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Questions and Answers
Match the silver halides with their respective colors:
Match the silver halides with their respective colors:
AgCl = White AgBr = Pale yellow AgI = Yellow AgF = Colorless
Match the silver halides with their solubility in dilute ammonia:
Match the silver halides with their solubility in dilute ammonia:
AgCl = Insoluble AgBr = Slightly soluble AgI = Insoluble
Match the following reactions with their resulting products:
Match the following reactions with their resulting products:
Ag + Br- = AgBr Ag + I- = AgI Ag + Cl- = AgCl AgBr + I- = AgI + Br-
Match the silver halides with their relative solubility in water:
Match the silver halides with their relative solubility in water:
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Match the silver halides with their corresponding complex formation in ammonia:
Match the silver halides with their corresponding complex formation in ammonia:
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Match the following reactions with their resulting products:
Match the following reactions with their resulting products:
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Match the following silver halides with their solubility characteristics:
Match the following silver halides with their solubility characteristics:
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Match the following reagents with their corresponding reactions:
Match the following reagents with their corresponding reactions:
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Match the following indicators with their usage:
Match the following indicators with their usage:
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Match the following statements about silver halides with their correct description:
Match the following statements about silver halides with their correct description:
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Study Notes
Halide Reactions
- Reactions of halide ions can be categorized as wet and dry reactions.
- Wet reactions refer to reactions occurring in solution with reagents such as silver nitrate (AgNO3).
- Dry reactions involve heating solid samples with concentrated sulfuric acid (H2SO4).
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Silver nitrate (AgNO3) reactions with halides produce precipitates that vary in color and solubility:
- Fluoride (F-) does not form a precipitate with AgNO3 because silver fluoride (AgF) is soluble in water.
- Chloride (Cl-) forms a white precipitate of silver chloride (AgCl), insoluble in nitric acid but soluble in potassium cyanide (KCN) and sodium thiosulfate (Na2S2O3). AgCl is also soluble in dilute ammonia solution, forming a silver amine complex.
- Bromide (Br-) forms a pale yellow precipitate of silver bromide (AgBr), sparingly soluble in dilute ammonia but readily soluble in concentrated ammonia.
- Iodide (I-) forms a yellow precipitate of silver iodide (AgI), insoluble in dilute, very slightly soluble in concentrated ammonia.
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AgCl, AgBr, and AgI exhibit a periodicity in their properties:
- Color: AgCl is white, AgBr is pale yellow, and AgI is yellow.
- Solubility in water: AgCl is most soluble, AgBr is less soluble, and AgI is least soluble.
- Solubility in dilute ammonia: AgCl is soluble, AgBr is slightly soluble, and AgI is insoluble.
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Reactions with Ferric Chloride (FeCl3):
- In the presence of ferricyanide ([Fe(CN)6]3-), FeCl3 produces a brown color in solution due to the formation of the non-ionized ferric-ferricyanide complex.
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Reactions with Ferrous Sulfate (FeSO4):
- Ferrous sulfate reacts with cyanide (CN-) to form a yellow-brown precipitate, which is a ferrocyanide.
- Ferrocyanide reacts with ferrous sulfate to form a white precipitate of potassium ferrous ferrocyanide.
- Ferricyanide reacts with ferrous sulfate to form a blue precipitate, known as Turnbull's blue, which is similar in composition to Prussian blue, but with a different distribution of iron oxidation states.
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Dry reactions with concentrated sulfuric acid (H2SO4):
- Chloride (Cl-) reacts with H2SO4 to produce fumes of hydrogen chloride (HCl) with a characteristic pungent odor.
- Bromide (Br-) reacts with H2SO4 to produce a mixture of hydrogen bromide (HBr) and bromine (Br2), which can be identified by their characteristic brown color, especially upon warming.
- Iodide (I-) reacts with H2SO4 to generate iodine (I2) vapor, which is readily identified by its violet color.
- Cyanogen anions are highly toxic and include cyanide (CN-), thiocyanate (SCN-), ferrocyanide ([Fe(CN)6]4-), and ferricyanide ([Fe(CN)6]3-).
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All cyanogen anions form complexes:
- Double cyanides: Examples include argentocyanide complex (Ag(CN)2)-.
- Complex cyanides: Examples include ferrocyanide ([Fe(CN)6]4-) and ferricyanide ([Fe(CN)6]3-).
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Reactions of cyanogen anions:
- Dilute HCl: Cyanides react with dilute HCl to produce hydrogen cyanide (HCN) gas, which has a characteristic bitter almond odor.
- Concentrated H2SO4: Cyanogen anions can be identified based on their reactions with concentrated H2SO4.
Cyanogen Anions - Testing & Identification
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Specific tests for cyanogen anions:
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HCN gas identification:
- Ammonium polysulphide: HCN can be converted to thiocyanate (SCN-) by reacting with ammonium polysulphide, which can then be identified by a blood-red color with FeCl3 solution acidified with dilute HCl.
- AgNO3 solution: HCN can be identified by reacting with AgNO3 solution, which produces a white precipitate of AgCN, insoluble in dilute HNO3, but soluble in ammonia solution.
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HCN gas identification:
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Wet reactions with cyanogen anions:
- Silver nitrate (AgNO3): The reaction with AgNO3 reagent yields a precipitate that is insoluble in dilute HNO3, but soluble in ammonia solution.
- Barium chloride (BaCl2): This test is not specific to cyanogen anion.
- Ferric chloride (FeCl3) and Ferrous sulfate (FeSO4): These reagents are used to differentiate between ferrocyanide and ferricyanide.
- Cobalt nitrate (Co(NO3)2): This reagent is not specific to cyanogen anion.
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Dry reactions with cyanogen anions:
- Dilute HCl: Cyanide (CN-) reacts with dilute HCl to produce HCN gas.
- Concentrated H2SO4: Cyanogen anions react with concentrated H2SO4, but the specific reactions vary depending on the anion.
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Description
Explore the fascinating world of halide reactions! This quiz focuses on both wet and dry reactions involving halide ions and reactions with silver nitrate. Test your knowledge on precipitate formation and the solubility of different halide compounds.
