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Questions and Answers
When a salt reacts with dilute hydrochloric acid (HCl), effervescence is observed and the evolved gas turns lime water turbid. Which acidic radical is likely present?
When a salt reacts with dilute hydrochloric acid (HCl), effervescence is observed and the evolved gas turns lime water turbid. Which acidic radical is likely present?
- Thiosulfate ($S_2O_3^{-2}$)
- Sulfite ($SO_3^{-2}$)
- Sulfide ($S^{-2}$)
- Carbonate ($CO_3^{-2}$) (correct)
A salt, when warmed with dilute HCl, releases a gas with a suffocating odor. This gas turns acidified potassium dichromate paper green, and the solution remains clear. What acidic radical does this indicate?
A salt, when warmed with dilute HCl, releases a gas with a suffocating odor. This gas turns acidified potassium dichromate paper green, and the solution remains clear. What acidic radical does this indicate?
- Sulfide ($S^{-2}$)
- Sulfite ($SO_3^{-2}$) (correct)
- Nitrite ($NO_2^{-}$)
- Chloride ($Cl^{-}$)
Upon warming a salt with dilute HCl, a suffocating odour is observed, and the acidified potassium dichromate paper turns green. The solution turns yellow due to the formation of a sulphide precipitate. Identify the acidic radical.
Upon warming a salt with dilute HCl, a suffocating odour is observed, and the acidified potassium dichromate paper turns green. The solution turns yellow due to the formation of a sulphide precipitate. Identify the acidic radical.
- Sulfite ($SO_3^{-2}$)
- Thiosulfate ($S_2O_3^{-2}$) (correct)
- Sulfide ($S^{-2}$)
- Nitrite ($NO_2^{-}$)
A salt is warmed with dilute HCl, producing a gas that smells like rotten eggs. This gas also causes blackening of lead acetate paper. What acidic radical is indicated?
A salt is warmed with dilute HCl, producing a gas that smells like rotten eggs. This gas also causes blackening of lead acetate paper. What acidic radical is indicated?
When a salt is treated with dilute HCl, brown fumes are evolved, and the solution turns faint blue. Which acidic radical is likely present?
When a salt is treated with dilute HCl, brown fumes are evolved, and the solution turns faint blue. Which acidic radical is likely present?
A salt solution gives a white precipitate with $BaCl_2$ solution that is insoluble in mineral acids. Which acidic radical is indicated?
A salt solution gives a white precipitate with $BaCl_2$ solution that is insoluble in mineral acids. Which acidic radical is indicated?
A salt solution produces a white precipitate with $BaCl_2$ that is soluble in mineral acids. Which of the following acidic radicals could be present?
A salt solution produces a white precipitate with $BaCl_2$ that is soluble in mineral acids. Which of the following acidic radicals could be present?
When a salt is treated with concentrated $H_2SO_4$, a colorless gas is evolved that gives dense white fumes when a glass rod dipped in ammonium hydroxide is brought near the mouth of the test tube. Identify the anion.
When a salt is treated with concentrated $H_2SO_4$, a colorless gas is evolved that gives dense white fumes when a glass rod dipped in ammonium hydroxide is brought near the mouth of the test tube. Identify the anion.
A salt reacts with concentrated $H_2SO_4$ to produce reddish-brown fumes. Which acidic radical is likely present?
A salt reacts with concentrated $H_2SO_4$ to produce reddish-brown fumes. Which acidic radical is likely present?
A salt treated with concentrated $H_2SO_4$ evolves violet vapors, which turn starch paper blue. What acidic radical is indicated?
A salt treated with concentrated $H_2SO_4$ evolves violet vapors, which turn starch paper blue. What acidic radical is indicated?
When a salt is heated with concentrated $H_2SO_4$ and copper turnings, dense brown fumes evolve, and the solution turns faint blue. Which acidic radical is present?
When a salt is heated with concentrated $H_2SO_4$ and copper turnings, dense brown fumes evolve, and the solution turns faint blue. Which acidic radical is present?
A concentrated salt solution treated with $AgNO_3$ produces a white precipitate that is soluble in dilute ammonia solution. Which anion is confirmed by this test?
A concentrated salt solution treated with $AgNO_3$ produces a white precipitate that is soluble in dilute ammonia solution. Which anion is confirmed by this test?
A salt solution treated with $AgNO_3$ gives a pale yellow precipitate that is soluble in dilute $HNO_3$. Which anion is indicated?
A salt solution treated with $AgNO_3$ gives a pale yellow precipitate that is soluble in dilute $HNO_3$. Which anion is indicated?
A salt solution reacts with $AgNO_3$ to form a yellow precipitate that is soluble in ammonia solution. What anion is likely present?
A salt solution reacts with $AgNO_3$ to form a yellow precipitate that is soluble in ammonia solution. What anion is likely present?
When testing for sulfate ions, a white precipitate of barium sulfate is formed with $BaCl_2$. What reagent is used in a confirmatory test to produce a white precipitate of $Ag_2SO_4$?
When testing for sulfate ions, a white precipitate of barium sulfate is formed with $BaCl_2$. What reagent is used in a confirmatory test to produce a white precipitate of $Ag_2SO_4$?
A phosphate ion ($PO_4^{3-}$) is confirmed by the formation of a yellow precipitate, soluble in $NH_4OH$, upon addition of which reagent?
A phosphate ion ($PO_4^{3-}$) is confirmed by the formation of a yellow precipitate, soluble in $NH_4OH$, upon addition of which reagent?
Which reagent, when added to a borate solution, will produce a white precipitate of $AgBO_2$ in a confirmatory test?
Which reagent, when added to a borate solution, will produce a white precipitate of $AgBO_2$ in a confirmatory test?
In the flame test, which cation imparts a brick-red color to the flame?
In the flame test, which cation imparts a brick-red color to the flame?
In qualitative analysis, which reagent is commonly used to precipitate Group I cations ($Pb^{++}$, $Ag^{+}$, $Hg_2^{++}$) as chlorides?
In qualitative analysis, which reagent is commonly used to precipitate Group I cations ($Pb^{++}$, $Ag^{+}$, $Hg_2^{++}$) as chlorides?
A solution of lead nitrate reacts with dilute HCl to form a white precipitate of lead chloride ($PbCl_2$). What happens to this precipitate when the solution is heated?
A solution of lead nitrate reacts with dilute HCl to form a white precipitate of lead chloride ($PbCl_2$). What happens to this precipitate when the solution is heated?
Which reagent is used to confirm the presence of $Mn^{2+}$ ions by forming a white precipitate of manganous hydroxide ($Mn(OH)_2$)?
Which reagent is used to confirm the presence of $Mn^{2+}$ ions by forming a white precipitate of manganous hydroxide ($Mn(OH)_2$)?
Nickel ions ($Ni^{2+}$) react with ammonium hydroxide ($NH_4OH$) and dimethylglyoxime to form which distinctive precipitate?
Nickel ions ($Ni^{2+}$) react with ammonium hydroxide ($NH_4OH$) and dimethylglyoxime to form which distinctive precipitate?
In testing for chromic ions ($Cr^{3+}$), the addition of sodium peroxide ($Na_2O_2$) results in what observable change?
In testing for chromic ions ($Cr^{3+}$), the addition of sodium peroxide ($Na_2O_2$) results in what observable change?
Aluminum ions ($Al^{3+}$) react with sodium hydroxide (NaOH) to form a white precipitate. What is the formula of this precipitate?
Aluminum ions ($Al^{3+}$) react with sodium hydroxide (NaOH) to form a white precipitate. What is the formula of this precipitate?
For ferrous ions ($Fe^{2+}$), identify the resulting color when potassium ferricyanide ($K_3[Fe(CN)_6]$) is added.
For ferrous ions ($Fe^{2+}$), identify the resulting color when potassium ferricyanide ($K_3[Fe(CN)_6]$) is added.
In testing for ferric ions ($Fe^{3+}$), reaction with potassium ferrocyanide ($K_4[Fe(CN)_6]$) results in which color precipitate?
In testing for ferric ions ($Fe^{3+}$), reaction with potassium ferrocyanide ($K_4[Fe(CN)_6]$) results in which color precipitate?
Identify the confirmatory test for ammonium ions ($NH_4^+$).
Identify the confirmatory test for ammonium ions ($NH_4^+$).
What color does the flame turn when potassium ions ($K^+$) are introduced to a flame?
What color does the flame turn when potassium ions ($K^+$) are introduced to a flame?
Which cation gives a golden yellow color to the flame in a flame test?
Which cation gives a golden yellow color to the flame in a flame test?
Flashcards
Carbonate/Bicarbonate Test
Carbonate/Bicarbonate Test
With dilute HCl, effervescence occurs, and CO2 gas is released, turning lime water turbid.
Sulfite Ion (SO3-2) Test
Sulfite Ion (SO3-2) Test
SO2 gas with a suffocating odor is released, turning acidified potassium dichromate paper green in a clear solution.
Thiosulfate Ion (S2O3-2) Test
Thiosulfate Ion (S2O3-2) Test
SO2 gas with a suffocating odor evolves, turning acidified potassium dichromate paper green; solution turns yellow due to sulphide ppt.
Sulfide Ion (S-2) Test
Sulfide Ion (S-2) Test
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Nitrite Ion (NO3-) Test
Nitrite Ion (NO3-) Test
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Chloride Ion (Cl-) Test
Chloride Ion (Cl-) Test
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Bromide Ion (Br-) Test
Bromide Ion (Br-) Test
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Iodide Ion (I-) Test
Iodide Ion (I-) Test
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Nitrate Ion (NO3-) Test
Nitrate Ion (NO3-) Test
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Sulfate Ion (SO42-) Test
Sulfate Ion (SO42-) Test
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Phosphate/Metaborate Test
Phosphate/Metaborate Test
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Chloride Ion Confirmation
Chloride Ion Confirmation
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Bromide Ion Confirmation
Bromide Ion Confirmation
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Iodide Ion Confirmation
Iodide Ion Confirmation
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Nitrate Ion Confirmation
Nitrate Ion Confirmation
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Carbonate Ion Test
Carbonate Ion Test
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Sulfide Ion Test
Sulfide Ion Test
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Sulfite Ion Test
Sulfite Ion Test
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Nitrite Ion Test
Nitrite Ion Test
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Barium Ion Confirmation
Barium Ion Confirmation
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Barium Flame Test
Barium Flame Test
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Strontium Flame Test
Strontium Flame Test
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Calcium Flame Test
Calcium Flame Test
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Ammonium Ion Test
Ammonium Ion Test
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Potassium Ion Test
Potassium Ion Test
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Potassium Flame Test
Potassium Flame Test
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Sodium Flame Test
Sodium Flame Test
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Chromic Ion (Cr3+)
Chromic Ion (Cr3+)
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Antimonious ion Sb3+
Antimonious ion Sb3+
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Study Notes
Acidic Radicals with diluted HCl
- Effervescence on cold indicates CO3-2 or HCO3-, confirmed by lime water turning turbid due to CO2 gas evolution.
- Suffocating odour of SO2 gas on warming suggests SO3-2, confirmed by acidified potassium dichromate paper turning green, with a clear solution.
- Suffocating odour of SO2 on warming indicates S2O3-2, confirmed by acidified potassium dichromate paper turning green, solution turning yellow due to sulphide precipitate (S + SO3-2).
- H2S gas evolves on warming, smelling like rotten eggs, indicates S-2, further confirmed by blackening of lead acetate paper.
- Brown fumes and faint blue solution indicate NO3- as NO2 gas evolves.
- An acidic radical is not from Group I if no gas evolves; it may be from Group II or III.
Acidic Radicals with concentrated H2SO4
- Colourless HCl gas evolves, forming dense white fumes with ammonium hydroxide, indicating Chloride (Cl-).
- Reddish-brown gases (HBr and Br2) evolving and solution turning reddish-brown indicates Bromide (Br-).
- Violet vapours of I2 and HF that turn starch paper blue, with violet sublimate on the tube sides, indicate Iodide (I-). Sulfur may precipitate on the tube walls.
- Brown fumes of NO2 evolving that become dense with copper turnings, and the solution turns faint blue, indicating Nitrate (NO3-).
- An acidic radical isn't from Group II but maybe Group III if no gas evolves.
Acidic Radicals with Salt solution and BaCl2
- White precipitate insoluble in mineral acids indicates SO42- (barium sulphate).
- White precipitate soluble in mineral acids indicates PO4-3 (barium phosphate) or B4O7-2 (barium metaborate).
Group III - Acidic Radical Tests
- Group III acidic radicals include SO4-2, PO4-3, and B4O7-2.
Test for Sulphate Ions (SO42-)
- Salt solution with barium chloride (BaCl2) produces a white precipitate of barium sulphate, insoluble in mineral acids.
- Concentrated salt solution with AgNO3 gives a white precipitate (Ag2SO4) as a confirmatory test.
- Salt solution with lead acetate results in a white precipitate soluble in ammonium acetate-NaOH.
Test for Phosphate Ion (PO43-)
- Salt solution with barium chloride (BaCl2) gives a white precipitate of barium phosphate soluble in mineral acids.
- Salt solution with AgNO3 results in a yellow precipitate soluble in NH4OH as a confirmatory test.
- Salt solution with FeCl3 results in a yellow precipitate of FePO4 soluble in mineral acids.
- Salt solution with excess ammonium molybdate and conc HNO3 and heat gives canary yellow precipitate.
Test for Borate Ions (B4O72-)
- Salt solution with barium chloride (BaCl2) yields a white precipitate of Ba(BO2)2, soluble in mineral acids.
- A concentrated salt solution with AgNO3 results in a white precipitate of AgBO2 for confirmation.
- Pink color disappears upon adding glycerol to the salt solution with ph-ph.
Group II - Acidic Radical Tests
- Group II acidic radicals include Cl-, Br-, I-, and NO3-.
Test for Chloride Anion (Cl-)
- HCl evolves when solid and concentrated H2SO4 are warmed, forming white ammonium chloride clouds when a glass rod with ammonia solution is near.
- Salt solution with AgNO3 forms a white precipitate of AgCl soluble in dilute ammonia solution for confirmation.
- Concentrated salt solution with lead acetate produces a white precipitate of lead chloride soluble in hot water.
Test for Bromide Anion (Br-)
- Reddish-brown vapours of Br2 and HBr evolve upon warming solid and concentrated H2SO4, turning the solution reddish-brown.
- Salt solution with AgNO3 forms a pale yellow precipitate soluble in dilute HNO3 for confirmation.
- Salt solution with lead acetate yields a white precipitate soluble in boiling water.
Test for Iodide Anion (I-)
- Solid with concentrated H2SO4 when warmed, violet vapours of I2 evolve; starch paper turns blue.
- Salt solution with AgNO3 forms a yellow precipitate soluble in ammonia solution for confirmation.
- Salt solution with HgCl2 yields a scarlet red precipitate of mercuric iodide soluble in excess KI.
Test for Nitrate Anion (NO3-)
- Solid with concentrated H2SO4 and heat produces brown fumes of NO2; the solution acquires a blue color.
- Salt solution with AgNO3 forms pale yellow precipitate for confirmation.
- Salt solution with FeSO4 and concentrated H2SO4 forms a brown ring.
Group I - Acidic Radical Tests
- Group I acidic radicals include CO32-, HCO3-, S2-, SO32-, S2O32-, and NO3-.
- The group reagent used is dilute HCl.
Test for Carbonate Ion (CO32-) and Bicarbonate (HCO3-)
- Effervescence with a colorless and odorless gas indicates carbonate ions' presence. Lime water turns milky due to CaCO3 formation.
- Na2CO3 + HCl -> NaCl + H2O + CO2
- Ca(OH)2 + CO2 -> CaCO3 + H2O
- Salt solution with MgSO4 results in a white precipitate on cold (MgCO3,) and boiling the solution white precipitate forms Mg(CHO3)2
- Salt solution with HgCl2 gives a reddish-brown precipitate on cold and boiling it reddish-brown precipitate forms.
- Salt solution with BaCl2 yields a white precipitate (BaCO3).
- Salt solution with AgNO3 give white precipitate (Ag2CO3).
Test for Sulfide Ion (S2-)
- With warm dilute HCl, a sulfide gives hydrogen sulfide gas that smells like rotten eggs.
- A piece of filter paper dipped in lead acetate solution turns black due to lead sulfide formation.
- Na2S + HCl -> NaCl + H2S
- (CH3COO)2Pb + H2S -> PbS + 2CH3COOH
- Salt solution + Na4[Fe(CN)5NOS], a purple complex forms.
- Salt solution + AgNO3 forms a black precipitate (Ag2S).
- Salt solution + lead acetate forms a black precipitate of lead sulfide (PbS).
Test for Sulfite Ion (SO32-)
- On treating Sulfite with warm dil. HCl, SO2 gas evolves, suffocating with the smell of burning Sulphur.
- The gas turns potassium dichromate paper acidified with dil. H2SO4 to green, and the solution becomes clear.
- Na2SO3 + HCl -> NaCl + H2O + SO2
- K2Cr2O7 + H2SO4 + 3SO2 -> K2SO4 + Cr2(SO4)3 + H2O
Confirmatory Tests for Sulfite Ion (SO32-)
- Salt solution with barium chloride solution (BaCl2) will produce a white precipitate of barium sulfite (BaSO3).
- The added drops of acidified potassium permanganate solution will lead to decolourisation.
- Lead Sulphite will produce a white ppt of lead soluble in cold dilute HNO3 if Salt solution +lead acetate is added.
Test for Thiosulphate Ion (S2O32-)
- On treating Sulphite with warm dil. HCl, SO2 gas evolves, having a strong suffocating smell of burning sulphur.
- Na2S2O3 + HCl -> NaCl + S + SO2;
- The potassium dichromate paper acidified with dil. H2SO4 turns to green, and the solution turns yellow.
Confirmatory Tests for Thiosulphate Ion (S2O32-)
- A white precipitate of barium thiosulphate forms when the Salt solution + barium is treated with chloride solution
- White ppt of lead thiosulphate (PbS2O3) if salt solution +Lead acetate, and on boiling, a black ppt is obtained.
- Dark violet coloration soon disappears after short time, on adding Salt solution +Ferric chloride solution (FeCl3).
Test for Nitrite Ion (NO2-)
- Reddish-brown fumes of NO2 gas evolve when a solid nitrite with dil. HCl and warming is being treated. Solution becomes pale blue.
- Confirmatory Tests:
- No precipitate if with Salt solution + barium chloride solution.
- White ppt is formed if Salt solution + AgNO3 - Brown ring is formed (FeSO4·NO) if Salt solution + FeSO4+ conc H2SO4
- Decolourisation happens if Salt solution + KMnO4+ drop of conc H2SO4
Group V - Basic Radical Tests
- Basic radicals in Group V include Ba2+, Sr2+, and Ca2+.
Test for Barium Ion (Ba2+)
- Barium chloride (NH4Cl ) + ammonium hydroxide (NH4OH) + ammonium carbonate (NH4)2 CO3 when added to the Salt solution, it produces White ppt of barium carbonate (BaCO3)
Confirmatory Tests for Barium
- Yellow ppt forms that are soluble in mineral acids (BaCrO4) after Salt solution+ potassium chromate (K2CrO4)
- Salt colors flame yellowish green when Flame test applied
- White ppt for Barium oxalate. (BaC2O4) if 5 drops of Salt solution +4 drops Ammonium oxalate. Salt colors flame yellowish greenif Flame test
Test for Strontium Ion [Sr2+]
- White ppt Strontium of Ammonium carbonate (SrCO3) when Salt chloride when mixed with ammonium chloride (NH4Cl ) + ammonium hydroxide (NH4OH) + ammonium carbonate (NH4)2 CO3 :
- White ppt of strontium oxalate (SrC2O4) after adding 6 drops of Salt solution +6 drops of Ammonium. Salt colors flame crimson color with Flame test
Test for Calcium Ion
- white precipitate of Calcium carbonate(CaCO3) when adding Salt solution + ammonium chloride(NH4Cl ) + ammonium hydroxide (NH4OH) + ammonium carbonate (NH4)2 CO3 : _Salt colors the flame brick- red color when exposed to Flame test _
-
*White ppt Caicium oxalate* (CaC2O4) is the White ppt Ammonium added to Salt solution
Group VI - Basic Radical Tests
Group VI: includes 3 Basic radicals (NH4+ , K+ , Mg2+ , Na+)
Test of Ammonium Ion [NH4+]
When (NaOH) solid is added to Salt solution boiling: NH3 gas evolved when exposed to glass rod wetted by HCl, it forms white fumes.
- Yellow ppt forms of ammonium cobalt nitrite (NH4)3[Co(NO2)6] when adding Salt Solution + ammonium cobalt nitrite Na3[Co(NO2)6].
Test of Potassium Ion [K+]
- When add Salt solution +sodium cobalt nitrite Na3[Co(NO2)6]-: it produces Yellow ppt potassium cobalt of nitrite K3[Co(NO2)6] Salt colors the flame violet color because of Flame test.
Test of Magnesium Ion[Mg2+]
- Salt solution +NH4Cl +NH4OH + Disodium hydrogen phosphate(Na2HPO4) it produces White ppt of Ammonium magnesium phosphate Mg (NH4)PO4
- Salt solution + NaoH- It white precipitate is forms magnesium Hydroxide Mg(OH)2
Test of Sodium Ion [Na+]
When Flame test applied is, Salt colors and flame golden-yellow
Group III
Group III, is a test of these 4 Cations Cr3+, Al3+ , Fe2+,Fe3+'
- Group reagent: Buffer (NH4Cl + NH4OH)
- Precipitation Form: As hydroxide
1 Test of Chromic ion Cr3+
SolnChromic of nitrate +buffer: forms green Pale CrCl3 + 3NH4OH -> Cr(OH)3 + 3NH4Cl
- with Soln+ and Na2O2 _ Sodium Peroixde_, it form Yellow Solution with(CrO4)2- withSoln + NaOH -> it forms Pale green Cr(OH)3
Test for Aluminium Ion Al3+
- Soln Aluminum of nitrate + buffer produces white Gelatinous Al(OH)3.
- Al3+ +3NH4OH -> Al(OH)3+3NH4* -soln + NaOH -> Aluminium white precipitate (Al(OH)3 )
Test of Ferrous Ion Fe2+
Soln Ferrous of ammonium and sulphate + buffer soln: it green precipitation of Fe(OH)2
(Fe2+)
-
Soln4K[Fe(CN)6] ->* it produced Pale precipitate blue Fe2[Fe(CN)6]4 Potassium+ Ferrocyanide
-
Soln + K3[Fe(CN)6]4-potassium:: forms Dark precipitate blue Fe3[Fe(CN)6]2
###- 4 Test for Ferric ion Fe3+ the soln of Ferric Chloride + buffer soln forms a Brown precipitate Fe(OH)3
- Soln NaOH -> = Brown precipitate *The Soln3+_ K3[Fe(CN)6]2_ = creates Dark precipitate blue Fe(CN)62_
Cations Radicals Basic Group 4
(Mn2+, Ni2+, Co2+, Zn2+)
test for Manganous basic Ion Mn2+
- Salt + ammonium: solutions with, chlorides chloride (NH4Cl ) + ammonium hydroxide (NH4OH) : plus Hydrogen and. generates (H2S) precipitate . Manganous (MnS) sulfide Salt + ammonium: solutions with, chlorides chloride (NH4Cl ) + ammonium hydroxide (NH4OH) plus and Hydrogen generates sulphide (H2S) precipitate Manganous (MnS) sulfide- Confirmatory tests with:[Mn2+ ] Solution Sodium results with ppt white and Mn2. reagent extra the to insoluble, hydroxide Sodium
Test for Ions NickelBasic Radical Ni2+
- Salt + ammonium: solutions with, chlorides chloride (NH4Cl ) + ammonium hydroxide (NH4OH) * Hydrogen Sulphide (H2S)* ::ppt Nickel blck, (NiS); solution aqua that soluble and acid mineral which to soluble
- SolutionSodium -> White* the .reagent, of and excess to insoluble, Hydroxide Nickel DMG with + Ammonia solution -> that solution ammonia plus the DMG
- that precipitate glyoxine Nickel* Ni[ DMG
###: Test for cobaltbasic Ion Co2+ Chloride that: solution ammonia that plus that Chloride (NH4Cl) + ammonium( NH4OH) * Sulphidethat Hydrogen*(H2S :: solution aqua acid to which soluble, chloride black cobalt with test .
Confirmatory tests: [co2+
- Sodium that with solution the salt solution ammonia and Solution the that heat from - NaOH. Hydroxide the Cobalt ppt turns bluest change - NH4SCN. alcohol drop to + solution the to ,solution to which due, the, Sulphur* ###. *H, . test zinc + ION Zn2
for zinkk test tests tests and test -
- Solution + chloride: solutions chloride (NH4Cl) +ammonium- Hydroxide :( that Hydroxide and Hydroxide ammonia Ammonium sulphide Hydrogen test which ppt Zinc + which, that precipitate that test
[SOLUTION +Na2, is ppt whiter, whiter whiter with + chloride :solution + the ( ammonium ( nh4cl + , to hydrooxihide
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