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contain."},{"text":"sulfates","correct":false,"explanation":"Sulfates are not universally soluble; barium sulfate, lead(II) sulfate and calcium sulfate are insoluble or only slightly soluble. The universal rule applies to nitrates."},{"text":"chlorides","correct":false,"explanation":"Chlorides are usually soluble, but silver chloride and lead(II) chloride are insoluble. Therefore, chlorides do not satisfy the rule that all such salts dissolve."},{"text":"carbonates","correct":false,"explanation":"Carbonates are generally insoluble except those of Group 1 metals and ammonium. They are not the salt group for which every compound is soluble in water."}]},{"id":"2e771373-7e28-4a30-9519-ca728ff33f04","cardType":"basic","points":2,"front":"Which chlorides are insoluble?","back":"

Silver chloride
Lead(II) chloride

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

Silver chloride
Lead(II) chloride

","correct":true,"explanation":"Silver chloride and lead(II) chloride are the principal insoluble chlorides at this level; most other chlorides dissolve in water."},{"text":"

Barium chloride
Lead(II) chloride

","correct":false,"explanation":"Barium sulfate and lead(II) sulfate are insoluble sulfates, not chlorides. The insoluble chlorides are silver chloride and lead(II) chloride."},{"text":"

Silver chloride
Calcium chloride

","correct":false,"explanation":"Calcium sulfate is an insoluble sulfate, while calcium chloride is soluble. The required insoluble chlorides are silver chloride and lead(II) chloride."},{"text":"

Copper(II) chloride
Iron(III) chloride

","correct":false,"explanation":"Copper(II) chloride and iron(III) chloride are soluble chlorides. The insoluble pair to learn is silver chloride and lead(II) chloride."}]},{"id":"c499308d-e751-4dc9-aebb-fb2dcf35067c","cardType":"basic","points":3,"front":"Which three sulfates are insoluble?","back":"

Barium sulfate
Calcium sulfate
Lead(II) sulfate

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Barium sulfate
Calcium sulfate
Lead(II) sulfate

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Barium sulfate
Silver chloride
Lead(II) sulfate

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Barium sulfate
Copper(II) sulfate
Lead(II) sulfate

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Barium sulfate
Calcium sulfate
Magnesium sulfate

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Carbonates or hydroxides are the groups generally insoluble except with Group 1 metals or ammonium."},{"text":"Sulfates (or chlorides)","correct":false,"explanation":"Sulfates are generally soluble but have particular insoluble examples, rather than the stated Group 1 and ammonium rule. The intended groups are carbonates or hydroxides."},{"text":"Oxides (or nitrates)","correct":false,"explanation":"Oxides are not the anion group described by this standard aqueous solubility rule. Carbonates or hydroxides are generally insoluble, except with Group 1 metals or ammonium."}]},{"id":"77fddc96-ba4a-4dcf-b656-c8763695884c","cardType":"cloze","points":null,"front":"In acid-base chemistry, a proton is a(n) [ ] ion.","back":"In acid-base chemistry, a proton is a(n) $H^{+}$ ion.","mcqOptions":[{"text":"$$H^{+}$","correct":true,"explanation":"A proton is a hydrogen ion formed when a hydrogen atom loses its electron, so in acid-base chemistry it is represented as $H^{+}$."},{"text":"$$e^{-}$","correct":false,"explanation":"An electron has a negative charge and is not a proton. A proton is the positively charged hydrogen ion, represented in acid-base chemistry as $H^{+}$."},{"text":"$$n^{0}$","correct":false,"explanation":"A neutron has no electric charge and is found in an atomic nucleus. The proton involved in acid-base reactions is the positively charged ion $H^{+}$."},{"text":"$$OH^{-}$","correct":false,"explanation":"A hydroxide ion contains oxygen and hydrogen and has a negative charge. It is not a proton; the proton is the hydrogen ion $H^{+}$."}]},{"id":"74dcc511-c5c4-4ad3-b081-c7d6021218ca","cardType":"basic","points":1,"front":"Define an acid in terms of proton transfer.","back":"A proton donor.","mcqOptions":[{"text":"A proton donor.","correct":true,"explanation":"According to the Brønsted-Lowry definition, an acid donates a proton to another species during an acid-base reaction."},{"text":"A proton acceptor.","correct":false,"explanation":"A proton acceptor is a base, not an acid. Acids are defined as proton donors because they transfer $H^{+}$ ions to another species."},{"text":"An electron donor.","correct":false,"explanation":"Electron donation describes a different type of chemical behaviour and does not define an acid in proton-transfer theory. An acid donates a proton."},{"text":"A proton absorber.","correct":false,"explanation":"A proton absorber is not the standard definition of an acid and suggests removal without identifying the transfer role. An acid is a proton donor."}]},{"id":"c543d251-3c55-4e48-8e63-a49f1ece3257","cardType":"basic","points":1,"front":"Define a base in terms of proton transfer.","back":"A proton acceptor.","mcqOptions":[{"text":"A proton acceptor.","correct":true,"explanation":"According to the Brønsted-Lowry definition, a base accepts a proton from another species during an acid-base reaction."},{"text":"A proton donor.","correct":false,"explanation":"A proton donor is an acid, not a base. A base is defined by accepting a proton, or $H^{+}$ ion, during the reaction."},{"text":"An electron acceptor.","correct":false,"explanation":"Electron acceptance does not give the Brønsted-Lowry definition of a base. In proton-transfer theory, a base accepts a proton."},{"text":"A proton absorber.","correct":false,"explanation":"A proton absorber is not the standard term for the proton-transfer definition. The precise description is a proton acceptor."}]},{"id":"590c823e-9a92-401e-8031-cbf8acac3480","cardType":"cloze","points":null,"front":"An alkali is a base that is [ ] in water.","back":"An alkali is a base that is soluble in water.","mcqOptions":[{"text":"soluble","correct":true,"explanation":"An alkali is specifically a base that dissolves in water, producing an alkaline solution. Insoluble bases are not called alkalis."},{"text":"insoluble","correct":false,"explanation":"An insoluble base cannot dissolve to form an alkaline solution in water, so insolubility contradicts the definition of an alkali. The required term is soluble."},{"text":"reactive","correct":false,"explanation":"Many bases can react with acids, but reactivity is not what distinguishes an alkali. An alkali is defined by being soluble in water."},{"text":"concentrated","correct":false,"explanation":"Concentration describes the amount of solute in a solution, not whether a base dissolves. The defining property of an alkali is solubility in water."}]},{"id":"31a90c0d-58d6-4a88-987d-6e4ad9a88612","cardType":"cloze","points":null,"front":"Nitric acid reacts to form [ ].","back":"Nitric acid reacts to form nitrates.","mcqOptions":[{"text":"nitrates","correct":true,"explanation":"Nitric acid produces nitrate salts because its characteristic negative ion is the nitrate ion, $\\mathrm{NO_3^-}$."},{"text":"sulfates","correct":false,"explanation":"Sulfates are formed from sulfuric acid, not nitric acid. Nitric acid supplies nitrate ions, so its reactions form nitrates."},{"text":"chlorides","correct":false,"explanation":"Chlorides are formed from hydrochloric acid, whose negative ion is chloride. Nitric acid contains nitrate ions and therefore forms nitrates."},{"text":"carbonates","correct":false,"explanation":"Carbonates contain the carbonate ion and are not the characteristic salts of nitric acid. Nitric acid reacts to form nitrates."}]},{"id":"e25398bf-2c7f-4193-abc9-f7e4cb66c723","cardType":"basic","points":3,"front":"What products are formed when an acid reacts with a metal carbonate?","back":"

Salt
Water
Carbon dioxide

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

Salt
Water
Carbon dioxide

","correct":true,"explanation":"An acid reacting with a metal carbonate produces a salt, water and carbon dioxide. The carbon dioxide causes the characteristic effervescence."},{"text":"

Salt
Water
Hydrogen

","correct":false,"explanation":"Hydrogen is produced when many metals react with acids, but metal carbonates release carbon dioxide instead. The products are salt, water and carbon dioxide."},{"text":"

Salt
Water
Oxygen

","correct":false,"explanation":"Oxygen is not released in an acid-carbonate reaction. The carbonate ion reacts with acid to produce water and carbon dioxide alongside the salt."},{"text":"

Salt
Water
Carbon monoxide

","correct":false,"explanation":"Carbon monoxide is not formed by the reaction of a carbonate with an acid. The gaseous product is carbon dioxide, together with salt and water."}]},{"id":"a6b44ffc-3526-417d-85be-d372c8e0c2b4","cardType":"basic","points":1,"front":"What is the product of the reaction between ammonia and nitric acid?","back":"Ammonium nitrate","mcqOptions":[{"text":"Ammonium nitrate","correct":true,"explanation":"Ammonia accepts a hydrogen ion from nitric acid, forming the ammonium ion. This combines with nitrate ions to produce ammonium nitrate."},{"text":"Ammonium nitrite","correct":false,"explanation":"Ammonium nitrite contains nitrite ions, but nitric acid supplies nitrate ions. Ammonia and nitric acid therefore form ammonium nitrate."},{"text":"Ammonium sulfate","correct":false,"explanation":"Ammonium sulfate would form from ammonia and sulfuric acid. Because the acid used here is nitric acid, the product is ammonium nitrate."},{"text":"Sodium nitrate","correct":false,"explanation":"Sodium nitrate requires a sodium-containing base or alkali. Ammonia forms ammonium ions, so its reaction with nitric acid produces ammonium nitrate."}]},{"id":"bbf15449-132c-4f98-a04f-4397885ed8e8","cardType":"basic","points":1,"front":"In the preparation of a soluble salt from an insoluble base, why is excess solid added?","back":"To ensure all of the acid has reacted.","mcqOptions":[{"text":"To ensure all of the acid has reacted.","correct":true,"explanation":"Adding excess insoluble base ensures that every available acid particle reacts. Any unreacted solid can then be removed by filtration, leaving a salt solution."},{"text":"To ensure all of the base has reacted.","correct":false,"explanation":"The base is deliberately added in excess, so some of it must remain unreacted. The purpose is to ensure all of the acid has reacted."},{"text":"To increase the acid concentration in the mixture.","correct":false,"explanation":"Adding an insoluble base does not increase the acid concentration because the base neutralises the acid. Excess is used to ensure all of the acid reacts."},{"text":"To ensure the salt precipitates immediately.","correct":false,"explanation":"A soluble salt remains dissolved rather than precipitating immediately. Excess solid is added to ensure all of the acid reacts, after which surplus solid is filtered off."}]},{"id":"ce91b557-11c4-4b51-87f2-c1656edccc0e","cardType":"basic","points":1,"front":"How do you know when the acid is used up when adding an insoluble metal oxide?","back":"Some unreacted solid remains at the bottom of the beaker.","mcqOptions":[{"text":"Some unreacted solid remains at the bottom of the beaker.","correct":true,"explanation":"Once the acid has all reacted, it can no longer dissolve additional metal oxide. The remaining unreacted solid therefore shows that the acid is used up."},{"text":"The metal oxide completely dissolves in the beaker.","correct":false,"explanation":"Complete dissolution suggests that more metal oxide may still react, so it does not show that the acid is exhausted. Unreacted solid must remain as evidence."},{"text":"The bubbling stops at the bottom of the beaker.","correct":false,"explanation":"Metal oxides neutralise acids without producing a gas, so bubbling is not the endpoint. The acid is used up when some unreacted solid remains."},{"text":"The indicator changes colour throughout the beaker.","correct":false,"explanation":"This preparation does not require an indicator, because excess insoluble solid reveals the endpoint. The acid is used up when some unreacted solid remains."}]},{"id":"2c902232-6708-4332-911a-077dbb4a4f3f","cardType":"basic","points":2,"front":"Why should you not evaporate a salt solution to dryness during crystallisation?","back":"

Prevents decomposition of crystals
Allows pure hydrated crystals to form

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

Prevents decomposition of crystals
Allows pure hydrated crystals to form

","correct":true,"explanation":"Heating to complete dryness can drive water from hydrated crystals or thermally decompose the salt. Concentrating and cooling the solution instead allows pure hydrated crystals to form."},{"text":"

Ensures complete evaporation of water
Allows anhydrous crystals to form

","correct":false,"explanation":"Crystallisation does not require every drop of water to be removed, and doing so may decompose the salt. Partial evaporation followed by cooling forms pure hydrated crystals."},{"text":"

Prevents crystallisation of the salt
Keeps all the salt dissolved

","correct":false,"explanation":"Preventing crystallisation would defeat the purpose of the procedure, while keeping all salt dissolved would reduce crystal yield. Avoiding dryness prevents decomposition and preserves hydration."},{"text":"

Produces a larger yield of crystals
Removes all water from crystals

","correct":false,"explanation":"Removing all water can destroy hydrated crystals and may cause decomposition rather than improving purity. The solution is concentrated and cooled so pure hydrated crystals form safely."}]},{"id":"922e5ba6-053b-4cf3-825b-bdbee0b2c567","cardType":"cloze","points":null,"front":"A hydrated crystal contains [ ] built into its crystal structure.","back":"A hydrated crystal contains water molecules built into its crystal structure.","mcqOptions":[{"text":"water molecules","correct":true,"explanation":"Hydrated crystals contain a fixed number of water molecules incorporated within their crystal lattice. This water is known as water of crystallisation."},{"text":"hydroxide ions","correct":false,"explanation":"Hydroxide ions may be part of some compounds, but they do not define hydration. A hydrated crystal specifically contains water molecules within its crystal structure."},{"text":"hydrogen molecules","correct":false,"explanation":"Hydration involves intact water molecules, not hydrogen molecules. A hydrated crystal contains water molecules incorporated into its crystal structure."},{"text":"oxygen atoms","correct":false,"explanation":"Individual oxygen atoms are not what makes a crystal hydrated. Hydrated crystals contain complete water molecules built into the crystal structure."}]},{"id":"2911acd6-e1b0-4873-9fa5-31c0e6c0b3ab","cardType":"basic","points":1,"front":"When making a soluble salt from an acid and alkali, why is a titration repeated without indicator?","back":"To prevent the indicator from contaminating the salt crystals.","mcqOptions":[{"text":"To prevent the indicator from contaminating the salt crystals.","correct":true,"explanation":"Indicator used to locate the endpoint would remain as an impurity in the final solution. Repeating the titration without it produces uncontaminated salt crystals."},{"text":"To prevent the alkali from contaminating the salt crystals.","correct":false,"explanation":"The measured acid and alkali volumes are chosen to react exactly, so excess alkali is already avoided. Repetition without indicator prevents indicator contamination."},{"text":"To make the indicator change colour more sharply.","correct":false,"explanation":"A sharper colour change is useful only when finding the endpoint initially. The repeat uses the known volumes without indicator to avoid contaminating the crystals."},{"text":"To increase the acid concentration in the solution.","correct":false,"explanation":"Repeating without indicator does not increase the acid concentration; the same measured reacting volumes are used. Its purpose is to prevent indicator contamination of the crystals."}]},{"id":"c2360de4-2b55-4110-85e0-3ac499753e17","cardType":"basic","points":1,"front":"What state of reactants are required for a precipitation reaction?","back":"Two soluble solutions.","mcqOptions":[{"text":"Two soluble solutions.","correct":true,"explanation":"Both reactants must be dissolved so their ions can move freely, collide and combine to form the insoluble solid called a precipitate."},{"text":"Two insoluble suspensions.","correct":false,"explanation":"Ions in insoluble suspensions are not freely available throughout the mixture. A precipitation reaction requires two soluble solutions whose dissolved ions form an insoluble product."},{"text":"One solid and one solution.","correct":false,"explanation":"Using a solid prevents its ions from mixing freely with ions throughout the solution. The standard precipitation method mixes two soluble solutions."},{"text":"One solution and one gas.","correct":false,"explanation":"A gas is not required to produce a precipitate. Two soluble solutions are mixed so that selected dissolved ions combine into an insoluble salt."}]},{"id":"f4ee6b01-2c59-40ab-a0a0-00d83ce4ab59","cardType":"basic","points":1,"front":"What is the second step in purifying an insoluble salt after it has been filtered?","back":"Wash with distilled water.","mcqOptions":[{"text":"Wash with distilled water.","correct":true,"explanation":"Distilled water removes soluble impurities remaining on the insoluble salt without introducing additional dissolved ions that could contaminate the product."},{"text":"Dry with filter paper.","correct":false,"explanation":"Drying is performed only after the residue has been washed. The second step is washing with distilled water to remove soluble impurities from the crystals."},{"text":"Wash with tap water.","correct":false,"explanation":"Tap water contains dissolved ions that could contaminate the salt. The filtered residue should instead be washed with distilled water before it is dried."},{"text":"Heat to evaporate water.","correct":false,"explanation":"Strong heating may decompose some salts and does not properly rinse away surface impurities. The residue should first be washed with distilled water."}]},{"id":"b55ee9e3-d3ab-4297-9544-e3364e0cc9d1","cardType":"cloze","points":null,"front":"Mixing lead(II) nitrate and sodium sulfate produces a [ ] precipitate of lead(II) sulfate.","back":"Mixing lead(II) nitrate and sodium sulfate produces a white precipitate of lead(II) sulfate.","mcqOptions":[{"text":"white","correct":true,"explanation":"Lead(II) ions react with sulfate ions to form insoluble lead(II) sulfate, which appears as a white precipitate in the mixture."},{"text":"yellow","correct":false,"explanation":"A yellow precipitate is associated with lead(II) iodide, not lead(II) sulfate. Lead(II) sulfate forms a white precipitate."},{"text":"blue","correct":false,"explanation":"Blue precipitates are commonly associated with copper(II) compounds, such as copper(II) hydroxide. Insoluble lead(II) sulfate is white."},{"text":"green","correct":false,"explanation":"Green precipitates are often associated with some iron(II) compounds. Lead(II) ions and sulfate ions instead produce a white precipitate."}]},{"id":"cdb66926-f86f-471d-868f-a546157a2471","cardType":"cloze","points":null,"front":"Mixing lead(II) nitrate and sodium sulfate produces a white precipitate of [ ].","back":"Mixing lead(II) nitrate and sodium sulfate produces a white precipitate of lead(II) sulfate.","mcqOptions":[{"text":"lead(II) sulfate","correct":true,"explanation":"Lead(II) ions combine with sulfate ions to produce insoluble lead(II) sulfate, while sodium and nitrate ions remain dissolved as spectator ions."},{"text":"sodium nitrate","correct":false,"explanation":"Sodium nitrate remains dissolved because all nitrates and all sodium salts are soluble. The insoluble precipitate formed is lead(II) sulfate."},{"text":"lead(II) nitrate","correct":false,"explanation":"Lead(II) nitrate is one of the soluble reactants, not the precipitate. Its lead(II) ions combine with sulfate ions to form lead(II) sulfate."},{"text":"sodium sulfate","correct":false,"explanation":"Sodium sulfate is the soluble reactant that supplies sulfate ions. These ions combine with lead(II) ions to form the lead(II) sulfate precipitate."}]},{"id":"482224cc-88dd-450e-96c3-96e449125d41","cardType":"basic","points":3,"front":"What general method is used to prepare copper(II) sulfate from copper(II) oxide?","back":"

React with excess oxide
Filter
Crystallise

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

React with excess oxide
Filter
Crystallise

","correct":true,"explanation":"Excess copper(II) oxide ensures all the acid reacts, filtration removes unreacted oxide, and crystallisation recovers pure copper(II) sulfate from the solution."},{"text":"

React with excess acid
Filter
Crystallise

","correct":false,"explanation":"Excess acid would remain dissolved and contaminate the copper(II) sulfate because it cannot be removed by filtration. Excess insoluble oxide should be used instead."},{"text":"

React with excess oxide
Crystallise
Filter

","correct":false,"explanation":"Crystallising before filtration leaves unreacted copper(II) oxide mixed with the crystals. The excess oxide must be filtered off before the solution is crystallised."},{"text":"

React with excess oxide
Filter
Evaporate to dryness

","correct":false,"explanation":"Evaporating to dryness can overheat the hydrated salt and remove its water of crystallisation. The filtered solution should be concentrated and allowed to crystallise."}]}]}],"examCountdown":{"examDate":"2027-05-19","paperLabel":"Paper 1"},"heading":"Acids, bases and salt preparations","title":"Acids, bases and salt preparations Flashcards","topbar":{"backHref":"/igcse/chemistry/edexcel/flashcards"},"topicSidebar":"$L36"}]}],"topicId":"68810669-af33-54ea-b1df-8db852686750","walled":"$L37"}],"$L38","$L39"]