volumetric pipette.","mcqOptions":[{"text":"A volumetric pipette.","correct":true,"explanation":"A volumetric pipette is calibrated to deliver one precise, fixed volume into the conical flask, giving an accurate measured amount of solution."},{"text":"A burette.","correct":false,"explanation":"A burette delivers a variable volume accurately and is read before and after titration. A volumetric pipette is used when one fixed volume must be transferred."},{"text":"A measuring cylinder.","correct":false,"explanation":"A measuring cylinder can measure different volumes but is less precise than a volumetric pipette. The pipette is calibrated to deliver a single fixed volume accurately."},{"text":"A conical flask.","correct":false,"explanation":"A conical flask holds and mixes the reactants but does not measure volume accurately. A volumetric pipette measures and transfers the fixed volume."}]},{"id":"d0bf7d18-27d1-4b14-a2b3-a75b6ae62ff9","cardType":"basic","points":2,"front":"Why rinse the burette with the solution it will contain?","back":"To prevent dilution/contamination of the burette solution.","mcqOptions":[{"text":"To prevent dilution/contamination of the burette solution.","correct":true,"explanation":"Rinsing with the solution removes residual water and other substances from the burette, preventing dilution or contamination that would alter the solution’s concentration."},{"text":"To increase the concentration of the burette solution.","correct":false,"explanation":"Rinsing is not intended to increase concentration. It removes residual water or contaminants; using the same solution prevents dilution or contamination of the burette contents."},{"text":"To prevent evaporation of the burette solution.","correct":false,"explanation":"Rinsing does not prevent evaporation, which is not the main titration error involved. It conditions the burette so leftover water or contaminants cannot alter the solution concentration."},{"text":"To make the burette opaque to light.","correct":false,"explanation":"The burette must remain readable, and opacity is unrelated to rinsing. The purpose is to avoid residual water or contaminants causing dilution or contamination of the burette solution."}]},{"id":"3827454b-63c9-427b-be51-0477fe1caeb0","cardType":"basic","points":2,"front":"Why rinse the conical flask only with deionised water?","back":"Solution rinse would add extra moles to the flask.","mcqOptions":[{"text":"Solution rinse would add extra moles to the flask.","correct":true,"explanation":"Any solution left after rinsing would contain reactant and add extra moles to the flask, changing the amount being titrated. Deionised water adds no relevant reactant moles."},{"text":"Deionised water would add extra moles to the flask.","correct":false,"explanation":"Deionised water does not add meaningful moles of titrant or analyte. A solution rinse is unsuitable because residual solution would add extra reactant moles to the flask."},{"text":"Solution rinse would remove extra moles from the flask.","correct":false,"explanation":"Rinsing with solution would not remove reactant moles; it could leave additional reactant behind. That is why only deionised water is used, since it does not affect the mole calculation."},{"text":"Deionised water would change the stoichiometric ratio.","correct":false,"explanation":"Adding deionised water changes volume and concentration temporarily but not the number of reactant moles. A solution rinse is avoided because it would add extra moles to the flask."}]},{"id":"e4d3ae31-223f-4290-9116-fa071479d1d8","cardType":"basic","points":1,"front":"What maximum difference commonly makes repeated titres concordant?","back":"Within 0.10 cm³.","mcqOptions":[{"text":"Within 0.10 cm³.","correct":true,"explanation":"Repeated titres are commonly considered concordant when their values differ by no more than 0.10 cm³, indicating good repeatability."},{"text":"Within 0.01 cm³.","correct":false,"explanation":"A 0.01 cm³ tolerance is usually too strict for ordinary school burette readings. The commonly applied concordance criterion is a maximum difference of 0.10 cm³."},{"text":"Within 0.20 cm³.","correct":false,"explanation":"A 0.20 cm³ spread is twice the commonly accepted limit and may hide poor repeatability. Concordant titres are normally within 0.10 cm³."},{"text":"Within 1.00 cm³.","correct":false,"explanation":"A 1.00 cm³ difference is far too large to show precise repeatability and could significantly affect the calculated concentration. The usual limit is 0.10 cm³."}]},{"id":"2fcb0a76-e63f-40b6-834b-83bf0a27902c","cardType":"basic","points":1,"front":"Should the rough titre be included in the mean titre?","back":"No - exclude it unless told otherwise.","mcqOptions":[{"text":"No - exclude it unless told otherwise.","correct":true,"explanation":"The rough titre is used to locate the endpoint approximately and may be less accurate. Exclude it from the mean unless instructions specifically say to include it."},{"text":"Yes - include it in every mean titre.","correct":false,"explanation":"The rough titre is not normally included because it is an approximate trial measurement. Calculate the mean from concordant accurate titres, unless told otherwise."},{"text":"Yes - include it only if it is the first titre.","correct":false,"explanation":"Being the first titre does not make it suitable for averaging. The rough titre is normally excluded because it is approximate; only concordant accurate titres should form the mean."},{"text":"No - discard all accurate titres as well.","correct":false,"explanation":"Only the rough titre is normally excluded. Accurate concordant titres are retained and averaged to obtain the best estimate of the titre."}]},{"id":"8a780e01-6d67-4631-a63f-9e4ba418b027","cardType":"basic","points":1,"front":"After finding moles of the known solution, what gives moles of the unknown?","back":"The balanced equation mole ratio.","mcqOptions":[{"text":"The balanced equation mole ratio.","correct":true,"explanation":"Stoichiometric coefficients in the balanced equation determine the proportion in which reactants react, allowing the known amount to be converted into moles of the unknown substance."},{"text":"The known solution concentration value.","correct":false,"explanation":"Concentration is used with volume to calculate the known amount, but it does not convert between substances. The balanced equation’s mole ratio gives the moles of the unknown."},{"text":"The measured solution titre volume.","correct":false,"explanation":"The titre provides the volume used to find the known amount, not the relationship between different reactants. The balanced equation’s mole ratio gives the unknown amount."},{"text":"The chosen indicator colour change.","correct":false,"explanation":"An indicator identifies the end point but provides no stoichiometric conversion between reactants. The balanced equation’s mole ratio determines the moles of the unknown substance."}]},{"id":"b1032ed8-e0fe-4796-90cf-bb054dee08c4","cardType":"basic","points":1,"front":"In H₂SO₄ + 2NaOH, how many moles of NaOH react with 1 mol H₂SO₄?","back":"2 mol of NaOH.","mcqOptions":[{"text":"2 mol of NaOH.","correct":true,"explanation":"The coefficient of NaOH is 2 while that of H₂SO₄ is 1, so two moles of sodium hydroxide neutralise each mole of sulfuric acid."},{"text":"1 mol of NaOH.","correct":false,"explanation":"This incorrectly treats the reactants as having a 1:1 ratio. Sulfuric acid is diprotic, so 1 mol requires 2 mol of NaOH for complete neutralisation."},{"text":"0.5 mol of NaOH.","correct":false,"explanation":"This reverses the 1:2 stoichiometric ratio. Each mole of sulfuric acid supplies two acidic protons and therefore reacts with 2 mol, not 0.5 mol, of NaOH."},{"text":"4 mol of NaOH.","correct":false,"explanation":"This doubles the NaOH coefficient unnecessarily, often by counting both hydrogen atoms twice. The balanced equation shows that exactly 2 mol of NaOH react per mole of acid."}]},{"id":"39f26b34-2d47-4e99-99f5-f05e80e42336","cardType":"basic","points":2,"front":"Calculate moles in 23.60 cm³ of 0.100 mol dm^-3 acid.","back":"0.002360 mol.","mcqOptions":[{"text":"0.002360 mol.","correct":true,"explanation":"Converting gives 23.60 cm³ = 0.02360 dm³. Using $n=cV$ gives $0.100\\times0.02360=0.002360$ mol."},{"text":"2.360 mol.","correct":false,"explanation":"This results from using the numerical volume in cm³ directly with a concentration stated per dm³. Dividing the volume by 1000 gives the correct amount, 0.002360 mol."},{"text":"0.0002360 mol.","correct":false,"explanation":"This is ten times too small because the converted volume has been divided by an extra factor of ten. The correct volume is 0.02360 dm³, giving 0.002360 mol."},{"text":"0.02360 mol.","correct":false,"explanation":"This is ten times too large because 23.60 cm³ has effectively been converted to 0.2360 dm³. The correct conversion gives 0.002360 mol."}]},{"id":"00570789-f8ef-4e7f-96a5-1a1731681306","cardType":"cloze","points":null,"front":"A strong acid [ ] in water; a weak acid [ ].","back":"A strong acid fully dissociates in water; a weak acid partially dissociates.","mcqOptions":[{"text":"A strong acid fully dissociates in water; a weak acid partially dissociates.","correct":true,"explanation":"Strong acids ionise essentially completely in aqueous solution, whereas weak acids establish an equilibrium in which only a proportion of the acid molecules have ionised."},{"text":"A strong acid partially dissociates in water; a weak acid partially dissociates.","correct":false,"explanation":"Partial ionisation is characteristic of a weak acid, not a strong acid. A strong acid dissociates fully in water, while a weak acid dissociates only partially."},{"text":"A strong acid fully dissociates in water; a weak acid does not dissociate.","correct":false,"explanation":"Weak acids do produce ions, but only a fraction of their molecules ionise at equilibrium. Therefore, the strong acid dissociates fully and the weak acid dissociates partially."},{"text":"A strong acid partially dissociates in water; a weak acid fully dissociates.","correct":false,"explanation":"This reverses the definitions of strong and weak acids. Strong acids dissociate fully in water, whereas weak acids establish an equilibrium and dissociate only partially."}]},{"id":"4fc28c1a-71ce-44c8-96d2-5d4940a00ab9","cardType":"cloze","points":null,"front":"A titration curve plots [ ] against [ ].","back":"A titration curve plots pH against volume of acid or base added.","mcqOptions":[{"text":"A titration curve plots pH against volume of acid or base added.","correct":true,"explanation":"During a titration, pH is measured after successive additions of titrant. Plotting it against the cumulative volume added reveals the buffer region and equivalence point."},{"text":"A titration curve plots concentration against volume of acid or base added.","correct":false,"explanation":"Concentration changes during a titration but is not normally the measured vertical-axis variable. A titration curve shows pH against the volume of acid or base added."},{"text":"A titration curve plots pH against time since the titration began.","correct":false,"explanation":"Time is not the independent variable in a standard titration curve because additions are measured by volume. The graph plots pH against the volume of titrant added."},{"text":"A titration curve plots temperature against concentration of the unknown solution.","correct":false,"explanation":"Temperature and concentration may affect an acid-base system, but they are not the standard axes of a titration curve. Its axes are pH and volume of titrant added."}]},{"id":"b21e6f69-1485-49dc-8368-c805031a83b3","cardType":"basic","points":1,"front":"What is the equivalence-point pH for strong acid + strong base at 298 K?","back":"pH 7.","mcqOptions":[{"text":"pH 7.","correct":true,"explanation":"At equivalence, equal amounts of strong acid and strong base have neutralised completely. Their salt does not hydrolyse significantly, so the solution is neutral at 298 K."},{"text":"pH 0.","correct":false,"explanation":"This confuses the initial highly acidic solution with the equivalence point. Complete neutralisation by a strong base produces a neutral solution with pH 7 at 298 K."},{"text":"pH 14.","correct":false,"explanation":"This would represent a strongly alkaline solution containing a large excess of base, not the equivalence point. At equivalence, strong acid and base give pH 7."},{"text":"pH 1.","correct":false,"explanation":"This assumes substantial acid remains at equivalence. The reactants are present in stoichiometrically equal amounts and neutralise completely, producing pH 7 at 298 K."}]},{"id":"7dd7e041-a2fe-4a31-be81-40233ae8f4da","cardType":"basic","points":1,"front":"How does a weak acid’s initial pH compare with a strong acid of the same concentration?","back":"It starts at a higher pH.","mcqOptions":[{"text":"It starts at a higher pH.","correct":true,"explanation":"A weak acid ionises only partially, so it produces a lower equilibrium concentration of H⁺ ions than an equally concentrated strong acid and therefore has a higher pH."},{"text":"It starts at a lower pH.","correct":false,"explanation":"This reverses the effect of partial dissociation. A weak acid releases fewer H⁺ ions than a strong acid of equal concentration, so its initial pH is higher."},{"text":"It starts at the same pH.","correct":false,"explanation":"Equal analytical concentrations do not imply equal H⁺ concentrations because the acids ionise to different extents. The weak acid therefore begins at a higher pH."},{"text":"It starts at a neutral pH.","correct":false,"explanation":"Partial ionisation does not make an acid solution neutral; it still contains excess H⁺ ions. Its pH is higher than the strong acid’s but remains below 7."}]},{"id":"5ca69bc9-1875-46c1-9402-2ede1198267c","cardType":"basic","points":2,"front":"Why is there a buffer region before equivalence for weak acid + strong base?","back":"Both weak acid and conjugate base are present.","mcqOptions":[{"text":"Both weak acid and conjugate base are present.","correct":true,"explanation":"Before equivalence, some acid remains while neutralisation has produced its conjugate base. This conjugate pair can remove added H⁺ or OH^-, resisting pH changes."},{"text":"Both strong acid and conjugate base are present.","correct":false,"explanation":"A strong acid is not generated by partially neutralising a weak acid. The buffer forms because unreacted weak acid and the conjugate base produced by neutralisation coexist."},{"text":"Both weak acid and conjugate acid are present.","correct":false,"explanation":"A buffer requires a weak acid and its conjugate base, not two acidic species. The added alkali converts some weak acid into the corresponding conjugate base."},{"text":"Both weak acid and strong base are present.","correct":false,"explanation":"Before equivalence, added strong base is consumed by the weak acid rather than remaining in the mixture. The resulting weak acid-conjugate base pair creates the buffer region."}]},{"id":"5f170b45-10f8-4dd9-9a66-b628e2c2fd5a","cardType":"basic","points":2,"front":"Why is the equivalence point above pH 7 for weak acid + strong base?","back":"The conjugate base reacts with water to form OH^-.","mcqOptions":[{"text":"The conjugate base reacts with water to form OH^-.","correct":true,"explanation":"At equivalence, the weak acid has been converted into its conjugate base. Hydrolysis produces OH^-, making the solution alkaline and placing the equivalence point above pH 7."},{"text":"The conjugate acid reacts with water to form H⁺.","correct":false,"explanation":"This describes the acidic effect of a conjugate acid, relevant to a weak base titration. Here, the conjugate base hydrolyses to produce OH^-, so the correct explanation involves alkalinity."},{"text":"The strong base reacts with water to form H⁺.","correct":false,"explanation":"A strong base does not produce H⁺ by reacting with water; it supplies OH^-. At equivalence, the weak acid’s conjugate base hydrolyses and makes the solution alkaline."},{"text":"The weak acid reacts with water to form H⁺.","correct":false,"explanation":"Although a weak acid can produce H⁺, it has been neutralised at equivalence. The remaining conjugate base reacts with water to form OH^-, raising the pH above 7."}]},{"id":"1f83acd2-6973-446a-be1c-7dcdbe0b4281","cardType":"basic","points":2,"front":"Why is the equivalence point below pH 7 for strong acid + weak base?","back":"The conjugate acid of the weak base makes it acidic.","mcqOptions":[{"text":"The conjugate acid of the weak base makes it acidic.","correct":true,"explanation":"At equivalence, the weak base has become its conjugate acid. This conjugate acid reacts with water and produces H⁺, so the solution is acidic and the equivalence point lies below pH 7."},{"text":"The conjugate base of the weak acid makes it acidic.","correct":false,"explanation":"A conjugate base normally makes a solution alkaline by accepting protons from water. In this titration, the weak base forms a conjugate acid, which produces H⁺ and lowers the pH."},{"text":"The strong acid remains completely unreacted at equivalence.","correct":false,"explanation":"At equivalence, the strong acid has reacted stoichiometrically with the weak base, so it is not left over. The weak base’s conjugate acid remains and hydrolyses to produce H⁺."},{"text":"The weak base reacts with water to form OH^-.","correct":false,"explanation":"The weak base has been converted mainly into its conjugate acid at equivalence, rather than remaining as the species responsible for the pH. The conjugate acid produces H⁺, making the solution acidic."}]},{"id":"6cde4ae6-e95f-4592-81a4-f93583b9d7e0","cardType":"basic","points":2,"front":"Why is a pH meter more suitable than an indicator for weak acid + weak base titrations?","back":"There is no sharp vertical section.","mcqOptions":[{"text":"There is no sharp vertical section.","correct":true,"explanation":"A weak acid and weak base produce a gradual pH change around equivalence, without a sharp vertical section. An indicator cannot change colour over a sufficiently narrow, clearly defined pH jump."},{"text":"There is a sharp vertical section.","correct":false,"explanation":"A sharp vertical section would provide a clear pH jump for selecting an indicator. Weak acid/weak base titrations lack this feature, so measuring pH directly with a meter is more suitable."},{"text":"The solution has no equivalence point.","correct":false,"explanation":"An equivalence point still exists when stoichiometric amounts have reacted. The problem is that the pH change near it is gradual, making an indicator endpoint difficult to identify accurately."},{"text":"The indicator has no transition range.","correct":false,"explanation":"Indicators do have transition ranges, but none can reliably identify this endpoint because the titration curve lacks a sharp vertical section. A pH meter records the gradual change directly."}]},{"id":"d6bde4b2-c951-44be-b8ee-e1ab5b4b0d4c","cardType":"cloze","points":null,"front":"At half-equivalence in a weak acid/strong base titration, [HA] = [ ] so pH = [ ].","back":"At half-equivalence in a weak acid/strong base titration, [HA] = [A^-] so pH = pK_a.","mcqOptions":[{"text":"At half-equivalence in a weak acid/strong base titration, [HA] = [A^-] so pH = pK_a.","correct":true,"explanation":"Half-equivalence means half the weak acid has been neutralised, leaving equal concentrations of HA and A^-. The Henderson-Hasselbalch equation then gives pH = pK_a."},{"text":"At half-equivalence in a weak acid/strong base titration, [HA] = [OH^-] so pH = pK_b.","correct":false,"explanation":"This confuses the weak acid buffer with a base equilibrium. At half-equivalence, [HA] equals [A^-], and substituting that ratio into the acid equation gives pH = pK_a."},{"text":"At half-equivalence in a weak acid/strong base titration, [HA] = [H^+}] so pH = 1/2pK_a.","correct":false,"explanation":"The hydrogen ion concentration is not equal to the acid concentration in this buffer. Equal HA and A^- concentrations make the logarithmic ratio zero, so pH equals pK_a."},{"text":"At half-equivalence in a weak acid/strong base titration, [HA] = [A^2-] so pH = 2pK_a.","correct":false,"explanation":"The conjugate base of a monoprotic acid is A^-, not A^2-. At half-equivalence, equal HA and A^- concentrations give pH = pK_a, not twice its value."}]},{"id":"04272d9b-ad9c-44dc-97de-0d6d0803ae9b","cardType":"basic","points":2,"front":"At half-equivalence, pH = 4.76. What is $K_a$?","back":"1.7 × 10^-5 mol dm^-3.","mcqOptions":[{"text":"1.7 × 10^-5 mol dm^-3.","correct":true,"explanation":"At half-equivalence, pH equals pK_a, so pK_a = 4.76. Therefore, K_a = 10^-4.76 = 1.7 × 10^-5 mol dm^-3."},{"text":"5.7 × 10^-5 mol dm^-3","correct":false,"explanation":"This value can result from treating 10^-4.76 as though the decimal part were converted incorrectly. Since pH equals pK_a, the correct calculation is 10^-4.76 = 1.7 × 10^-5 mol dm^-3."},{"text":"1.7 × 10^-4 mol dm^-3","correct":false,"explanation":"The power of ten is one order too large, a common place-value error when evaluating 10^-4.76. Using the full pK_a gives 1.7 × 10^-5 mol dm^-3."},{"text":"5.9 × 10^-10 mol dm^-3","correct":false,"explanation":"This incorrectly squares or otherwise overcomplicates the hydrogen ion concentration instead of using K_a = 10^-pK_a. With pK_a = 4.76, K_a is 1.7 × 10^-5 mol dm^-3."}]},{"id":"3f65bbb2-cd38-4e43-b0cb-a4569858eaf6","cardType":"cloze","points":null,"front":"An indicator’s [ ] is the pH range over which it changes colour.","back":"An indicator’s transition range is the pH range over which it changes colour.","mcqOptions":[{"text":"transition range","correct":true,"explanation":"An indicator changes colour over a limited interval of pH rather than at one exact value. This interval is called its transition range and determines which titration endpoints it can detect."},{"text":"equivalence range","correct":false,"explanation":"Equivalence refers to the stoichiometric point in a titration, not the pH interval over which an indicator changes colour. The colour-change interval is called the transition range."},{"text":"neutralisation range","correct":false,"explanation":"Neutralisation describes the reaction between acid and base, but it is not the name for an indicator’s colour-change interval. That pH interval is specifically the transition range."},{"text":"buffer range","correct":false,"explanation":"A buffer range describes the pH region where a buffer resists added acid or alkali. An indicator’s colour change occurs across its transition range, which is a different concept."}]},{"id":"2fdbefc1-c15f-4f66-9f1c-94b6af50c063","cardType":"basic","points":2,"front":"When is an indicator suitable for a titration?","back":"Its transition range lies within the steep vertical section.","mcqOptions":[{"text":"Its transition range lies within the steep vertical section.","correct":true,"explanation":"The indicator must change colour during the rapid pH jump near equivalence. If its transition range lies within the steep vertical section, the observed colour change gives an accurate endpoint."},{"text":"Its transition range lies within the buffer region.","correct":false,"explanation":"The buffer region has relatively small pH changes, so an indicator changing there would give a poor endpoint. Its transition range should lie within the steep vertical section around equivalence."},{"text":"Its transition range lies below the equivalence point.","correct":false,"explanation":"An indicator changing entirely before equivalence would signal an endpoint too early. For accuracy, its transition range must fall within the steep vertical section where the pH changes rapidly."},{"text":"Its transition range lies above the starting pH.","correct":false,"explanation":"Being above the starting pH does not ensure that the indicator changes near equivalence. The essential condition is that its transition range lies within the steep vertical section of the curve."}]},{"id":"c5e907ab-9456-4911-ac3e-ff5b3358afb8","cardType":"basic","points":2,"front":"A curve’s steep section is pH 7.8-10.7. Choose methyl orange or phenolphthalein.","back":"Phenolphthalein - its pH 8.3-10.0 range fits.","mcqOptions":[{"text":"Phenolphthalein - its pH 8.3-10.0 range fits.","correct":true,"explanation":"The indicator’s transition range must lie within the curve’s steep vertical section. Phenolphthalein changes colour from pH 8.3-10.0, which is contained within pH 7.8-10.7."},{"text":"Methyl orange - its pH 3.1-4.4 range fits.","correct":false,"explanation":"Methyl orange changes colour at much lower pH, from 3.1-4.4, outside the steep section at pH 7.8-10.7. Phenolphthalein is suitable because its pH 8.3-10.0 range fits."},{"text":"Methyl orange - its pH 8.3-10.0 range fits.","correct":false,"explanation":"The pH range 8.3-10.0 belongs to phenolphthalein, not methyl orange. Methyl orange changes at pH 3.1-4.4, whereas phenolphthalein fits the steep section."},{"text":"Phenolphthalein - its pH 3.1-4.4 range fits.","correct":false,"explanation":"Phenolphthalein has the suitable indicator identity, but its actual transition range is pH 8.3-10.0, not 3.1-4.4. The latter range belongs to methyl orange and lies outside the steep section."}]}]}],"examCountdown":{"examDate":"2027-05-28","paperLabel":"Paper 1"},"heading":"Acid-base titrations","title":"Acid-base titrations Flashcards","topbar":{"backHref":"/a-level/chemistry/edexcel/flashcards"},"topicSidebar":"$L38"}]}],"topicId":"39d0d4e7-8150-5e5a-a18e-6e2d17048f79","walled":"$L39"}],"$L3a","$L3b"]