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24:[["$","$L33",null,{"feature":"flashcards"}],"$L34",["$","$L35",null,{"href":"/a-level/chemistry/aqa/carboxylic-acids-and-esters-a-level-only/flashcards","label":"Carboxylic acids and esters (A-level only)","subjectCode":"a_level_chemistry__aqa","surface":"flashcards"}],["$","$L36",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L37",null,{"decks":[{"id":"fe5a0eb3-d530-48dd-b2ac-9f67cd485388","title":"Carboxylic acids and esters (A-level only) Flashcards","topicId":"1e5dc209-ea42-5f0f-8dc3-7a90cf2afa4a","topicSlug":"carboxylic-acids-and-esters-a-level-only","cards":[{"id":"2c64f9fb-c4f4-4784-8923-a39e3e2414de","cardType":"cloze","points":null,"front":"Carboxylic acids contain [ ]; esters contain [ ].","back":"Carboxylic acids contain -COOH; esters contain -COO-.","mcqOptions":[{"text":"Carboxylic acids contain -COOH; esters contain -COO-.","correct":true,"explanation":"The -COOH group is the carboxyl functional group, while -COO- is the ester linkage connecting the acid-derived and alcohol-derived parts of an ester."},{"text":"Carboxylic acids contain -COO-; esters contain -COOH.","correct":false,"explanation":"The functional groups have been reversed. Carboxylic acids contain -COOH, whereas esters contain the -COO- linkage between two carbon-containing groups."},{"text":"Carboxylic acids contain -CHO; esters contain -COOH.","correct":false,"explanation":"The -CHO group identifies an aldehyde, and -COOH identifies a carboxylic acid rather than an ester. The required groups are -COOH and -COO-, respectively."},{"text":"Carboxylic acids contain -OH; esters contain -CHO.","correct":false,"explanation":"The -OH group alone identifies an alcohol, while -CHO identifies an aldehyde. Carboxylic acids contain -COOH and esters contain -COO-."}]},{"id":"bddfaecd-c310-4a8e-b6c2-75d6765236bb","cardType":"basic","points":1,"front":"What does being a weak acid predict about a carboxylic acid in water?","back":"It only partially dissociates in water.","mcqOptions":[{"text":"It only partially dissociates in water.","correct":true,"explanation":"A weak acid establishes an equilibrium in water in which only a proportion of its molecules donate protons, so most remain undissociated."},{"text":"It completely dissociates in water.","correct":false,"explanation":"Complete dissociation is characteristic of a strong acid, not a weak one. A carboxylic acid only partially dissociates in water, establishing an equilibrium."},{"text":"It only slowly dissociates in water.","correct":false,"explanation":"Weakness refers to the extent of dissociation, not the speed at which dissociation occurs. A carboxylic acid only partially dissociates in water."},{"text":"It remains completely undissociated in water.","correct":false,"explanation":"A carboxylic acid does release protons in water, but only from a fraction of its molecules. It therefore partially dissociates rather than remaining entirely undissociated."}]},{"id":"0ed01980-bffc-4e56-b1e1-6bb3d35a7e43","cardType":"basic","points":2,"front":"Why can the O-H bond in a carboxylic acid release H⁺?","back":"Carboxyl oxygen atoms pull electron density from the hydrogen.","mcqOptions":[{"text":"Carboxyl oxygen atoms pull electron density from the hydrogen.","correct":true,"explanation":"The electronegative oxygen atoms withdraw electron density through the carboxyl group, polarising the O-H bond and allowing the hydrogen to leave as H⁺."},{"text":"Carboxyl carbon atoms pull electron density from the hydrogen.","correct":false,"explanation":"Carbon atoms are not responsible for directly withdrawing electron density from the acidic hydrogen. The electronegative carboxyl oxygen atoms polarise the O-H bond instead."},{"text":"Carboxyl oxygen atoms push electron density towards the hydrogen.","correct":false,"explanation":"Oxygen does not push electron density towards the acidic hydrogen; its electronegativity draws electron density away. This polarises the O-H bond and facilitates H⁺ release."},{"text":"Carboxyl hydrogen atoms pull electron density from the hydrogen.","correct":false,"explanation":"Hydrogen atoms do not withdraw electron density from the acidic hydrogen. The carboxyl oxygen atoms are electronegative and pull electron density away from it."}]},{"id":"93cc4ac6-8fd3-402c-8ccc-985e5659763d","cardType":"basic","points":2,"front":"What happens when a carboxylic acid reacts with sodium carbonate?","back":"It fizzes as carbon dioxide is released.","mcqOptions":[{"text":"It fizzes as carbon dioxide is released.","correct":true,"explanation":"The acid reacts with carbonate ions to form a salt, water and carbon dioxide. Escaping carbon dioxide gas produces the observed fizzing."},{"text":"It fizzes as hydrogen gas is released.","correct":false,"explanation":"Hydrogen gas is associated with acid-metal reactions, not acid-carbonate reactions. Sodium carbonate reacts with the acid to release carbon dioxide, causing fizzing."},{"text":"It shows no visible change because no gas is released.","correct":false,"explanation":"Sodium carbonate is sufficiently basic to react with a carboxylic acid. The reaction releases carbon dioxide gas, so fizzing is observed rather than no visible change."},{"text":"It fizzes as oxygen gas is released.","correct":false,"explanation":"The gas released by an acid-carbonate reaction is carbon dioxide, not oxygen. Its escape from the reaction mixture produces fizzing."}]},{"id":"353ebd96-f441-4c2b-8993-65e96ca585f6","cardType":"basic","points":1,"front":"Why would an alcohol not fizz with sodium carbonate?","back":"It is not acidic enough to liberate carbon dioxide.","mcqOptions":[{"text":"It is not acidic enough to liberate carbon dioxide.","correct":true,"explanation":"Alcohols are much weaker acids than carboxylic acids, so they cannot protonate carbonate ions sufficiently to produce and liberate carbon dioxide gas."},{"text":"It is not soluble enough to liberate carbon dioxide.","correct":false,"explanation":"Solubility is not the decisive issue in this test. An alcohol fails to fizz because it is not acidic enough to react with carbonate and release carbon dioxide."},{"text":"It has no O-H bond to liberate carbon dioxide.","correct":false,"explanation":"Alcohols do contain O-H bonds, but those bonds do not make them sufficiently acidic. They fail to release carbon dioxide because they are not acidic enough."},{"text":"It is not reactive enough to liberate carbon dioxide.","correct":false,"explanation":"Alcohols can undergo many reactions, so a general lack of reactivity is not the explanation. Their acidity is specifically too low to liberate carbon dioxide from carbonate."}]},{"id":"5d1d1c03-a95d-4f78-9ff4-367013273e95","cardType":"basic","points":2,"front":"What conditions form an ester from a carboxylic acid and an alcohol?","back":"

Heat the reactants.
Use concentrated H₂SO₄ as acid catalyst.

","mcqOptions":[{"text":"

Heat the reactants.
Use concentrated H₂SO₄ as acid catalyst.

","correct":true,"explanation":"Heating increases the reaction rate, while concentrated sulfuric acid supplies H⁺ ions to catalyse the reversible esterification reaction without being consumed."},{"text":"

Heat the reactants.
Use dilute HCl as acid catalyst.

","correct":false,"explanation":"Dilute hydrochloric acid introduces substantial water, which favours the reverse hydrolysis equilibrium and reduces ester yield. Concentrated sulfuric acid is the appropriate acid catalyst."},{"text":"

Heat the reactants.
Use concentrated NaOH as base catalyst.

","correct":false,"explanation":"Sodium hydroxide creates alkaline conditions and neutralises the carboxylic acid rather than catalysing esterification. The reactants should be heated with concentrated sulfuric acid."},{"text":"

Cool the reactants.
Use concentrated H₂SO₄ as acid catalyst.

","correct":false,"explanation":"Cooling slows esterification rather than providing the required energy. The reactants are heated and concentrated sulfuric acid is used as the acid catalyst."}]},{"id":"4f81ecc3-a71e-49bb-8d34-6ad787110ec7","cardType":"cloze","points":null,"front":"Esterification forms an ester and [ ]; the reaction is [ ].","back":"Esterification forms an ester and water; the reaction is reversible.","mcqOptions":[{"text":"Esterification forms an ester and water; the reaction is reversible.","correct":true,"explanation":"Esterification is a condensation reaction that produces water alongside the ester. Both products can react to reform the acid and alcohol, making the reaction reversible."},{"text":"Esterification forms an ester and hydrogen; the reaction is reversible.","correct":false,"explanation":"Esterification produces water, not hydrogen, when components of the acid and alcohol combine. The forward and reverse reactions can both occur, so it is reversible."},{"text":"Esterification forms an ester and water; the reaction is irreversible.","correct":false,"explanation":"Water is the correct small-molecule product, but esterification does not normally go to completion. An equilibrium forms because the ester can undergo hydrolysis, making the reaction reversible."},{"text":"Esterification forms an ester and carbon dioxide; the reaction is irreversible.","correct":false,"explanation":"Carbon dioxide is produced in acid-carbonate reactions, not esterification. Esterification forms water and establishes an equilibrium, so the reaction is reversible."}]},{"id":"77eceb80-8a12-49dc-8a62-970ee32bd3e1","cardType":"cloze","points":null,"front":"During esterification, the [ ] group is lost from the carboxylic acid; the [ ] atom is lost from the alcohol.","back":"During esterification, the -OH group is lost from the carboxylic acid; the H atom is lost from the alcohol.","mcqOptions":[{"text":"During esterification, the -OH group is lost from the carboxylic acid; the H atom is lost from the alcohol.","correct":true,"explanation":"The acid supplies its -OH group and the alcohol supplies an H atom, which combine to form water. The alcohol’s oxygen remains in the ester linkage."},{"text":"During esterification, the H group is lost from the carboxylic acid; the -OH atom is lost from the alcohol.","correct":false,"explanation":"This reverses the origins of the components removed as water. The carboxylic acid loses -OH, while the alcohol loses H and retains its oxygen in the ester."},{"text":"During esterification, the -OH group is lost from the carboxylic acid; the -OH atom is lost from the alcohol.","correct":false,"explanation":"The acid does lose -OH, but the alcohol loses only H rather than its entire -OH group. The alcohol’s oxygen becomes part of the ester linkage."},{"text":"During esterification, the =O group is lost from the carboxylic acid; the H atom is lost from the alcohol.","correct":false,"explanation":"The carbonyl oxygen is retained in the ester rather than removed. Water forms from the carboxylic acid’s -OH group and an H atom from the alcohol."}]},{"id":"6ca18e43-5cc0-4353-af99-373d6aae1f81","cardType":"basic","points":2,"front":"How are the two parts of an ester name chosen?","back":"

Alcohol part ends in -yl.
Acid part ends in -oate.

","mcqOptions":[{"text":"

Alcohol part ends in -yl.
Acid part ends in -oate.

","correct":true,"explanation":"The alkyl group comes from the alcohol and uses the -yl ending, while the carboxylate part comes from the acid and uses the -oate ending."},{"text":"

Alcohol part ends in -oate.
Acid part ends in -yl.

","correct":false,"explanation":"This reverses the naming origins: the alcohol supplies the -yl alkyl group, whereas the acid supplies the -oate carboxylate part."},{"text":"

Alcohol part ends in -ane.
Acid part ends in -ol.

","correct":false,"explanation":"These endings belong to other naming patterns, not ester nomenclature. Esters are named using an -yl group from the alcohol and an -oate group from the acid."},{"text":"

Alcohol part ends in -ol.
Acid part ends in -ic.

","correct":false,"explanation":"Those endings describe the original alcohol and carboxylic acid functional groups, rather than the endings used when naming the ester product."}]},{"id":"ab0d1e25-e11c-4a9c-a4d3-4d369bcd7f14","cardType":"basic","points":1,"front":"What is the ester name of CH₃CH₂COOCH₃?","back":"Methyl propanoate.","mcqOptions":[{"text":"Methyl propanoate.","correct":true,"explanation":"The -OCH₃ group gives the methyl part, and the CH₃CH₂COO- section comes from propanoic acid, giving the -oate ending."},{"text":"Propyl methanoate.","correct":false,"explanation":"This swaps the fragments: propyl would require an -OCH₂CH₂CH₃ group, while the structure contains a methyl group attached to oxygen."},{"text":"Ethyl ethanoate.","correct":false,"explanation":"That name corresponds to CH₃COOCH₂CH₃. Here, the oxygen-side group is methyl and the acid-derived chain contains three carbons."},{"text":"Methyl butanoate.","correct":false,"explanation":"The methyl group is identified correctly, but the acid-derived chain has three carbons, not four, so the correct acid-based name uses propanoate."}]},{"id":"75d30f47-2816-4f92-81a1-0f8cf42e91d9","cardType":"basic","points":2,"front":"Why are short-chain esters useful in perfumes and food flavourings?","back":"They are volatile liquids with sweet, fruity smells.","mcqOptions":[{"text":"They are volatile liquids with sweet, fruity smells.","correct":true,"explanation":"Short-chain esters evaporate readily, so their molecules reach the nose easily, and their characteristic sweet, fruity aromas make them suitable for perfumes and flavourings."},{"text":"They are viscous liquids with sharp, acidic smells.","correct":false,"explanation":"High viscosity would hinder evaporation and does not account for their aromas. Short-chain esters are useful because they are volatile liquids with sweet, fruity smells."},{"text":"They are water-soluble liquids with strong, alkaline smells.","correct":false,"explanation":"Water solubility is not the key property, and esters are not characterised by alkaline smells. Their volatility and sweet, fruity aromas make them useful."},{"text":"They are non-volatile liquids with bitter, smoky smells.","correct":false,"explanation":"Low volatility would prevent an aroma from readily reaching the nose. Short-chain esters are instead volatile liquids whose sweet, fruity smells suit these applications."}]},{"id":"479b4bba-adf8-4beb-93f5-3d661b5a3b45","cardType":"basic","points":2,"front":"Why do esters have low boiling points despite being polar liquids?","back":"They lack hydrogen bonding between their own molecules.","mcqOptions":[{"text":"They lack hydrogen bonding between their own molecules.","correct":true,"explanation":"Although ester molecules are polar and have permanent dipole-dipole attractions, they cannot hydrogen-bond to one another because they have no O-H or N-H bond."},{"text":"They have strong ionic bonding between their own molecules.","correct":false,"explanation":"Esters are covalent molecules, not ionic lattices. Their relatively low boiling points result from the absence of hydrogen bonding between ester molecules."},{"text":"They lack permanent dipoles between their own molecules.","correct":false,"explanation":"Esters are polar because their carbonyl and C-O bonds create permanent dipoles. The key missing attraction is hydrogen bonding, not dipole-dipole attraction."},{"text":"They have weak covalent bonds between their own molecules.","correct":false,"explanation":"Covalent bonds hold atoms together within each ester molecule; they are not the intermolecular forces overcome during boiling. The molecules lack hydrogen bonding between themselves."}]},{"id":"ab49fb9d-5fff-4f3f-abd5-9c22a694d1ee","cardType":"basic","points":2,"front":"How do ester plasticisers make rigid polymers flexible?","back":"

They slip between polymer chains.
They weaken intermolecular forces.

","mcqOptions":[{"text":"

They slip between polymer chains.
They weaken intermolecular forces.

","correct":true,"explanation":"Plasticiser molecules fit between polymer chains and reduce the attractions holding neighbouring chains together, so the chains can slide past one another more readily."},{"text":"

They form covalent bonds between polymer chains.
They strengthen intermolecular forces.

","correct":false,"explanation":"Plasticisers do not covalently join chains or strengthen their attractions. They insert between chains and reduce intermolecular forces, allowing the chains to move more easily."},{"text":"

They slip between polymer chains.
They strengthen intermolecular forces.

","correct":false,"explanation":"Insertion between chains is correct, but strengthening their attractions would make the polymer more rigid. Plasticisers weaken intermolecular forces and increase flexibility."},{"text":"

They slip between monomer units.
They weaken intermolecular forces.

","correct":false,"explanation":"The weakening effect is correct, but plasticiser molecules occupy spaces between polymer chains, not between the individual monomer units joined within a chain."}]},{"id":"20918df9-4656-477b-b280-8b7ae968893a","cardType":"cloze","points":null,"front":"Acid hydrolysis of an ester is done by heating under [ ] with a [ ].","back":"Acid hydrolysis of an ester is done by heating under reflux with a dilute acid.","mcqOptions":[{"text":"Acid hydrolysis of an ester is done by heating under reflux with a dilute acid.","correct":true,"explanation":"Reflux allows prolonged heating without losing volatile substances, while dilute acid catalyses ester hydrolysis and supplies the acidic conditions needed for the reaction."},{"text":"Acid hydrolysis of an ester is done by heating under distillation with a dilute acid.","correct":false,"explanation":"Distillation removes and separates volatile components rather than allowing sustained reaction without loss. The correct setup uses reflux with dilute acid."},{"text":"Acid hydrolysis of an ester is done by heating under reflux with a concentrated alkali.","correct":false,"explanation":"An alkali would produce alkaline hydrolysis and a carboxylate salt, not acid hydrolysis. The reaction requires reflux with dilute acid."},{"text":"Acid hydrolysis of an ester is done by heating under reflux with a concentrated acid.","correct":false,"explanation":"Reflux is appropriate, but concentrated acid is not the specified reagent and can promote unwanted side reactions. Acid hydrolysis uses dilute acid."}]},{"id":"9c6b6bcc-d752-42b4-a95f-bad510ca8b14","cardType":"cloze","points":null,"front":"Acid hydrolysis of an ester gives a [ ]; alkaline hydrolysis gives a [ ].","back":"Acid hydrolysis of an ester gives a carboxylic acid; alkaline hydrolysis gives a carboxylate salt.","mcqOptions":[{"text":"Acid hydrolysis of an ester gives a carboxylic acid; alkaline hydrolysis gives a carboxylate salt.","correct":true,"explanation":"Acidic conditions protonate the carboxylate product to form the carboxylic acid, whereas alkaline conditions leave it as the carboxylate salt."},{"text":"Acid hydrolysis of an ester gives an ester; alkaline hydrolysis gives a carboxylate salt.","correct":false,"explanation":"The alkaline product is correctly identified, but hydrolysis breaks the ester bond. Under acidic conditions, the acid-derived product is a carboxylic acid."},{"text":"Acid hydrolysis of an ester gives a carboxylic acid; alkaline hydrolysis gives a carboxylic acid.","correct":false,"explanation":"Acidic conditions give the protonated carboxylic acid, but alkaline conditions deprotonate it and therefore produce a carboxylate salt instead."},{"text":"Acid hydrolysis of an ester gives a carboxylate salt; alkaline hydrolysis gives an alcohol.","correct":false,"explanation":"This reverses the important acid-base outcomes and omits the acid-derived product under alkaline conditions. Acid gives a carboxylic acid, while alkali gives its carboxylate salt."}]},{"id":"39a4debb-31f9-43ef-b903-0d7a7d189583","cardType":"basic","points":2,"front":"Why can acid hydrolysis of an ester not give 100% yield?","back":"It is reversible and reaches equilibrium.","mcqOptions":[{"text":"It is reversible and reaches equilibrium.","correct":true,"explanation":"Ester hydrolysis can proceed in both directions. At equilibrium, reactants and products remain present, so the reaction does not convert all ester into products."},{"text":"It is irreversible and reaches equilibrium.","correct":false,"explanation":"An irreversible reaction would proceed essentially to completion rather than establish a balance of reactants and products. Ester hydrolysis is reversible and reaches equilibrium."},{"text":"It is reversible and goes to completion.","correct":false,"explanation":"Reversibility means the reverse esterification reaction competes with hydrolysis. Equilibrium is therefore established, preventing complete conversion and a 100% yield."},{"text":"It is too slow to reach equilibrium.","correct":false,"explanation":"A catalyst and heating can increase the reaction rate, but they do not remove the equilibrium limitation. The less-than-100% yield results from reversibility."}]},{"id":"1658fe4a-7f6d-42c2-bcec-54465e671aee","cardType":"basic","points":2,"front":"What products form when ethyl ethanoate is heated under reflux with aqueous NaOH?","back":"Sodium ethanoate and ethanol.","mcqOptions":[{"text":"Sodium ethanoate and ethanol.","correct":true,"explanation":"Hydroxide ions hydrolyse ethyl ethanoate into the carboxylate salt sodium ethanoate and the alcohol ethanol under alkaline reflux conditions."},{"text":"Ethanoic acid and ethanol.","correct":false,"explanation":"Ethanoic acid is produced by acidic hydrolysis, not in excess aqueous NaOH. Alkaline hydrolysis forms sodium ethanoate together with ethanol."},{"text":"Sodium ethanoate and methanol.","correct":false,"explanation":"The alcohol comes from the ethyl group attached through oxygen, so it is ethanol rather than methanol. The products are sodium ethanoate and ethanol."},{"text":"Sodium methanoate and methanol.","correct":false,"explanation":"This incorrectly swaps both fragments of the ester. Ethyl ethanoate contains an ethanoate acyl group and an ethyl alkoxy group, producing sodium ethanoate and ethanol."}]},{"id":"fc0f8999-c0a7-41f2-929d-fb50e409a15d","cardType":"basic","points":2,"front":"Why does alkaline hydrolysis of an ester go to completion?","back":"The acid product forms a carboxylate salt, preventing recombination.","mcqOptions":[{"text":"The acid product forms a carboxylate salt, preventing recombination.","correct":true,"explanation":"The carboxylic acid is deprotonated by the alkali to form a carboxylate salt, which does not readily esterify with the alcohol, driving hydrolysis to completion."},{"text":"The alcohol product forms a volatile vapour, preventing recombination.","correct":false,"explanation":"Removing the alcohol is not what drives alkaline hydrolysis. The acid product is converted into a carboxylate salt, preventing it from recombining with the alcohol."},{"text":"The water reactant forms a stable hydrate, preventing recombination.","correct":false,"explanation":"Water is not used up to prevent the reverse reaction. Completion occurs because the carboxylic acid product forms a carboxylate salt that cannot readily re-form the ester."},{"text":"The ester reactant forms an insoluble precipitate, preventing recombination.","correct":false,"explanation":"The ester is not removed by precipitation, as esters are generally molecular liquids. The reaction is driven forward when the acid becomes a carboxylate salt."}]},{"id":"e34b7798-74cf-498f-ba4a-184cdf53de4b","cardType":"cloze","points":null,"front":"Fats and oils are esters of long-chain carboxylic acids and [ ]; glycerol is [ ].","back":"Fats and oils are esters of long-chain carboxylic acids and glycerol; glycerol is propane-1,2,3-triol.","mcqOptions":[{"text":"Fats and oils are esters of long-chain carboxylic acids and glycerol; glycerol is propane-1,2,3-triol.","correct":true,"explanation":"Fats and oils are triesters formed when glycerol reacts with three long-chain carboxylic acids. Glycerol has three hydroxyl groups and is propane-1,2,3-triol."},{"text":"Fats and oils are esters of long-chain carboxylic acids and ethane-1,2-diol; glycerol is ethane-1,2-diol.","correct":false,"explanation":"Ethane-1,2-diol has only two hydroxyl groups and is not glycerol, so it cannot be the alcohol forming the three ester links in a triglyceride."},{"text":"Fats and oils are esters of long-chain carboxylic acids and glycerol; glycerol is propan-1-ol.","correct":false,"explanation":"Glycerol is the correct alcohol component, but its systematic name is propane-1,2,3-triol, not propan-1-ol, because it contains three hydroxyl groups."},{"text":"Fats and oils are esters of long-chain carboxylic acids and propan-1-ol; glycerol is propane-1,2,3-triol.","correct":false,"explanation":"Propan-1-ol is monohydric and forms only one ester bond per molecule. Fats and oils use glycerol, whose systematic name is propane-1,2,3-triol."}]},{"id":"18fbffd1-cb20-48c8-afc0-80f2daab570a","cardType":"basic","points":2,"front":"Why can glycerol form a triglyceride with fatty acids?","back":"Its three -OH groups form three ester bonds.","mcqOptions":[{"text":"Its three -OH groups form three ester bonds.","correct":true,"explanation":"Glycerol contains three hydroxyl groups, and each can react with a fatty acid carboxyl group in a condensation reaction, producing three ester bonds."},{"text":"Its three -COOH groups form three ester bonds.","correct":false,"explanation":"Glycerol has no carboxyl groups; those groups are supplied by the fatty acids. Its three hydroxyl groups each form an ester bond."},{"text":"Its three C-H bonds form three ester bonds.","correct":false,"explanation":"Carbon-hydrogen bonds in glycerol do not undergo esterification. Triglyceride formation uses its three hydroxyl groups, each reacting with a fatty acid."},{"text":"Its three C=C bonds form three ester bonds.","correct":false,"explanation":"Glycerol does not contain carbon-carbon double bonds, and esterification does not involve addition across double bonds. Its three hydroxyl groups form the ester bonds."}]},{"id":"f9109751-2be7-42f0-9856-76f634212b39","cardType":"basic","points":2,"front":"What products form when a triglyceride is hydrolysed with concentrated NaOH?","back":"

One molecule of glycerol.
Three sodium salts of long-chain fatty acids.

","mcqOptions":[{"text":"

One molecule of glycerol.
Three sodium salts of long-chain fatty acids.

","correct":true,"explanation":"Alkaline hydrolysis breaks all three ester bonds in a triglyceride, yielding one glycerol molecule and three carboxylate salts of the long-chain fatty acids."},{"text":"

One molecule of glycerol.
Three free molecules of long-chain fatty acids.

","correct":false,"explanation":"Free fatty acids form after acidification, not directly in concentrated NaOH. The alkaline conditions convert them into three sodium carboxylate salts alongside glycerol."},{"text":"

One molecule of ethane-1,2-diol.
Three sodium salts of long-chain fatty acids.

","correct":false,"explanation":"A triglyceride is derived from glycerol, not ethane-1,2-diol. Complete alkaline hydrolysis therefore gives one glycerol molecule and three sodium salts of fatty acids."},{"text":"

One molecule of propan-1-ol.
Three potassium salts of long-chain fatty acids.

","correct":false,"explanation":"Potassium salts would require KOH rather than NaOH, while propan-1-ol is not the triglyceride backbone. The actual products are glycerol and three sodium salts."}]},{"id":"07871e86-2d55-469d-82a2-a1b2959778f0","cardType":"basic","points":2,"front":"How does crude-oil diesel differ chemically from biodiesel?","back":"

Crude-oil diesel contains long-chain alkanes.
Biodiesel contains long-chain methyl esters.

","mcqOptions":[{"text":"

Crude-oil diesel contains long-chain alkanes.
Biodiesel contains long-chain methyl esters.

","correct":true,"explanation":"Conventional diesel is primarily a mixture of long-chain hydrocarbons, including alkanes, whereas biodiesel consists mainly of long-chain fatty acid methyl esters."},{"text":"

Crude-oil diesel contains long-chain methyl esters.
Biodiesel contains long-chain alkanes.

","correct":false,"explanation":"This reverses the two fuel types. Crude-oil diesel is hydrocarbon-based and contains long-chain alkanes, while biodiesel contains long-chain methyl esters."},{"text":"

Crude-oil diesel contains long-chain alkanes.
Biodiesel contains long-chain carboxylic acids.

","correct":false,"explanation":"Carboxylic acids are feedstocks for ester production rather than the principal components of biodiesel. Biodiesel contains long-chain methyl esters, while crude-oil diesel contains alkanes."},{"text":"

Crude-oil diesel contains short-chain alkenes.
Biodiesel contains long-chain methyl esters.

","correct":false,"explanation":"Short-chain alkenes are volatile petrochemical feedstocks, not the main constituents of diesel. Crude-oil diesel contains long-chain alkanes, whereas biodiesel contains long-chain methyl esters."}]},{"id":"eb5e9d4e-b485-40ce-bdd6-03ecd00bae30","cardType":"cloze","points":null,"front":"To make biodiesel, triglycerides react with [ ] using a strong alkaline catalyst such as [ ].","back":"To make biodiesel, triglycerides react with methanol using a strong alkaline catalyst such as KOH.","mcqOptions":[{"text":"To make biodiesel, triglycerides react with methanol using a strong alkaline catalyst such as KOH.","correct":true,"explanation":"Methanol undergoes transesterification with triglycerides, producing fatty acid methyl esters and glycerol. A strong alkali such as KOH catalyses the reaction."},{"text":"To make biodiesel, triglycerides react with methane using a strong alkaline catalyst such as KOH.","correct":false,"explanation":"Methane is an unreactive alkane and cannot replace the alcohol in transesterification. Methanol is required, with a strong alkaline catalyst such as KOH."},{"text":"To make biodiesel, triglycerides react with methanol using a strong alkaline catalyst such as HCl.","correct":false,"explanation":"Hydrochloric acid is not a strong alkaline catalyst. The specified biodiesel process reacts triglycerides with methanol using an alkali such as KOH."},{"text":"To make biodiesel, triglycerides react with ethanoic acid using a strong alkaline catalyst such as NaCl.","correct":false,"explanation":"Ethanoic acid would not supply the methyl groups needed for fatty acid methyl esters, and NaCl is not an alkaline catalyst. Methanol and KOH are used."}]},{"id":"b416ab0a-7846-4e59-9e5a-a6449fdcf682","cardType":"basic","points":2,"front":"Why is biodiesel production called transesterification?","back":"It swaps glycerol out of the ester for methanol.","mcqOptions":[{"text":"It swaps glycerol out of the ester for methanol.","correct":true,"explanation":"Methanol replaces the glycerol-derived part of triglyceride esters, producing fatty acid methyl esters and glycerol. Exchanging one alcohol-derived group for another makes the process transesterification."},{"text":"It swaps methanol out of the ester for glycerol.","correct":false,"explanation":"This reverses the reaction: methanol is added, while glycerol is released. Biodiesel production swaps glycerol out of triglyceride esters for methanol, forming methyl esters."},{"text":"It swaps fatty acids out of the ester for methanol.","correct":false,"explanation":"The fatty acid chains are retained in the biodiesel molecules rather than removed. Transesterification replaces the glycerol-derived part with methanol while preserving the fatty acid acyl groups."},{"text":"It swaps water out of the ester for methanol.","correct":false,"explanation":"This confuses transesterification with reactions involving water, such as hydrolysis or condensation. Biodiesel production instead exchanges the ester’s glycerol-derived part for methanol."}]}]}],"examCountdown":{"examDate":"2027-05-28","paperLabel":"Paper 1"},"heading":"Carboxylic acids and esters (A-level only)","title":"Carboxylic acids and esters (A-level only) Flashcards","topbar":{"backHref":"/a-level/chemistry/aqa/flashcards"},"topicSidebar":"$L38"}]}],"topicId":"1e5dc209-ea42-5f0f-8dc3-7a90cf2afa4a","walled":"$L39"}],"$L3a","$L3b"]