Why Correct: Baking soda reacts with acids to produce carbon dioxide gas. This gas forms bubbles that cause dough to rise during baking.
Distractor Analysis: Oxygen supports combustion but is not produced in this reaction. Hydrogen is a flammable gas generated in some metal-acid reactions. Nitrogen is an inert gas that does not form from baking soda-acid reactions.
Takeaway: The chemical reaction is NaHCO3 + H+ -> Na+ + H2O + CO2, where carbon dioxide is the leavening agent.

Why Correct: Sodium carbonate decahydrate (Na2CO3·10H2O) is washing soda. It softens hard water by removing calcium and magnesium ions.
Distractor Analysis: Sodium hydrogen carbonate is baking soda used in cooking. Calcium carbonate is limestone used in construction and antacids. Magnesium hydroxide is milk of magnesia used as an antacid.
Takeaway: Washing soda loses water molecules on heating to become anhydrous sodium carbonate (Na2CO3), known as soda ash.

Why Correct: Washing soda is sodium carbonate decahydrate with the chemical formula Na2CO3·10H2O. It contains ten water molecules of crystallization.
Distractor Analysis: NaHCO3 is baking soda or sodium hydrogen carbonate. NaOH is sodium hydroxide or caustic soda. NaCl is common salt or sodium chloride.
Takeaway: Baking soda (NaHCO3) loses water and carbon dioxide on heating to form washing soda (Na2CO3) through the reaction 2NaHCO3 -> Na2CO3 + H2O + CO2.

Why Correct: Phenolphthalein is colorless in acidic solutions and turns pink in basic solutions with pH above 8.3.
Distractor Analysis: Litmus paper turns red in acids and blue in bases. Methyl orange shows red color in acids and yellow in bases. Turmeric paper turns red in basic solutions.
Takeaway: Universal indicator shows different colors across the pH scale - red for strong acids, green for neutral, and violet for strong bases.

Why Correct: Acids typically have a sour taste (like citric acid in lemons) and bases have a bitter taste with a soapy or slippery feel (like sodium hydroxide). This is a fundamental property distinguishing acids from bases.
Distractor Analysis: Option A reverses the properties of acids and bases. Option C incorrectly gives acids and bases the same taste. Option D gives both acids and bases bitter taste, which is incorrect.
Takeaway: The sour taste of acids and bitter taste with soapy feel of bases are basic sensory properties that help identify these substances in everyday contexts.

Why Correct: Gastric juice contains hydrochloric acid with a pH range of 1.5-3.5.
Distractor Analysis: Vinegar has a pH range of 2.4-3.4. Milk maintains a pH of 6.5-6.7. Human blood has a tightly regulated pH of 7.35-7.45.
Takeaway:

Why Correct: Lime water is specifically defined as a saturated aqueous solution of calcium hydroxide (Ca(OH)₂), which is a base with pH typically between 10.5-12.4.
Distractor Analysis: Lemon juice contains citric acid, human blood maintains a slightly basic pH through buffering systems, and antacids typically contain bases like magnesium hydroxide or aluminum hydroxide.
Takeaway: Lime water is chemically distinct from lime juice (which is acidic) and is commonly used in laboratory tests for carbon dioxide detection.

Why Correct: Human blood maintains a pH range of 7.35-7.45, which is slightly alkaline, due to bicarbonate buffer systems that regulate acid-base balance.
Distractor Analysis: Lime water (calcium hydroxide solution) has pH 10.5-12.4, antacids like magnesium hydroxide have pH 10-11, and lemon juice contains citric acid with pH around 2.2-2.4, making it acidic.
Takeaway: Biological fluids like blood have tightly regulated pH ranges, while common household substances can vary widely in acidity or alkalinity.

Why Correct: Baking soda solution is sodium bicarbonate dissolved in water, creating a basic solution with pH around 8.3. Phenolphthalein turns pink in basic solutions.
Distractor Analysis: Vinegar contains acetic acid with pH 2.4-3.4. Lemon juice contains citric acid with pH around 2.2-2.4. Milk has pH 6.5-6.7, slightly acidic.
Takeaway: Litmus paper turns red in acids and blue in bases, while methyl orange shows red in acids and yellow in bases.

Why Correct: Arrhenius theory defines bases as substances that release hydroxide ions (OH⁻) when dissolved in water.
Distractor Analysis: Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. Arrhenius theory defines acids as substances that release hydrogen ions (H⁺) in aqueous solution.

Why Correct: Fluoride ions replace hydroxide ions in hydroxyapatite to form fluorapatite. Fluorapatite is more resistant to acid attack from oral bacteria than hydroxyapatite.
Distractor Analysis: Calcium carbonate is a common abrasive and basic compound in toothpaste that helps remove plaque. Sodium bicarbonate serves as a mild abrasive and neutralizer of acids in toothpaste. Calcium phosphate is a general term for phosphate salts of calcium found in bones and teeth.
Takeaway: Hydroxyapatite has the chemical formula Ca10(PO4)6(OH)2, while fluorapatite has the formula Ca10(PO4)6F2.

Why Correct: Johannes Bronsted and Thomas Lowry independently proposed the proton transfer theory of acids and bases in 1923. This theory expanded upon Arrhenius's definition to include non-aqueous systems.
Distractor Analysis: Gilbert Lewis developed the electron pair theory of acids and bases in 1923, defining acids as electron pair acceptors. Svante Arrhenius proposed the ion dissociation theory in 1884, defining acids as substances that release H+ ions in water. Antoine Lavoisier was an 18th-century French chemist known for his work on combustion and the law of conservation of mass.
Takeaway: The Lewis acid-base theory is the broadest definition, encompassing substances that do not involve proton transfer, such as boron trifluoride (BF3) as a Lewis acid.

Why Correct: Oral bacteria like Streptococcus mutans ferment dietary carbohydrates to produce organic acids, primarily lactic acid. These acids dissolve the hydroxyapatite mineral structure of tooth enamel.
Distractor Analysis: Fluorapatite formation strengthens enamel against acid attack. Basic toothpaste neutralizes acids to prevent demineralization. Oxidation involves electron transfer rather than acid dissolution.
Takeaway: The critical pH for enamel demineralization is approximately 5.5, below which hydroxyapatite begins to dissolve in the acidic oral environment.

Why Correct: Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. This is the broadest definition among the three major theories.
Distractor Analysis: Arrhenius theory defines acids as substances that release H+ ions in aqueous solution and bases as substances that release OH- ions. Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Ostwald theory relates to acid strength and dissociation constants.
Takeaway: Arrhenius theory only applies to aqueous solutions, while Bronsted-Lowry theory extends to non-aqueous systems, and Lewis theory covers even more reactions including coordination compounds.

Why Correct: Glacial acetic acid refers to nearly pure acetic acid (99-100% concentration), while vinegar is a dilute solution containing only 5-8% acetic acid in water, along with flavor compounds from fermentation.
Distractor Analysis: Sodium nitrate (NaNO₃) is a food preservative unrelated to acetic acid concentration. Chloride of lime (Ca(OCl)₂) is bleaching powder used for disinfection. Option D is incorrect because vinegar and glacial acetic acid have vastly different acetic acid concentrations.
Takeaway: The term 'glacial' indicates high purity (99-100%) due to its freezing point just below room temperature, while vinegar's 5-8% concentration makes it suitable for culinary and cleaning uses.

Why Correct: Sodium nitrate (NaNO3) acts as a preservative in processed meats like bacon and ham. It inhibits bacterial growth, particularly Clostridium botulinum, which causes botulism.
Distractor Analysis: Dilute acetic acid is vinegar, containing 5-8% acetic acid in water. Chloride of lime is bleaching powder (Ca(OCl)2) used for disinfection and water treatment. Calcium is a metallic element (Ca) essential for bones and teeth.
Takeaway: Sodium nitrite (NaNO2) is often used alongside sodium nitrate in curing processes to maintain pink color in meats.

Why Correct: Svante Arrhenius proposed the first modern acid-base theory in 1884, defining acids as substances that dissociate in water to produce hydrogen ions (H⁺) and bases as substances that produce hydroxide ions (OH⁻).
Distractor Analysis: Johannes Brønsted (with Thomas Lowry) developed the Brønsted-Lowry acid-base theory in 1923, focusing on proton transfer. Gilbert Lewis proposed the Lewis acid-base theory in 1923, emphasizing electron pair donation and acceptance. Robert Boyle was a 17th-century chemist known for Boyle's law and early acid-base experiments, but not for modern acid-base theory.
Takeaway: Arrhenius theory laid the foundation for understanding acid-base behavior in aqueous solutions, though later theories (Brønsted-Lowry and Lewis) expanded the concepts to broader contexts.

Why Correct: Acetic acid in vinegar is produced through the fermentation of ethanol by acetic acid bacteria, specifically Acetobacter species. This biochemical oxidation process converts ethanol (C₂H₅OH) to acetic acid (CH₃COOH).
Distractor Analysis: Sodium nitrate is a preservative, not involved in vinegar production. Chloride of lime is bleaching powder used for disinfection, not fermentation. Calcium compounds may be present in some vinegar types but don't drive the ethanol-to-acetic acid conversion.
Takeaway: The fermentation process by Acetobacter is essential for vinegar production, distinguishing it from other chemical processes involving the distractors.

Why Correct: Vinegar is a dilute solution containing 5-8% acetic acid in water. Glacial acetic acid is the concentrated form with 99-100% purity.
Distractor Analysis: Both vinegar and glacial acetic acid can be produced through fermentation of ethanol by acetic acid bacteria. Vinegar typically has a pH of 2.4-3.4, making it more acidic than many solutions but still a weak acid. Vinegar contains acetic acid, not ethanol, as its primary acidic component.
Takeaway: The term 'glacial' refers to the pure acetic acid's tendency to form ice-like crystals at temperatures below 16.7°C.

Why Correct: Hydrofluoric acid (HF) reacts with silicon dioxide in glass, requiring storage in plastic containers like polyethylene or Teflon. It also causes severe tissue burns that penetrate deeply due to fluoride ion interference with calcium metabolism.
Distractor Analysis: Nitric acid (HNO₃) is a strong oxidizing acid but can be stored in glass. Hydrochloric acid (HCl) is a strong acid commonly stored in glass containers. Hydrobromic acid (HBr) is similar to HCl and does not require special plastic storage.
Takeaway: HF's unique properties necessitate specific handling precautions including plastic storage containers and immediate medical attention for exposure.

Why Correct: Nitric acid (HNO3) is a strong oxidizing acid extensively used in fertilizer production (ammonium nitrate) and explosives manufacturing (nitroglycerin, TNT). Its oxidizing nature makes it valuable for nitration reactions.Distractor Analysis: Hydrochloric acid (HCl) is used in steel pickling and PVC production but lacks strong oxidizing properties for these applications. Hydrofluoric acid (HF) is used in glass etching and petroleum refining but not typically for fertilizers/explosives. Hydrobromic acid (HBr) is used in pharmaceuticals and organic synthesis but has limited industrial use in these fields.Takeaway: HNO3's oxidizing capability distinguishes it from other mineral acids in industrial chemistry applications.

Why Correct: Hydrochloric acid (HCl) is produced by parietal cells in the stomach lining. It creates an acidic environment for pepsin activation and kills ingested microorganisms. The industrial name muriatic acid refers to impure hydrochloric acid.
Distractor Analysis: Nitric acid (HNO3) is a strong oxidizing acid used in fertilizer and explosive production. Sulfuric acid (H2SO4) is the most widely produced industrial chemical, used in batteries and fertilizer manufacturing. Hydrofluoric acid (HF) attacks glass and is used in semiconductor etching.
Takeaway: Gastric juice typically has a pH between 1.5 and 3.5 due to hydrochloric acid concentration. This highly acidic environment denatures proteins and activates digestive enzymes.

Why Correct: Hydrofluoric acid's reaction with silicon dioxide in glass makes it ideal for etching glass surfaces and cleaning silicon wafers in semiconductor manufacturing.
Distractor Analysis: Fertilizer manufacturing primarily uses sulfuric acid and nitric acid. Synthetic fiber production involves organic acids like acetic acid. Petroleum refining employs sulfuric acid and hydrofluoric acid in alkylation processes, but glass etching is the direct application of its SiO2 reaction.
Takeaway: HF is also used in the production of fluorocarbons and as a catalyst in alkylation reactions in petroleum refining.

Why Correct: The Bronsted-Lowry theory defines a base as a proton acceptor. This theory expanded the Arrhenius definition to include substances that do not contain OH⁻ ions.
Distractor Analysis: The Arrhenius theory defines a base as a substance that produces OH⁻ ions in water. The Lewis theory defines a base as an electron pair donor. Strong electrolytes are substances that dissociate completely in solution.
Takeaway: The Bronsted-Lowry theory also defines an acid as a proton donor, making acid-base reactions proton transfer processes.

Why Correct: Sodium bicarbonate (NaHCO₃), commonly known as baking soda, decomposes upon heating or reacts with acids to release carbon dioxide gas. This property makes it useful as a leavening agent in baking.
Distractor Analysis: Sodium carbonate (Na₂CO₃), or washing soda, does not produce gas under these conditions and is more alkaline. Sodium hydroxide (NaOH) is a strong base that reacts with acids but does not release CO₂. Calcium carbonate (CaCO₃) reacts with acids to produce CO₂, but this reaction is not typically associated with heating alone in the context of common household compounds.
Takeaway: The gas-producing reaction of baking soda distinguishes it from washing soda and other bases, aligning with the parent explanation's key distinction.

Why Correct: Calcium carbonate (CaCO₃) is indeed the main constituent of limestone, chalk, and marble, widely utilized in building materials and as an antacid to neutralize stomach acid.
Distractor Analysis: Sodium carbonate (Na₂CO₃) is washing soda, used in cleaning and water softening. Sodium bicarbonate (NaHCO₃) is baking soda, a leavening agent and mild antacid. Sodium hydroxide (NaOH) is caustic soda, a strong base employed in soap production and drain cleaners.
Takeaway: Recognizing the real-world applications of common compounds helps distinguish their roles in chemistry and everyday use.

Why Correct: Sodium bicarbonate (NaHCO₃) is baking soda, which releases carbon dioxide gas when heated or mixed with acids, making it an effective leavening agent in baking.
Distractor Analysis: Sodium carbonate (Na₂CO₃) is washing soda, used for cleaning and water softening. Sodium hydroxide (NaOH) is caustic soda, a strong base used in soap making. Calcium carbonate (CaCO₃) is found in limestone and antacids, but not used as a leavening agent.
Takeaway: Baking soda's ability to produce CO₂ makes it essential in baking, distinguishing it from other sodium compounds with different chemical properties and uses.

Why Correct: Svante Arrhenius proposed the Arrhenius theory in 1884, defining acids as substances that increase H⁺ ion concentration and bases as substances that increase OH⁻ ion concentration in aqueous solutions.
Distractor Analysis: Johannes Brønsted (with Thomas Lowry) developed the Brønsted-Lowry theory in 1923, focusing on proton transfer. Gilbert Lewis proposed the Lewis theory in 1923, emphasizing electron pair donation/acceptance. Robert Boyle was a 17th-century chemist who studied acids using indicators but didn't propose a formal ion-based theory.
Takeaway: Arrhenius theory laid the foundation for modern acid-base chemistry by linking properties to specific ions in solution.

Why Correct: Acid rain forms when sulfur dioxide (SO2) and nitrogen oxides (NOx) react with water vapor in the atmosphere to produce sulfuric acid (H2SO4) and nitric acid (HNO3).
Distractor Analysis: Carbon monoxide oxidation produces carbon dioxide, a greenhouse gas but not acidic. Methane combustion yields carbon dioxide and water vapor, contributing to global warming. Ozone decomposition produces oxygen and does not directly cause acid rain.
Takeaway: Acid rain typically has a pH below 5.6, damaging aquatic life, forests, and historical monuments like the Taj Mahal.

Why Correct: Hydrochloric acid (HCl) is called 'spirits of salt' because it can be produced by reacting sodium chloride (common salt) with sulfuric acid: 2NaCl + H₂SO₄ → Na₂SO₄ + 2HCl. This historical name reflects its origin from salt.
Distractor Analysis: Acetic acid is vinegar's main component. Oxalic acid is a rust remover found in plants. Aqua regia is a mixture of acids used to dissolve noble metals.
Takeaway: Common names like 'spirits of salt' often reveal chemical origins or properties, aiding in recall.

Why Correct: Oxalic acid (C2H2O4) occurs naturally in plants like spinach and rhubarb and effectively removes rust stains by forming soluble complexes with iron.
Distractor Analysis: Acetic acid is the main component of vinegar. Hydrochloric acid is a strong industrial acid also known as muriatic acid. Sulfuric acid is called the 'king of chemicals' for its extensive industrial applications.
Takeaway: Oxalic acid crystals are sometimes called 'sorrel salt' and can be toxic in large quantities, causing kidney stones.

Why Correct: Acid rain contains sulfuric acid (H2SO4) which reacts with marble's calcium carbonate (CaCO3) to form calcium sulfate (CaSO4). This calcium sulfate is water-soluble and washes away, causing erosion.
Distractor Analysis: Calcium carbonate is the original component of marble that gets destroyed in the reaction. Calcium nitrate forms when nitric acid in acid rain reacts with calcium carbonate. Calcium oxide (quicklime) is produced by heating limestone, not by acid rain action.
Takeaway:

Why Correct: Acetic acid (CH3COOH) is the main organic acid in vinegar, giving it the characteristic sour taste and pungent smell.
Distractor Analysis: Citric acid is found in citrus fruits like lemons and oranges. Tartaric acid occurs in grapes and tamarind. Lactic acid forms in sour milk and fermented foods.
Takeaway: Vinegar typically contains 4-8% acetic acid by volume, with the rest being water and trace compounds.

Why Correct: Sulfuric acid (H2SO4) earns the title 'king of chemicals' because of its massive-scale use in fertilizer production, petroleum refining, and battery manufacturing.
Distractor Analysis: Nitric acid is crucial for making explosives and fertilizers. Hydrochloric acid is widely used in pickling steel and PVC production. Phosphoric acid serves in fertilizer manufacturing and soft drinks.
Takeaway: Sulfuric acid production through the Contact Process involves catalytic oxidation of sulfur dioxide to sulfur trioxide.

Why Correct: Svante Arrhenius, a Swedish chemist, defined acids as substances that increase H+ ion concentration in water and bases as those that increase OH- ion concentration.
Distractor Analysis: Johannes Brønsted co-proposed the Brønsted-Lowry acid-base theory in 1923. Gilbert N. Lewis developed the Lewis acid-base theory focusing on electron pairs. Thomas Lowry collaborated with Brønsted on their 1923 theory.
Takeaway: Arrhenius won the 1903 Nobel Prize in Chemistry for his electrolytic dissociation theory, which underpinned his acid-base concepts.

Why Correct: Vinegar's acetic acid reacts with calcium carbonate in limescale through neutralization, producing soluble calcium acetate, water, and carbon dioxide gas.
Distractor Analysis: Oxidation reactions involve electron loss, not typical in vinegar cleaning. Reduction reactions involve electron gain, opposite of acid cleaning mechanisms. Double displacement reactions exchange ions between two compounds, not the vinegar-limescale interaction.
Takeaway: The chemical equation for this reaction is CH3COOH + CaCO3 -> Ca(CH3COO)2 + H2O + CO2, demonstrating acid-carbonate neutralization.

Why Correct: The Bronsted-Lowry theory defines acids as proton donors, exactly describing acetic acid in vinegar donating H+ ions to water.
Distractor Analysis: Arrhenius theory defines acids as substances increasing H+ concentration in water, but doesn't emphasize proton donation. Lewis theory defines acids as electron pair acceptors, not applicable to vinegar's behavior. Ostwald's dilution law describes dissociation constants of weak electrolytes, not acid definition.
Takeaway: Johannes Bronsted and Thomas Lowry independently proposed this theory in 1923, expanding acid-base concepts beyond aqueous solutions.

Why Correct: Acetic acid (CH₃COOH) is the main acidic component in vinegar, giving it its characteristic sour taste and pungent smell, produced through fermentation of ethanol by acetic acid bacteria.
Distractor Analysis: Formic acid (HCOOH) is found in ant venom and some industrial processes but not in vinegar. Citric acid is abundant in citrus fruits like lemons and oranges. Lactic acid is produced during fermentation in dairy products and muscle cells.
Takeaway: Vinegar's sour taste comes specifically from acetic acid, which distinguishes it from other organic acids like formic acid in ant venom or citric acid in fruits.

Why Correct: Acetic acid (CH3COOH) is indeed characterized by its sour taste and pungent smell, which are distinctive properties of this weak organic acid. These sensory characteristics are directly observable in vinegar, where acetic acid is the primary acidic component.
Distractor Analysis: Option B is incorrect because acetic acid is a weak acid and thus a weak electrolyte, not a strong one. Option C is misleading - while acetic acid turns blue litmus paper red, this occurs at all concentrations where it's acidic, not just high concentrations. Option D describes behavior more typical of strong mineral acids; acetic acid reacts slowly with some metals but not vigorously.
Takeaway: The sour taste and pungent smell are key identifying characteristics of acetic acid that distinguish it from other acids, particularly mineral acids which often lack these specific sensory properties.

Why Correct: Acetobacter bacteria oxidize ethanol to acetic acid in the second stage of vinegar fermentation.
Distractor Analysis: Yeast ferments sugars to produce ethanol in the first stage of vinegar production. Acetic acid does not convert to carbon dioxide in vinegar fermentation. Preservatives like sodium benzoate prevent spoilage but are not produced by Acetobacter.
Takeaway: White vinegar is typically distilled from grain alcohol, while apple cider vinegar comes from fermented apple cider.

Why Correct: Johannes Brønsted and Thomas Lowry proposed the Brønsted-Lowry theory in 1923. This theory defines acids as proton donors and bases as proton acceptors.
Distractor Analysis: Gilbert N. Lewis proposed the Lewis theory which defines acids as electron pair acceptors and bases as electron pair donors. Svante Arrhenius proposed the Arrhenius theory which defines acids as substances that increase H+ concentration and bases as substances that increase OH- concentration in aqueous solutions. Robert Boyle was a 17th-century chemist who first identified acids by their sour taste and ability to change the color of vegetable dyes.
Takeaway: The Lewis acid-base theory is the most general, explaining reactions even without proton transfer, such as the formation of coordinate covalent bonds.

Why Correct: Sodium bicarbonate (NaHCO₃) contains a hydrogen atom in its HCO₃⁻ ion, making it amphoteric - it can donate a proton (act as acid) to strong bases or accept a proton (act as base) from strong acids. Sodium carbonate (Na₂CO₃) contains CO₃²⁻ ions which only accept protons, acting purely as a base.
Distractor Analysis: Option B is incorrect because Na₂CO₃ produces more hydroxide ions through hydrolysis of CO₃²⁻. Option C is wrong as Na₂CO₃ solutions have higher pH (more basic) than NaHCO₃ at equal concentrations. Option D is false since both turn red litmus blue, being basic salts.
Takeaway: The presence of hydrogen in HCO₃⁻ gives bicarbonate its amphoteric character, allowing it to function as both Bronsted-Lowry acid and base, unlike carbonate which only acts as a proton acceptor.

Why Correct: The Arrhenius theory specifically defines acids as substances that dissociate in water to yield hydrogen ions (H⁺). This is the core definition that distinguishes Arrhenius acids from other acid-base theories.
Distractor Analysis: Option B describes Bronsted-Lowry bases (proton acceptors). Option C describes Lewis acids (electron pair acceptors). Option D describes Arrhenius bases, which dissociate to produce hydroxide ions (OH⁻).
Takeaway: Arrhenius theory provides the simplest acid-base definition based on ion production in aqueous solutions: acids give H⁺ ions, bases give OH⁻ ions.

Why Correct: The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Bicarbonate ion (HCO₃⁻) can donate a proton to form carbonate ion (CO₃²⁻) or accept a proton to form carbonic acid (H₂CO₃), demonstrating amphoteric behavior.
Distractor Analysis: Option B is incorrect because HCO₃⁻ can also accept protons. Option C is incorrect because HCO₃⁻ can also donate protons. Option D is incorrect as HCO₃⁻ actively participates in proton transfer reactions.
Takeaway: Amphoteric substances like bicarbonate can function as both acids and bases in proton transfer reactions, a key distinction of the Bronsted-Lowry theory.

Why Correct: Lewis theory defines acids as electron pair acceptors and bases as electron pair donors, expanding acid-base chemistry beyond proton transfer. In contrast, Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors.
Distractor Analysis: Option B reverses the definitions incorrectly. Option C is false because Lewis theory applies beyond aqueous solutions and proton transfer. Option D is incorrect as Lewis theory is broader, not a subset, and applies to both organic and inorganic compounds.
Takeaway: Lewis theory provides the most general definition of acids and bases, encompassing reactions that don't involve proton transfer, such as those with metal ions or boron compounds.