General Chemistry Practical 2024-2025 PDF

 Safety Rules 1. You must wear protective clothing (Lab coat, Safety glasses, Closed shoes & Gloves) 2. Never work in Lab without an instructor. 3. Never do an unauthorized experiment. 4. Never remove any reagents from its area. 5. Never taste chemicals and never...

 Safety Rules 1. You must wear protective clothing (Lab coat, Safety glasses, Closed shoes & Gloves) 2. Never work in Lab without an instructor. 3. Never do an unauthorized experiment. 4. Never remove any reagents from its area. 5. Never taste chemicals and never mouth the pipette. 6. Never return unused chemical to bottles. 7. Never direct look or direct smell test tubes. 8. Never insert your dropper or pipette or spatula in reagent bottles. 9. No food, no drink, no contact lenses and no gum in Lab. 10. Before beginning: o Clean and dry bench, glassware and equipment. 11. Heating chemicals: o Point the test tube away from you and others. o Hold the test tube with its holder at an angle over the flame and continuously move the test tube. o Never heat a flammable liquid on a direct (open) flame. o Never place a heated object on the balance (Cool it first). 12. Diluting acid: o Always pour (add) acid into water. √(Never water into acid) 13. dispose of waste products according to instructions o Liquids and water-soluble chemicals may be disposed in sink. o Hazardous Organic liquids should be disposed in special containers in the hood. o Dispose the insoluble solid chemicals and broken glassware in waste basket. 14. Before leaving the lab: o Return equipment and chemicals to their proper places. o Clean all your equipment after use.( 15 min before lab end) DR: A.E 15. Learn the location and the usage of the following: o Eyewash Fountain o Fire extinguisher o Safety shower o Emergency exit o Fire blanket If chemicals is spilled on your hand, wash them for 10 minutes. (Don’t try to neutralize spilled acid or base) Material Safety Data Sheets (MSDS): A Material Safety Data Sheet (MSDS) is a document containing information on the material's potential hazards. DR: A.E What is the hazard? Anything that can hurt you or make you ill or cause damage. Types of Hazards: I. Chemical Hazard o Toxic - Corrosive - Irritant - Explosive II. Biological Hazard o Biological tissues - pathogenic microbes III. Physical Hazard o Noise - Radiation VI. Mechanical or electrical Hazard o High voltage equipment V. Psychological Hazard Hazard Rating Systems: National fire protection agency (NFPA) designed colored system to explain the kind of hazardous material ❖ Red: Flammability ❖ Yellow: Reactivity ❖ Blue: Health Hazard ❖ White: Specific Hazard Routes of exposure to hazards: 1- Inhalation (Lungs) 3- Direct contact (skin or eyes) 2- Ingestion (Mouth) 4- Injection DR: A.E Hazards Exposure Limits: 1. For Exposure by Inhalation: a) Lethal Concentration 50 "Lc50" Concentration of a chemical needed to cause death of 50% of test animals when they exposed to chemical by inhalation route. b) Lethal Concentration low "LCLo" The lowest concentration of a chemical needed to kill one human or animal when it exposed to chemical by inhalation route. 2. For Exposure by any route other than Inhalation: a) Lethal Dose 50 "LD50" Dose of a chemical needed to cause death of 50% of test animals when they exposed to chemical by any other route than inhalation. b) Lethal Dose low "LDLo" The minimum amount of a chemical needed to kill one human or animal when it exposed to chemical by any other route than inhalation. As Lc50 or LD50 increases this mean it is more safe Laboratory Equipment and Glassware: Dropper DR: A.E  Identification of inorganic Compounds Chemical analysis Qualitative Quantitative Identification of Unkown Substance Determination of amount known (Name of Compound) substance (Concentration) Qualitative analysis of inorganic salts: Acid + Base → Salt + H2O Ex) HCl + NaOH → NaCl + H2O NaCl Na+ Cl- + Ve ion -Ve ion Cation Anion Basic radical (B.R) Acidic radical (AR) Types of Salts 1-Neutral salt: a-Strong acid + strong base → Neutral salt + H2O Ex) HCl + NaOH → NaCl + H2O b-Weak acid + Weak base → neutral salt + H2O Ex) H2CO3 + NH4OH → (NH4)2 CO3 + H2O 2-Acidic salt: Strong acid + Weak base → Acidic salt + H2O Ex) HCl + NH4OH → NH4Cl + H2O 3-Basic Salt: Weak acid + strong base → Basic salt + H2O Ex) H2CO3 + NaOH → (Na4)2CO3 + H2O DR: A.E  1. Identification of acidic radical The acidic radicals are classified into 3 main groups: Group I Group II Group III AR affected by dil. HCl A.R affected by Conc. H2SO4 A.R affected by BaCl2 𝐶𝑂32− : Carbonate Cl- : chloride SO2− 4 : Sulphate HCO− 3 : Bicarbonate Br- : Bromide PO3− 4 : phosphate S2- : Sulphide I- : Iodide BO− 2 Borate SO2− 3 : Sulphite NO− 3 : Nitrate 𝑆2 O2− 3 : thioSulphate NO− 2 : Nitrite Idea of classification: Strong acid Replace weak acid from its salt. Ex1: HCl + Na2CO3 → NaCl + H2CO3 Strong acid Salt of Weak acid weak acid ∴HCl can react (replace) Carbonate HCl used to identify 𝐶𝑂32− Ex2: HCl + NaCl (Salt of Strong acid) → -Ve ∴ Cl- can't identified by HCl But: H2SO4 + NaCl → Na2SO4 + HCl Stronger Acid ∴Cl- is affected by H2SO4 H2SO4 is used to identify Cl- N.B BaCl2 > H2SO4 > HCl in strength. DR: A.E N.B: 1. 𝑪𝑶𝟐− − 2- 𝟐− 𝟐− − 𝟑 , 𝐇𝐂𝐎𝟑 , S , 𝐒𝐎𝟑 , 𝑺𝟐 𝐎𝟑 , 𝐍𝐎𝟐 Acid radical of weak acids. ∴HCl is used to identify them. 2. Cl-, Br-, I-, 𝐍𝐎− 𝟑 Acid radical of strong acids > HCl ∴HCl can’t be used ∴ H2SO4 is used to identify them. 3. 𝐒𝐎𝟐− 𝟑− − 𝟒 , 𝐏𝐎𝟒 , 𝐁𝐎𝟐 Acid radical of highly strong acids > H2SO4 ∴ HCl & H2SO4 can’t be used BaCl2 is used to identify them. Important Notes: All bicarbonate salts are soluble in water. ( NaHCO3, KHCO3,…..) All carbonate salts are insoluble in water except (Li2CO3, Na2CO3, K2CO3, (NH4)2CO3) All ( NH4, Na, K) salts are soluble in water. 2 HCO3- CO32- + H2O + CO2 N.B: Strong acid: HCl, H2SO4, H3PO4, HNO3 Strong base: NaOH, KOH, Ca(OH)2 Weak acid: H2CO3, CH3COOH Weak base: NH4OH DR: A.E  Scheme for A.R and B.R I. Physical Properties: 1. Color: Colorless, white,... 2. Shape: Powder, Crystalline Cold 3. Solubility: Soluble in water Hot Soluble in dil. HCl A.R → is 𝑪𝑶𝟐– 𝟑 Very small amount of solid Soluble in dil. HNO3 ‫)أقل بكتير من‬ A.R → is 𝑪𝑶𝟐–𝟑 (spatula ‫ربع‬ 2+ B.R → Pb → Exp. )2( 4. Effect on litmus paper: (ONLY done for water soluble salts) If litmus paper turns from: blue → red (Acidic salt) red → blue (basic salt) no change (neutral salt) DR: A.E  Detection of acidic radical Group (I): A.R affected by HCl Test Observation Result Solid + dil HCl A) Effervescence & evolution of may be carbonate (CO32) colorless gas (CO2) which turbids lime or bicarbonate (HCO3-) water I- The salt is water insoluble ∴A.R is CO32- To Differentiae: II- If salt is water Soluble ∴may be CO32- or HCO3- 1. Soln. + MgSO4 a) White ppt in cold ( MgSO4) A.R is Carbonate b) White ppt after boiling A.R is bicarbonate 2. Soln. + HgCl2 a) Reddish brown ppt in cold A.R is Carbonate (HgCO3.3HgO) (mercuric chloride) b) Reddish brown ppt after boiling A.R is bicarbonate Test Observation Result Solid + dil HCl B) Yellow suspension + evolution of A.R may be thiosulphate a colorless gas (SO2) which turns (𝑆2 O2− 3 ) acidified potassium dichromate into green Confirmatory Test 1. Soln. + FeCl3 Dark violet color that decolorized with A.R is thiosulphate time 2. Soln. + lead acetate White ppt (PbS2O3) A.R is thiosulphate Pb(CH3COO)2 (PbS2O3) PbS (black ppt) Test Observation Result Solid + dil HCl C) Evolution of a colorless gas (SO2) A.R may be Sulphite which turns acidified potassium (SO2− 3 ) dichromate into green C.T Decolorization A.R is Sulphite Soln. + acidified KMnO4 Soln. + lead acetate White ppt (PbSO3) A.R is Sulphite DR: A.E  Test Observation Result Solid + dil HCl D) Evolution of a colorless gas (H2S) A.R may be Sulphide which has rotten egg odor and turns (S2-) lead acetate paper into black(pbs) C.T Black ppt (Ag2S) A.R is Sulphide Soln. + AgNO3 Soln. + lead acetate Black ppt (PbS) A.R is Sulphide Test Observation Result Solid + dil HCl E) Evolution of brown fumes (NO2↑) A.R may be Nitrite which turns KI-Starch paper into blue (NO2-) (Bluish-Black) C.T Decolorization (MnSO4) A.R is Nitrite Soln. + acidified KMnO4 Soln. + AgNO3 White ppt (AgNO2↓) A.R is Nitrite Group (II): A.R affected by Conc.H2 SO4 (1) Cl¯ Chloride Test Observation Result A) Evolution of colorless 2) Solid + Conc.H2SO4 gas (HCl), which forms A.R may be Cl¯ white fumes with ammonia. Confirmatory Test: 1) Soln + AgNO3 → White ppt A.R Is Chloride (Cl¯) 2) Soln + lead acetate → White ppt A.R Is Chloride (Cl¯) Pb(CH₃COO)₂ DR: A.E (2) Br– Bromide Test Observation Result B) Evolution of reddish brown vapors gas (Br2), 2) Solid + Conc.H2SO4 A.R may be Br¯ which turn starch paper reddish orange. Confirmatory Test: 1) Soln + AgNO3 → Pale yellow ppt A.R Is Bromide (Br- ) 2) Soln + lead acetate → White ppt which is A.R Is Bromide (Br- ) Pb(CH₃COO)₂ soluble by boiling (3) I¯ Iodide Test Observation Result C) Evolution of Violet 2) Solid + Conc.H2SO4 vapors gas (I2), which turn A.R may be I¯ starch paper blue. Confirmatory Test: → yellow ppt insoluble in 1) Soln + AgNO3 A.R Is Iodide (I¯) both ammonia and dil. HNO3 2) Soln + CuSO4 A.R Is Iodide (I¯) → Brown ppt (4) NO3¯ Nitrate Test Observation Result D) Evolution of brown fumes (NO2), which turn 2) Solid + Conc.H2SO4 A.R may be NO3¯ KI-starch paper into blue. (in presence of Cu-metal) Confirmatory Test: → Brown ring Brown ring test A.R Is Nitrate (NO3¯) [Fe(NO)(H2O)5SO4] FeSO4, C.H2SO4 DR: A.E Group (III) A.R affected by BaCl2 Test Observation Result Soln+ barium chloride White ppt A.R may be sulphate, phosphate, borate ppt + dil. nitric acid A) ppt is Insoluble A.R may be sulphate B) ppt is Soluble A.R may be phosphate, borate C.T for sulphate White ppt i) Soln. + silver nitrate (Ag2SO4↓) A.R is Sulphate ii) Soln. + lead acetate White ppt 𝐒𝐎𝟐− 𝟒 (PbSO4↓) Test Observation Result ppt + dil. nitric acid B) ppt is Soluble may be phosphate 𝐏𝐎𝟑− 𝟒 or borate 𝐁𝐎− 𝟐 Diff between PO43- & BO2- 1) Soln. + Magnesia mixture a) White ppt A.R may be phosphate (MgCl2, NH4OH, NH4Cl) b) -ve A.R may be borate 2) Soln. + silver nitrate a) Yellow ppt A.R is phosphate b) White ppt A.R is borate 3) Soln. + ammonium molybdate a) Cannary yellow ppt A.R is phosphate ((NH4)2MoO4)+ conc. nitric acid A.R is borate b) -ve a) Red paper turned into A.R is borate 4) Turmeric paper test blue DR: A.E  Detection of Basic radical B.R. Precipitating ppt. Gp. Medium PPT form agent Ag+ AgCl white 1 (I) Pb2+ dil. HCl Acidic Chlorides PbCl2 white Hg22+ Hg2Cl2 white Cd2+ CdS yellow Bi3+ Bi2S3 Brown 2 (II) H2S + dil. HCl Acidic Sulphides Cu2+ CuS Black Hg2+ HgS Black Fe2+ Fe(OH)2 Dirty green Cr3+ Basic Cr(OH)3 Gray green 3 (III) NH4OH + NH4Cl Hydroxides Fe3+ = Alkaline Fe(OH)3 Brown A13+ Al(OH)3 gel.white Zn2+ ZnS white Mn2+ H2S + NH4OH + Basic MnS Buff 4 (IV) Sulphides Ni2+ NH4Cl = Alkaline NIS Black Co2+ CoS Black Ca2+ CaCO3 white (NH4)2CO3 + Basic 5 (V) Ba2+ Carbonates BaCO3 white NH4OH+NH4Cl = Alkaline Sr2+ SrCO3 white Mg2+ Na3PO4 + NH4OH + NH4Cl → white ppt. K+ Sod. cobaltinitrite Na3[Co(NO2)6] → yellow ppt. 6 (VI) NH4+ 30% NaOH→ order of ammonia Na+ Flame Test → Golden Yellow Ksp increases from up (group I) to down (group VI) DR: A.E 1) 𝑵𝑯+ 𝟒 𝑏𝑜𝑖𝑙 Solid + 30% NaOH or soda lime → evolution of NH3 ↑ ammonia gas NH3 detected by: 1. its odor 2. Forms white Fumes with HCl 3. Turns red Litmus paper into blue Confirmatory Test a- Soln + Nessler's reagent K2[HgI4] → brown ppt. (Hg2O.NH2I) b- Soln + Hydrogen Tartrate → white ppt. c- Soln + acetic acid + sod. cobaltinitrite → Yellow ppt.(NH4)3[Co(NO2)6] 2) Gp.I Pb2+ , Ag+ , 𝑯𝒈𝟐+ 𝟐 mercurous PbCl2 soluble in hot H2O → Pb2+ Soln + dil. HCl → while ppt. AgCl soluble in NH3 → Ag+ HgCl2 not soluble → 𝐻𝑔22+ Confirmatory Test Yellow ppt. → Pb2+ Soln + K2CrO4 Red ppt. → Ag+ brown ppt → 𝐻𝑔22+ brown ppt, soluble in ammonia ∴ Ag+ 𝑁𝐻3 Ag2O ↓ → [Ag(NH3)2+] soluble Soln + NaOH white ppt, soluble in excess NaOH ∴ Pb2+ 𝑒𝑥𝑐𝑒𝑠𝑠 Pb(OH)2 → Na2pbO2 black ppt ∴ 𝐻𝑔22+ Note: PbCl2 is soluble in hot water and ppted in cold water DR: A.E 3) Gp.II Cd2+, Cu2+, Bi3+ , Hg2+ mercuric yellow ppt. → CdS Solid + H2S + Brown ppt. → Bi2S3 dil. HCl Black ppt. → CuS Black ppt. → HgS white ppt. → Cd2+ ∆ Blue ppt → Black ppt. → Cu2+ Soln + NaOH ∆ white ppt. → Yellow ppt. → Bi3+ ∆ Yellow ppt → Hg2+ excess of KI brown ppt. → Yellow Soln + Bi3+ Soln + KI white ppt → Cu2+ Red ppt. → Hg2+ 4) Gys III Fe2+ Ferrous, Fe3+ Ferric, Al3+, Cr3+ White gelatinous ppt→ Al3+ Gray green ppt → Cr3+ Soln + excess NH₄Cl + aq. NH3(till alkalinity) Brown ppt. → Fe3+ Dirty green ppt. → Fe2+ DR: A.E  (C.T) 1. Soln + NaOH White gelatinous ppt → Al3+ OR Soln + Na3PO4 Gray green ppt or Green ppt → Cr3+ blood red Color → Fe3+ 2. Soln + NH4SCN -Ve → Fe2+ or Al3+ or Cr3+ 3. Soln + K4[Fe(CN)6] Blue ppt → Fe2+ OR K3 [Fe(CN)6] -Ve → Fe3+ or Al3+ or Cr3+ 5) Gp IV Zn2+, Mn2+, Ni2+, Co2+ Buff ppt → Mn2+ white ppt → Zn2+ 1. Soln + excess NH₄Cl + aq. NH3 (till alkalinity) + H₂S → Ni2+ Black ppt → Co2+ (C.T) Buff ppt → Mn2+ white ppt → Zn2+ 2. Soln + NaOH Green ppt → Ni2+ Blue ppt → Co2+ 3. Soln + dimethylglyoxime C4H8N2O2 Red ppt. → Ni2+ (DMG) + aq. NH3 -Ve → Co 2+ DR: A.E 6). Gp V Ca2+, Ba2+, Sr2+ white ppt → CaCO3 Soln + (NH4)2CO3 + white ppt → BaCO3 NH4OH+NH4Cl white ppt → SrCO3 while ppt immediately → Ba2+ Soln + CaSO4 while ppt. after boiling or after scratching → Sr2+ -Ve → Ca2+ 7) Mg2+ Soln + NH4Cl + NH4OH + Na3PO4 → white ppt C.T Soln + Na2CO3 → white ppt. 8) K+ Soln + acetic acid + Sod-Cobaltinitrite → Yellow pp. C.T Soln + Tartaric acid → white ppt. Flame Test: Na+ → Golden Yellow K+ → Violet Ba2+ → apple green Ca2+ → brick red Sr2+ → Crimson red Cu2+ → green DR: A.E  Solubility product constant (Ksp) Product of concentration of ions at equilibrium. For AgCl: AgCl ⇌ Ag+ + Cl- ∴Ksp = [Ag+][Cl-] Solubility product constant (Ksp) Solubility of ppt Precipitation 1) Group II is precipitated as Sulphide in Acidic medium H2 S ⇌ 2H+ + S2- in AM : HCl → H+ + Cl- Common ion effect The reaction (equilibrium) shift to left (back) ∴ [S2-] ↓ & Ksp ↓ So group II only is ppted (not gp IV) 2) Group IV is ppted as sulphide in Basic medium S ⇌ S2- + 2H+ H2O in B.M: NH4OH ⇌ 𝑁𝐻4+ + OH - diverse ion effect The reaction shift to right (Forward) ∴ [S2-] ↑ & ksp ↑ So group IV Can be ppted. Note ❖ NH4OH is added to increase [S2-] ❖ NH4Cl is added to decrease [OH-] DR: A.E 3) Group III ppted as hydroxide in presence of NH4CI NH4OH ⇌ 𝑁𝐻4+ + OH- NH4CI ⇌ 𝑁𝐻4+ + Cl- Commen ion effect reaction shifts to left (back) ∴ [OH-] ↓ & Ksp ↓ So group II only ppt. (To prevent pptn of group V and VI). 4) Group V ppted as carbonate in presence of NH4OH + NH4CI. (NH4)2CO3 ⇌ 2 𝑁𝐻4+ + 𝐶𝑂32− NH4OH ⇌ 𝑁𝐻4+ + OH- NH4Cl ⇌ 𝑁𝐻4+ + Cl- Common ion effect reaction shifts to left ∴ [𝐶𝑂32− ] ↓ & Ksp ↓ Note ❖ NH4OH to decrease [𝐶𝑂32− ] ❖ NH4Cl to decrease [OH-] So group V only is ppted as Carbonate and to prevent pptn of Mg2+ as carbonate. DR: A.E Properties of Metal Hydroxides: 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 1) 𝑃𝑏 2+ →.Pb(OH)2white ppt → Na2 PbO2 (sod. plumbite) Soluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 2) 𝑍𝑛2+ → Zn(OH)2 white ppt → Na2 ZnO2 Soluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 3) 𝐴𝑙 3+ → Al(OH)3 gelatinous white→ Na2AlO2(sodium aluminate) Soluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 4) 𝐶𝑟 3+ → Cr(OH)3 green ppt → Na2 CrO2 Soluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 5) 𝑀𝑛2+ → Mn(OH)2 white ppt. → Insoluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 6) 𝐶𝑢2+ → Cu(OH)2 blue ppt. → Insoluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 7) 𝐶𝑜 2+ → Co(OH)2 blue ppt. → Insoluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 8) 𝑁𝑖 2+ → Ni(OH)2 pale green ppt. → Insoluble 𝑁𝑎𝑂𝐻 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 9) 𝐹𝑒 3+ → Fe(OH)3 brown ppt. → Insoluble 𝑁𝑎𝑂𝐻 𝑎𝑖𝑟 𝑜𝑥𝑖𝑑𝑎𝑡𝑖𝑜𝑛 10) 𝐹𝑒 2+ → Fe(OH)2 dirty green ppt → Fe(OH)3 brown ppt. 𝑒𝑥𝑐𝑒𝑠𝑠 𝑁𝑎𝑂𝐻 → Insoluble DR: A.E  Identification of Gases Note: + 𝐹𝑒 3+ ❖ NH4SCN (ammonium thiocyanate) → blood-red color + 𝐶𝑜2+ NH4SCN → blue color + 𝑃𝑏3+ + 𝐵𝑎 2+ + 𝑆𝑟 2+ ❖ K2CrO4 (Pot. Chromate) → yellow ppt + 𝐴𝑔+ K2CrO4 → red ppt + 𝐻𝑔22+ K2CrO4 → brown ppt DR: A.E  Chemical formula of compounds HCl Hydrochloric acid CO2 Carbon dioxide H2 S Hydrogen Sulphide Ag2S Silver Sulphide (Black ppt) MgSO4 Magnesium Sulphate MgCO3 Magnesium Carbonate (white ppt) HgCl2 Mercuric Chloride SO2 Sulphur dioxide K2Cr2O7 Potassium dichromate BaCl2 Barium Chloride K2CrO4 Potassium Chromate AgNO3 Silver Nitrate HgCO3.3HgO Basic Mercuric Carbonate (Reddish brown ppt) H2SO4 Sulphoric acid Pb(CH3COO)2 Lead acetate S Sulphur NH4Cl Ammonium Chloride NaOH Sodium Hydroxide NH4OH Ammonium Hydroxide AgCl Silver Chloride (White ppt) AgBr Silver Bromide (Pale yellow ppt) AgI Silver Iodide (yellow ppt) HNO3 Nitric acid Ag3PO4 Silver phosphate (Yellow ppt) MgCl2 +NH4Cl + NH4OH Magnesia Mixture (NH4)2MoO4 Ammonium molybdate DR: A.E  Name Symbol Name Symbol Basic mercuric Pot. Ferro Cyanide K4[Fe(CN)6] HgO.Hg(NH2)NO3 amino Salt pot. Ferri Cyanide K3[Fe(CN)6] Nessler's reagent K2[HgI4] Cupric Ferro Cyanide Cu2[Fe(CN)6] Silver Chrorrate Ag2CrO4 Ferric Ferro Cyanide Silver amino Fe4[Fe(CN)6]3 [Ag(NH3)2]Cl (Prussian blue) Chloride Ferrous Ferri Cyanide Fe3[Fe(CN)6]2 Stannous Chloride SnCl2 (Turnbull's blue) Ferrous ferro Cyanide Fe2[Fe(CN)6] Stannic Chloride SnCl4 Ferric ferri Cyanide Fe[Fe(CN)6] lead Chromate pbCrO4 Amm. thio Cyanide NH4SCN pot Bismuth iodide K[BiI4] Pot. Cyanide KCN Bismuth Sulphide Bi2S3 Sod. Aluminate NaAlO2 Bismuth oxy iodide BiOI Sod. Plumbite Na2PbO2 Cupric oxide CuO mercurous Chloride Hg2Cl2 Cuprous oxide Cu2O mercuric Chloride HgCl2 Sod. Zincate Na2ZnO2 Manganous mercuric oxide HgO Mn(OH)2 hydroxide mercurous oxide Hg2O Manganic hydroxide Mn(OH)3 Ferrous Ammonium Fe(NH4)2(SO4)2 Zinc Sulphide ZnS Sulphate Ferric Amm Sulphate Fe(NH4) (SO4)2 Zinc Ferro Cyanide Zn2 [Fe (CN)6] Pot. Cobalt nitrite K3 [Co(NO2)6] Strantium Sr Sod. Cobalti nitrite Na3 [Co(NO2)6] Strantium Sulphate Sr SO4 DR: A.E