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23:[["$","$L32",null,{"feature":"flashcards"}],"$L33",["$","$L34",null,{"href":"/as-level/chemistry/edexcel/as-buffers/flashcards","label":"Buffers","subjectCode":"as_level_chemistry","surface":"flashcards"}],["$","$L35",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L36",null,{"decks":[{"id":"ec3452c2-c5dd-462e-af82-1c3139f4e063","title":"Buffers Flashcards","topicId":"9a7a1f4c-4e59-564c-8de2-2dbcfcfbe481","topicSlug":"as-buffers","cards":[{"id":"dbda967c-e9ea-48f0-891b-0b2b75e115db","cardType":"basic","points":1,"front":"What is the primary function of a buffer solution?","back":"Resists pH change when small amounts of acid or alkali are added.","mcqOptions":[{"text":"Resists pH change when small amounts of acid or alkali are added.","correct":true,"explanation":"A buffer contains a weak acid and its conjugate base, which react with added alkali or acid respectively, limiting the change in hydrogen ion concentration and pH."},{"text":"Maintains a constant pH when large amounts of acid or alkali are added.","correct":false,"explanation":"Buffers limit pH changes only when small amounts are added; large additions can use up one component. The correct function is resisting pH change when small amounts are added."},{"text":"Causes a large pH change when small amounts of acid or alkali are added.","correct":false,"explanation":"A large pH change describes an unbuffered solution, not a buffer. The buffer’s weak acid and conjugate base react with additions to resist small pH changes."},{"text":"Keeps the solution at pH 7 when small amounts of acid or alkali are added.","correct":false,"explanation":"Buffers can operate at acidic or alkaline pH, so they do not necessarily maintain pH 7. Their primary function is resisting pH change after small additions."}]},{"id":"e3b97223-e79f-421c-9e0f-5597566f8a25","cardType":"basic","points":1,"front":"What two components are required to make an acidic buffer?","back":"

A weak acid
A salt of its conjugate base

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

A weak acid
A salt of its conjugate base

","correct":true,"explanation":"An acidic buffer needs a weak acid and a soluble source of its conjugate base. Together, they remove added hydroxide ions and hydrogen ions, limiting pH change."},{"text":"

A strong acid
A salt of its conjugate base

","correct":false,"explanation":"A strong acid dissociates almost completely and does not establish the required weak acid-conjugate base equilibrium. The correct components are a weak acid and a salt of its conjugate base."},{"text":"

A weak base
A salt of its conjugate acid

","correct":false,"explanation":"These components form a basic buffer rather than an acidic buffer. An acidic buffer specifically requires a weak acid together with a salt containing its conjugate base."},{"text":"

A strong acid
A salt of its conjugate acid

","correct":false,"explanation":"A strong acid and a salt of its conjugate acid do not provide the weak acid-conjugate base pair needed for buffering. The required pair is a weak acid and its conjugate base salt."}]},{"id":"54e9dde4-35b6-4c5a-88ef-16f2776da870","cardType":"basic","points":1,"front":"Write the ionic equation for how an ethanoic acid buffer removes added $H^{+}$ ions.","back":"$$CH_3COO^-(aq) + H^+(aq) \\to CH_3COOH(aq)$","mcqOptions":[{"text":"$$CH_3COO^-(aq) + H^+(aq) \\to CH_3COOH(aq)$","correct":true,"explanation":"Added hydrogen ions react with ethanoate ions, the conjugate base, to form weak ethanoic acid. This removes most of the added $H^+$ and limits the pH decrease."},{"text":"$$CH_3COOH(aq) + H^+(aq) \\to CH_3COOH_2^+(aq)$","correct":false,"explanation":"This protonates ethanoic acid rather than using the buffer’s ethanoate ions as the main hydrogen ion acceptor. The correct reaction is $CH_3COO^-(aq) + H^+(aq) \\to CH_3COOH(aq)$."},{"text":"$$CH_3COOH(aq) + H^+(aq) \\to CH_3COO^-(aq) + H_2(aq)$","correct":false,"explanation":"Added hydrogen ions do not convert ethanoic acid into ethanoate while producing hydrogen gas. Ethanoate ions accept the added $H^+$ to form $CH_3COOH(aq)$."},{"text":"$$CH_3COO^-(aq) + OH^-(aq) \\to CH_3COOH(aq) + O^{2-}(aq)$","correct":false,"explanation":"This uses hydroxide instead of the added hydrogen ion and introduces an implausible oxide product. Added $H^+$ is removed when ethanoate ions form ethanoic acid."}]},{"id":"714eb86b-5d89-458e-8ff0-0d921872662c","cardType":"basic","points":1,"front":"Write the ionic equation for how an ethanoic acid buffer removes added $OH^{-}$ ions.","back":"$$CH_3COOH(aq) + OH^-(aq) \\to CH_3COO^-(aq) + H_2O(l)$","mcqOptions":[{"text":"$$CH_3COOH(aq) + OH^-(aq) \\to CH_3COO^-(aq) + H_2O(l)$","correct":true,"explanation":"Ethanoic acid donates a proton to added hydroxide ions, producing ethanoate ions and water. Removing $OH^-$ prevents a large increase in pH."},{"text":"$$CH_3COO^-(aq) + OH^-(aq) \\to CH_3COOH(aq) + H_2O(l)$","correct":false,"explanation":"Both ethanoate and hydroxide ions are bases, so this equation incorrectly treats ethanoate as a proton donor. Ethanoic acid reacts with added $OH^-$ to form ethanoate and water."},{"text":"$$CH_3COOH(aq) + H^+(aq) \\to CH_3COO^-(aq) + H_2O(l)$","correct":false,"explanation":"The added ion is hydroxide, not hydrogen ion, and ethanoic acid cannot produce water without accepting $OH^-$. The correct reaction neutralises hydroxide with ethanoic acid."},{"text":"$$CH_3COOH(aq) + OH^-(aq) \\to CH_3COO^-(aq) + H_2(g)$","correct":false,"explanation":"Neutralisation produces water, not hydrogen gas. Ethanoic acid transfers its acidic proton to hydroxide, giving $CH_3COO^-(aq)$ and $H_2O(l)$."}]},{"id":"f498f974-e589-430a-ad10-11ee46120abe","cardType":"basic","points":2,"front":"Why is a weak acid solution on its own not an effective buffer?","back":"It contains insufficient conjugate base to react with added acid.","mcqOptions":[{"text":"It contains insufficient conjugate base to react with added acid.","correct":true,"explanation":"A weak acid solution contains some conjugate base, but usually not enough to remove significant added acid. An effective acidic buffer needs comparable amounts of both components."},{"text":"It contains insufficient weak acid to react with added alkali.","correct":false,"explanation":"A weak acid solution generally contains plenty of weak acid to react with added hydroxide. It is ineffective because it lacks sufficient conjugate base to remove added acid."},{"text":"It contains insufficient hydrogen ions to react with added alkali.","correct":false,"explanation":"Hydrogen ions are not the required buffer component for neutralising added acid, and a weak acid solution can supply protons to added alkali. The missing component is conjugate base."},{"text":"It contains insufficient water to dilute added acid.","correct":false,"explanation":"Buffer action depends on chemical reactions, not simply dilution by water. A weak acid alone lacks enough conjugate base to react with added acid, so it cannot resist pH change effectively."}]},{"id":"3a97901b-c65b-4889-808e-436384d9b9ba","cardType":"basic","points":1,"front":"State the rearranged $K_a$ expression used to find the hydrogen ion concentration of a buffer.","back":"$$[H^+] = K_a \\times \\frac{[HA]}{[A^-]}$","mcqOptions":[{"text":"$$[H^+] = K_a \\times \\frac{[HA]}{[A^-]}$","correct":true,"explanation":"Rearranging $K_a = \\frac{[H^+][A^-]}{[HA]}$ gives $[H^+] = K_a \\times \\frac{[HA]}{[A^-]}$. The weak acid concentration is divided by the conjugate base concentration."},{"text":"$$[H^+] = K_a \\times \\frac{[A^-]}{[HA]}$","correct":false,"explanation":"This reverses the concentration ratio, a common rearrangement error. Starting from $K_a = \\frac{[H^+][A^-]}{[HA]}$, the correct expression is $[H^+] = K_a \\times \\frac{[HA]}{[A^-]}$."},{"text":"$$[H^+] = K_a + \\frac{[HA]}{[A^-]}$","correct":false,"explanation":"The equilibrium expression requires multiplication by the concentration ratio, not addition. Correct rearrangement gives $[H^+] = K_a \\times \\frac{[HA]}{[A^-]}$."},{"text":"$$[H^+] = K_a \\times \\frac{[HA]}{[A^-]^2}$","correct":false,"explanation":"Squaring the conjugate base concentration introduces an extra factor that is not present in the acid dissociation expression. Only the ratio $\\frac{[HA]}{[A^-]}$ is required."}]}]}],"examCountdown":{"examDate":"2027-05-11","paperLabel":"Paper 1"},"heading":"Buffers","title":"Buffers Flashcards","topbar":{"backHref":"/as-level/chemistry/edexcel/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"9a7a1f4c-4e59-564c-8de2-2dbcfcfbe481","walled":"$L38"}],"$L39","$L3a"]