School Science Lessons
2026-03-18
Royal Society of Chemistry

Prepare chemicals

Contents
Preparation instructions: 5.4.0
Prepare acetylene: 16.6.6.1
Prepare acid-base indicators: 5.6.2
Prepare acids and bases: 11.0

Prepare alcohol using immobilized yeast cells: 4.3.15
Prepare alkalis: 5.4.3
Prepare alum crystals: 35.9.4
Prepare aluminium hydroxide precipitate: 7.6.0
Prepare ammonia and ammonium compounds: 3.7.0
Prepare ammonia, Haber precess: 3.01
Prepare ammonia solution: 5.4.0
Prepare amyl acetate. (pear oil): 16.3.7
Prepare apple juice gel: 4.4.1
Prepare artificial gemstones: 12.10.1
Prepare aspirin crystals: 3.1.1
Prepare baking powder: 19.1.12
Prepare BAP solution: 3.3
Prepare bath salts: 12.1.28
Prepare bean curd: 7.6.0
Prepare beeswax candles: 8.1.24
Prepare Benedict's solution: 9.4.2
Prepare biology fixatives: 2.0
Prepare biology solutions: 3.0
Prepare boric acid crystals: 3.1.2
Prepare Bouin's solution: 2.2
Prepare bromine water: 12.19.9.1.1
Prepare buffer solutions: 12.12.1
Prepare butane: 16.6.4.1
Prepare Calberla's pollen stain: 7.11
Prepare calcium oxide: 34.2.7
Prepare camphor oil: 19.3.6 Prepare camphor oil
Prepare Canada balsam mounting solution: 6.1
Prepare candles: 8.1.24, beeswax candles
Prepare carbon dioxide: 3.4.0
Prepare carbon dioxide: 19.1.7
Prepare Carnoy's solution: 2.3
Prepare casein plastic from milk: 3.3.5
Prepare chlorine: 12.19.7
Prepare chloroform: 16.1.8
Prepare chrome alum: 12.8.10
Prepare chromium trioxide: 12.8.2
Prepare cider from apple juice: 4.4.2
Prepare citric acid crystals with lemon juice: 12.6.1
Prepare colloidal sulfur: 7.6.0
Prepare copper compounds: 12.5.0
Prepare creams and ointments: 5.5.0
Prepare CRAF biology fixative solution: 2.4
Prepare crystals: 3.appendixBH
Prepare crystal blossoms 3.1.2
Prepare crystal clusters 3.1.3
Prepare culture media to identify fungi: 4.0
Prepare cup of tea: 12.2.8
Prepare Czapek Dox solution: 1.4
Prepare DCIP solution: 7.16
Prepare DPX mountant solution: 6.2
Prepare decoctions: 5.5.0
Prepare Delafield's haematoxylin solution: 7.15
Prepare detergent, alcohol-based detergent: 12.5.10
Prepare dilute acids: 5.4.0
Prepare dilute acids and bases, (Safety): 3.4.10
Prepare dilute bases: 5.4.0
Prepare distilled water: 2.2.14
Prepare DOMESTOS solution: 3.8
Prepare DRBC agar solution: 1.5
Prepare egg recipes: 16.3.8, (See: 1.)
Prepare eggs for food: 13.0
Prepare Ehrlich's haematoxylin solution: 7.17
Prepare eosin solution: 7.18
Prepare esters: 16.3.9
Prepare ethanal with potassium dichromate: 16.3.2.7
Prepare ethanal with potassium manganate (VII): 16.3.2.6
Prepare ethane: 16.6.1.1
Prepare glucose with sugar: 16.6.4
Prepare ethane gas: 16.6.4.1
Prepare ethanoic acid: 9.1.10
Prepare ethene: 16.4.3
Prepare ethyl acetate: 16.4.2
Prepare ethyl butyrate, (pineapple oil): 16.4.3
Prepare ethyl chloride: 16.4.1
Prepare ethyl ethanoate: 16.4.2
Prepare ethyne: 16.4.5.6.1
Prepare excipients: 5.5.0
Prepare face cream emulsion: 7.6.0
Prepare Fehling's solution: 9.5.1
Prepare ferric hydroxide colloid: 7.6.0
Prepare ferric tannate with tea leaves: 16.4.4
Prepare fibrous plaster board with plaster of Paris: 3.6.5
Prepare flour glue: 9.1.1
Prepare fluorescence staining of cells and tissues: 7.22
Prepare foams: 7.6.0
Prepare food, using microbiology: 4.4.0
Prepare formaldehyde-resorcinol resin: 3.3.6
Prepare forms of sulfur: 7.5.0
Prepare fresh material for microscope work (wet mount): 2.5.7
Prepare fruit salts, "health salts": 16.4.5
Prepare gases at standard conditions: 3.32
Prepare gases from coal: 16.1.2
Prepare gases from coal:16.1.2
Prepare gases from wood: 3.99.0
Prepare gases with gas generation apparatus: 13.3.0
Prepare gels in the home kitchen: 7.6.0
Prepare gelatine gel: 7.6.0
Prepare Giemsa stain: 7.19
Prepare glacial acetic acid: 9.1.10
Prepare glucose with starch: 16.6.3
Prepare glucose with starch: 16.6.3
Prepare glucose with sugar: 16.6.4
Prepare glycerine jelly solution: 6.3
Prepare Gram stain: 7.20
Prepare Gram's iodine solution: 3.11
Prepare hard water: 12.2.4
Prepare Haupt's adhesive solution: 6.4
Prepare haematoxylin stain: 7.23
Prepare herbal infusions: 5.5.0
Prepare herbal solutions: 5.5.0
Prepare herbal tinctures: 5.5.0
Prepare hydrochloric acid with sodium chloride: 13.3.27
Prepare hydrogen chloride / hydrochloric acid: 13.3.14
Prepare hydrogen bromide: 12.19.9.3
Prepare hydrogen fluoride: 12.19.7.1
Prepare hydrogen gas: 13.3.15
Prepare hydrogen iodide, HI: 12.19.6.1
Prepare hydrogen peroxide solution: 17.7.22
Prepare hydrogen sulfide: 13.3.16
Prepare hydroxides with ammonia solution: 3.7.6
Prepare immersion oil: 7.26
Prepare infused oils: 5.5.0
Prepare insect-fixing solutions: 5.0
Prepare insoluble salts: 12.10.10
Prepare invert sugar: 3.1.12
Prepare invisible ink: 3.2.0
Prepare iodine compounds: 1.0
Prepare jelly with fresh pineapple and tinned pineapple: 19.2.9.1
Prepare known concentration solutions: 5.4.0
Prepare lactic acid with milk: 12.7.10
Prepare lactic acid with sourdough: 4.4.3
Prepare lactose from milk 4.4.4
4.8 Prepare lactophenol solution, (LPCB)
Prepare lampblack: 8.1.25
Prepare lead-acid battery electrolyte: 32.5.3.6
Prepare lead-tin alloys in a casting mould: 3.61.0
Prepare lead dioxide and lead (II) nitrate: 12.9.4
Prepare Leishman's stain: 7.29
Prepare lime, quicklime: 34.2.7
Prepare lime, slaked lime: 34.2.8
Prepare limewater: 5.4.0
Prepare litmus solution: 15.00
Prepare Loeffler serum solution: 4.9
Prepare Lugol's iodine solution: 3.14
Prepare magnesium carbonate precipitate: 7.6.0
Prepare manganates: 12.8.2
Prepare Mayer's haematoxylin solution: 7.28
Prepare mayonnaise and salad dressing emulsions: 7.6.0
Prepare metallic salts gels: 7.6.0
Prepare metanil yellow solution: 18.00
Prepare methane gas: 16.5.1.1
Prepare methyl chloride gas: 16.4.8
Prepare methyl green solution: 19.00
Prepare methyl salicylate: 16.4.9
Prepare methylene blue solution: 7.30
Prepare Meyer's albumen solution: 6.5
Prepare microbiology cultures: 4.1.0
Prepare microbiology techniques: 4.3.0
Prepare microscopy stains and adhesives: 7.0
Prepare microcosmic salt: 12.9.0
Prepare molar solutions: 5.4.0
Prepare molar volume of oxygen with hydrogen peroxide: 17.7.21
Prepare monoprotic acid solution from unknown molarity acid: 12.11.4.8
Prepare mordants: 19.4.3
Prepare naphthalene crystals from mothballs: 12.8.3
Prepare natural buffer: 12.12.6
Prepare nitric acid: 13.3.17
Prepare nitric oxide: 13.3.18
Prepare nitrous acid: 13.3.21
Prepare nitrous oxide: 13.3.22
Prepare nitrogen dioxide: 13.3.19
Prepare nitrogen gas: 13.3.20
Prepare oil of wintergreen: 16.4.9
Prepare orange IV solution: 7.33
Prepare Orcinol-Bial's reagent: 4.11
Prepare oxalic acid: 9.1.12
Prepare oxides by direct oxidation: 12.13.2
Prepare oxides by indirect oxidation: 12.13
Prepare oxygen absorbent: 12.12.7
Prepare oxygen gas: 12.12.0
Prepare ozone gas: 3.5.0
Prepare Papanicolaou stain: 7.34
Prepare permanent crease solution: 19.4.4
Prepare Peru balsam: 6.6
Prepare phenolphthalein: 30.01
Prepare phenylamine: 16.7.15
Prepare phloroglucinol solution: 7.35
Prepare phosphorus pentachloride: 12.9.0
Prepare phosphorus pentoxide: 12.9.0
Prepare phosphorus trichloride: 12.9.0
Prepare plant acid-base indicators: 24.01
Prepare plant dyes: 3.30
Prepare plastics: 3.3.0
Prepare polymers: 3.3.0
Prepare potash alum: 12.14.2
Prepare potash from ash: 6.9.16
Prepare potassium dichromate: 12.8.6
Prepare potassium compounds: 4.0
Prepare potassium perchlorate crystals: 12.19.8.5
Prepare poultices: 5.5.0
Prepare preserving agents for cut flowers: 19.3.8
Prepare putty: 34.2.9
Prepare protein solutions: 16.6.1
Prepare quicklime: 34.2.7
Prepare reagents: 14.0
Prepare red cabbage acid-base indicator: 25.01
Prepare resazurin stain test for milk: 16.1.6
Prepare rayon: 3.3.8
Prepare reagents: 14.0
Prepare Ringer solution: 3.20
Prepare rose petal acid-base indicator: 26.01
Prepare safranin solution: 7.36
Prepare salt solutions: 13.0
Prepare salts: 12.6.0
Prepare salts with clay suspension: 7.6.0
Prepare sauerkraut: 4.4.6
Prepare Scott's blueing solution: 3.22
Prepare sedimentary rocks: 35.9.4
Prepare self-leavened flour, "self-raising flour": 19.1.9, (See: 7.)
Prepare serial dilutions: 12.0
Prepare serial dilution, different % concentrations: 5.2.0
Prepare sets of apparatus: 2.2.7
Prepare silica / silicon compounds: 1.0
Prepare silica gel: 7.6.0
Prepare silicon glass: 7.6.0
Prepare silly putty: 12.10.9
Prepare silver chloride precipitate: 7.6.0
Prepare simple chemical rectifier: 33.3.5
Prepare slaked lime, lime: 34.2.8
Prepare slime, PVA slime: 3.3.9
Prepare soap: 12.4.0
19.3.7 Prepare soap, household soap
Prepare soda lime: 34.2.12
Prepare sodium carbonate: 12.6.22
Prepare sodium carbonate solutions: 5.4.0
Prepare sodium thiosulfate crystals: 12.18.6.1
Prepare sparklers: 15.515
Prepare stock materials and apparatus: 2.2.8
Prepare stock solutions: 5.7.0
Prepare streptomycin using Streptomyces griseus: 4.1.11
Prepare sugar crystals: 16.5.8
Prepare sugar crystals from brown sugar: 3.1.17
Prepare sulfides: 12.18.2.0
Prepare sulfur allotropes: 7.5.1
Prepare sulfur crystals: 35.9.4
Prepare sulfur, forms of sulfur: 7.1.5
Prepare sulfur dioxide by heating sulfur: 7.1.5.5
Prepare sulfur dioxide: 13.10.3
Prepare sulfur monochloride: 12.18.3.1
Prepare sulfuric acid: 12.16.4.0
Prepare sunbeam mists, HCl + NH4Cl: 7.6.0
Prepare syrups: 5.5.0
Prepare tea, (cup of tea): 12.2.8
Prepare tin (IV) chloride: 12.20.2
Prepare toluidine blue solution: 7.38
Prepare tonic wines: 5.5.0
Prepare triodomethane, (iodoform): 16.1.13
Prepare trichloromethane, chloroform: 16.1.8
Prepare turpentine copying fluid: 9.1.4
Prepare universal indicator solution: 37.00
Prepare urea-formaldehyde resin: 3.3.12
Prepare verdigris with copper and vinegar: 12.11.1
Prepare vinegar from wine: 19.1.15
Prepare vinegar with (Acetobacter aceti): 4.4.7
Prepare "volcanos" with baking soda: 12.15.8
Prepare wallpaper paste: 9.1.3
Prepare wine from grape juice and prepare vinegar from wine: 4.4.8
Prepare wood gas and wood tar by heating sawdust: 16.5.2
Prepare Wright's stain: 7.29
Prepare xylene and methylbenzoate solution: 3.28
Prepare Ziehl-Neelsen stain: 7.40
Prepare Zenker's solution: 2.12
Prepare zinc sulfate crystals: 12.10.8
11.0 Prepare acids and bases
molarity 1 × volume 1 = molarity 2 × volume 2, M1V1 = M2V2
Prepare dilute acids
Acetic acid 3 M: Dilute 172 mL of 17.4 M acid to 1 litre of water, (99-800 px acetic acid, ethanoic acid).
Hydrochloric acid 3 M: Dilute 258 mL of 11.6 M acid to 1 litre with water, (35% hydrochloric acid).
Hydrochloric acid 4 M: Dilute 400 mL of 10 M acid to 1 litre of water, for normal class use.
Nitric acid 4 M: Dilute 240 mL of 15 M acid to 1 litre water, for normal class use.
Nitric acid 3 M: Dilute 195 mL of 15.4 M acid to 1 litre of water, (69% nitric acid).
Sulfuric acid 6 M: Dilute 168 mL of 17.8 M acid to 1 litre of water, (95% sulfuric acid).
Sulfuric acid 2 M: Dilute 112 mL of 35 M in 800 mL water, then add water to 1 litre, for normal class use.
Prepare dilute bases
Ammonia solution 4 M: Dilute 220 mL (28% ammonia), 18 M concentrated solution to 1 litre of water, ("ammonium hydroxide").
Ammonia solution 3 M: Dilute 200 mL (28% ammonia), 14.8 M concentrated solution to 1 litre of water.
Ammonia solution 2 M: Dilute 330 mL (10% ammonia), 6 M concentrated solution to 1 litre of water, for normal class use.
Potassium hydroxide 4 M: Dissolve 220 g KOH sticks in water, dilute to 1 litre of water, for normal class use.
Sodium hydroxide 3 M: Dissolve 126 g the sticks, 95%, in water and dilute to 1 litre of water.
Sodium hydroxide 4 M Dissolve 160 g NaOH in 500 mL water, then dilute to 1 litre of water, for normal class use.
Sodium hydroxide 8.5 M Dissolve 330 g NaOH in water, dilute to 1 litre of water, for CO2 absorption.
Prepare solutions:
Saturated solution 1. 1.5 g Ca(OH)2per litre, use some excess, filter off CaCO3, and protect from CO2 of the air.
Saturated solution 2. Add 125 g of slaked lime, Ca(OH)2, to 3 litres of water, shake, allow precipitate to settle, siphon off clear liquid, protect from CO2 in air.
13.0 Prepare salt solututions
Dissolve amount below, then dilute to 1 L with water.
Aluminium chloride, AlCl3.6H2O, For 0.1 M solution, use 24 g of hydrated salt in 1 L water.
Aluminium sulfate, Al2(SO4)3.18H2O, For 0.l M solution, use 66 g of hydrated salt in 1 L water.
Ammonia, NH3(aq) or NH4OH, For 2 M solution, use dilute 330 mL of 10% solution in 1 L water.
Ammonium chloride, NH4Cl, For 5 M solution, use 270 g in water.
Ammonium carbonate (NH4)2CO3.3H2O, For 2 M solution, use 300 g in 450 mL 10% NH3, then dilute in 1L water.
Ammonium iron (II) sulfate, For 0.1 M solution, use 39.2 g in water, add 5 mL conc. H2SO4 in 1 L water.
Ammonium oxalate, C2O4(NH4)2.2H2O, For 0.1 M solution, use 16 g in 1 L water.
Ammonium sulfate (NH4)2SO4, For 0.1 M solution, use 13.2 g in 1 L water.
Barium chloride, BaCl2.2H2O, For 0.1 M solution, use 24.4 g in 1 L water.
Bismuth chloride, BICl3, For 0.17 M solution, use 53 g in 1 litre of dilute HCl, 1 part conc. HCl to 5 parts water.
Bismuth nitrate, Bi(NO3)3.5H2O, For 0.083 M solution, use 40 g in 1 litre of dilute HNO3, 1 part conc. HNO3 to 5 parts water.
Calcium chloride, CaCl2 anhydrous 0.l M solution, use 11 g in1 L water.
Calcium chloride, CaCl2.2H2O, For 0.1 M solution, use 14.7 g in 1 L water.
Calcium hydroxide, Ca(OH)2, limewater, 10 g in 1 L water, shake, allow it to settle, decant clear liquid.
Calcium nitrate, Ca(NO3)2, For 0.1 M solution, use 16.4 g in 1 L water.
Calcium sulfate, CaSO4.2H2O, For 0.1 M solution, shake 10 g in 1 L water, leave to stand, decant the clear liquid.
Cobalt (II) chloride-6-water, CoCl2.6H2O, For 0.1M solution, use 23.8 g in 1 L water.
Cobalt nitrate, Co(NO3)2.6H2O, For 0.1M solution, use 29 g in 1 L water.
Copper (II) nitrate, Cu(NO3)2.6H2O, For 0.1 M solution, use 29.6 g in 1 L water.
Copper (II) sulfate, CuSO4.5H2O, For 0.1 M solution, use 25 g in 1 L water + 5 mL conc. H2SO4.
Iron (II) ammonium sulfate, Fe(NH4SO4)2.6H2O, For 0.5 M solution, use 196 g in 1 L water + 10 mL conc. H2SO4, dilute to 1 litre.
Iron (III) chloride, FeCl3.6H2O, For 0.1 M solution, use 27 g in 1 L water + 20 mL HCl.
Iron (III) nitrate, Fe(NO3)3.9H2O, For 0.1 M solution, use 40.4 g in 1 L water.
Iron (II) sulfate, FeSO4.7H2O, For 0.1 M solution, use 27.8 g in 1 L water + 1 mL conc. H2SO4 to clear.
Iron (III) sulfate, Fe2(SO4)3.9H2O, For 0.1 M solution, use 56 g in 1 L water.
Lead ethanoate (CH3COO)2Pb.3H2O, For 0.1 M solution, use 38 g in 1 L water + dilute ethanoic acid to clear.
Lead nitrate, Pb(N03)2, For 0.1 M solution, use 33 g in 1 L water.
Magnesium chloride, MgCl2.6H2O, For 0.1 M solution, use 20.3 g in 1 L water.
Magnesium nitrate, Mg(N03)2.6H2O, For 0.1 M solution, use 25.6 g in 1 L water.
Magnesium sulfate, MgSO4.7H2O, For 0.1 M solution, use 24.7 g in 1 L water.
Manganese sulfate, MnSO4.H2O, For 0.1 M solution, use 16.9 g in water.
Nickel chloride, NiCl2.6H2O, For 0.1 M solution, use 24 g in 1 L water.
Potassium bromide, KBr, For 0.1 M solution, use 12 g in 1 L water.
Potassium carbonate, K2CO3, For 0.1 M solution, use 13.8 g in water.
Potassium chloride, KCl, For 0.1 M solution, use 7.5 g in 1 L water.
Potassium dichromate, For 0.1 M solution, use 29.4 g in 1 L water (K2Cr2O7).
Potassium dihydrogen orthophosphate, For 0.1 M solution, use 13.6 g in 1Lwater (KH2PO4).
Potassium hydroxide, KOH, For 2 M solution, use 110 g of KOH sticks in 1 L water.
Potassium iodide, KI, For 0.1 M solution, use 16.6 g in 1 L water.
Potassium nitrate, KNO3, For 0.1 M solution, use 10.l g in 1 L water.
Potassium permanganate, KMnO4, For 0.1 M solution, use 15.8 g in 1 L water.
Potassium sulfate, K2SO4, For 0.1 M solution, use 17.4 g in 1 L water.
Silver nitrate, AgNO3, For 0.1 M solution, use 17 g in 1 L water.
Sodium borate, Na2B4O7.l0H2O, For 0.1 M solution, use 38 g in 1 L water.
Sodium carbonate, Na2CO3.10H2O, For 0.1 M solution, use 28.6 g in 1 L water.
Sodium carbonate, Na2CO3 (anhydrous), For 0.1 M solution, use 10.6 g in 1 L water.
Sodium chloride, NaCl, For 0.1 M solution, use 5.8 g in 1 L water.
Sodium chromate, Na2CrO4.4H2O, For 0.1M solution, use 23.4g in 1 L water.
Sodium dichromate, Na2Cr2O7.2H2O, For 0.1 M solution, use 29.8 g in 1 L water.
Sodium ethanoate, CH3COONa.3H2O, For 00.1 M solution, use 13.6 g in 1 L water (sodium acetate).
Sodium hydrogen carbonate, NaHCO3, For 0.1 M solution, use 8.4 g in 1 L water.
Sodium iodide, NaI, For 0.1 M solution, use 15 g in 1 L water.
Sodium molybdate, Na2MoO4.2H2O, For 0.1 M solution, use 24.2 g in 1 L water.
Sodium nitrate, NaNO3, For 0.1 M solution, use 8.5 g in 1 L water.
Sodium nitrite, NaNO2, For 0.1 M solution, use 7 g in 1 L water.
Sodium oxalate, Na2C2O4, For 0.1 M solution, use 13.4 g in 1 L water.
Sodium sulfate, Na2SO4.10H2O, For 0.1 M solution, use 32.2 g in 1 L water.
Sodium sulfide, Na2S.9H2O, For 0.5 M solution, use 120 g in 1L water.
Sodium sulfite, Na2SO3.6H2O, For 0.1 M solution, use 23.4 g in 1 L water.
Sodium sulfite, Na2SO3 (anhydrous), For 0.1 M solution, use 12.6 g in 1 L water.
Sodium thiosulfate, Na2S2O3.5H2O, For 0.1 M solution, use 24.8 g in 1 L water.
Strontium (II) chloride, SrCl2.6H2O, For 0.1 M solution, use 26.7 g in 1 L water.
tri-Sodium phosphate, Na3PO4.12H2O, For 0.1 M solution, use 38 g in 1 L water.
Tin (II) chloride, SnCl2.2H2O, For 0.5 M solution, use 113 g in 170 mL conc. HCl, dilute to 1 L + add tin foil.
Tin (IV) chloride, SnCl2.5H2O, For 0.1 M solution, use 35 g in 1 L water.
Zinc sulfate, ZnSO4.7H2O, For 0.1 M solution, use 28.8 g in 1 L water.
14.0 Prepare reagents
("in water" = "dissolve in 1 litre of distilled water")
Substance, formula Concentration M, dissolve amount below then dilute to 1 litre with water.
Aluminium chloride, AlCl3.6H2O 0.1 M, 24 g of hydrated salt in water
Aluminium sulfate, Al2(SO4)3.18H2O 0.l M, 66 g of hydrated salt in water
Ammonia, NH3(aq) or NH4OH 2 M, dilute 330 mL of 10% soln.
Ammonium chloride, NH4Cl 5 M, 270 g in water
Ammonium carbonate (NH4)2CO3.3H2O 2 M, 300 g in 450 mL 10% NH3, then dilute
Ammonium iron (II) sulfate 0.1 M, 39.2 g in water, add 5 mL conc. H2SO4
Ammonium oxalate, C2O4(NH4)2.2H2O 0.1 M, 16 g in water
Ammonium sulfate (NH4)2SO4 0.1 M, 13.2 g in water
Barium chloride, BaCl2.2H2O 0.1 M, 24.4 g in water
Bismuth chloride, BiCl3
 0.17 M, 53 g in 1 litre of dilute HCl, 1 part conc. HCl to 5 parts water
Bismuth nitrate, Bi(NO3)3.5H2O 0.083 M, 40 g in 1 litre of dilute HNO3, 1 part conc. HNO3 to 5 parts water
Calcium chloride, CaCl2, anhydrous 0.l M, 11 g in water
Calcium chloride, CaCl2.2H2O 0.1 M, 14.7 g
Calcium hydroxide, Ca(OH)2 limewater, 10 g in water, shake, allow it to settle, decant clear liquid
Calcium nitrate, Ca(NO3)2 0.1 M, 16.4 g in water
Calcium sulfate, CaSO4.2H2O 0.1 M, Shake 10 g in water, leave to stand, decant the clear liquid
Cobalt (II) chloride-6-water, CoCl2.6H2O 0.1 M, 23.8 g in water
Cobalt nitrate, Co(NO3)2.6H2O 0.1 M, 29 g in water
Copper (II) nitrate, Cu(NO3)2.6H2O
 0.1 M, 29.6 g in water
Copper (II) sulfate, CuSO4.5H2O
 0.1 M, 25 g in water + 5 mL conc. sulfuric acid
Copper (II) sulfate, CuSO4.5H2O 0.5 M, 124.8 g in water + 5 mL of conc. sulfuric acid
Iron (II) ammonium sulfate, Fe(NH4SO4)2.6H2O 0.5 M, 196 g in water + 10 mL conc. H2SO4, dilute to 1 litre
Iron (III) chloride, FeCl3.6H2O
 0.1 M, 27 g in water + 20 mL hydrochloric acid
Iron (III) chloride, FeCl3.6H2O 0.5 M, 135.2 g in water + 20 mL conc. HCl, dilute to 1 litre
Iron (III) nitrate, Fe(NO3)3.9H2O 0.1 M, 40.4 g in water
Iron (II) sulfate, FeSO4.7H2O
 0.1 M, 27.8 g in water + 1 mL conc. H2SO4 to clear
Iron (II) sulfate 0.5 M, 139 g in water + 10 mL conc. H2SO4, dilute to 1 litre
Iron (III) sulfate, Fe2(SO4)3.9H2O
 0.1 M, 56 g in water
Iron (III) sulfate 0.25 M, 140.5 g in water + 100 mL conc.H2SO4, dilute to 1 litre.
Lead ethanoate (CH3COO)2Pb.3H2O 0.1 M, 38 g in water + dilute ethanoic acid to clear
Lead nitrate, Pb(NO3)2 0.1 M, 33 g in water
Magnesium chloride, MgCl2.6H2O 0.1 M, 20.3 g in water
Magnesium nitrate, Mg(N03)2.6H2O 0.1 M, 25.6 g in water
Magnesium sulfate, MgSO4.7H2O 0.1 M, 24.7 g in water
Manganese sulfate, MnSO4.H2O 0.1 M, 16.9 g in water
Nickel chloride, NiCl2.6H2O 0.1 M, 24 g in water
Potassium bromide, KBr 0.1 M, 12 g in water
Potassium carbonate, K2CO3 0.1 M, 13.8 g in water
Potassium chloride, KCl 0.1 M, 7.5 g in water
Potassium dichromate 0.1 M, 29.4 g in water (K2Cr2O7)
Potassium dihydrogen orthophosphate 0.1 M, 13.6 g in water (KH2PO4)
Potassium hydroxide, KOH 2 M, 112 g in water. Use gloves.
Potassium hydroxide, KOH 2 M, 110 g of KOH sticks
Potassium iodide, KI 0.1 M, 16.6 g in water
Potassium nitrate, KNO3 0.1 M, 10.l g in water
Potassium permanganate, KMnO4 0.1 M, 15.8 g in water
Potassium sulfate, K2SO4 0.1 M, 17.4 g in water
Silver nitrate, AgNO3 0.1 M, 17 g in water
Sodium borate, Na2B4O7.l0H2O 0.1 M, 38 g in water
Sodium carbonate, Na2CO3.10H2O 0.1 M, 28.6 g in water
Sodium carbonate, Na2CO3, (anhydrous) 0.1 M, 10.6 g in water
Sodium chloride, NaCl 0.1 M, 5.8 g in water
Sodium chromate, Na2CrO4.4H2O 0.1 M, 23.4g in water
Sodium dichromate, Na2Cr207.2H2O 0.1 M, 29.8 g in water
Sodium ethanoate, CH3COONa.3H2O 00.1 M, 13.6 g in water (sodium acetate)
Sodium hydrogen carbonate, NaHCO3 0.1 M, 8.4 g in water
Sodium iodide, NaI 0.1 M, 15 g in water
Sodium molybdate, Na2MoO4.2H2O 0.1 M, 24.2 g in water
Sodium nitrate, NaNO3 0.1 M, 8.5 g in water
Sodium nitrite, NaNO2 0.1 M, 7 g in water
Sodium oxalate, Na2C2O4 0.1 M, 13.4 g in water
Sodium sulfate, Na2SO4.10H2O
 0.1 M, 32.2 g in water
Sodium sulfide, Na2S.9H2O 0.5 M 120 g in water and dilute to 1 litre
Sodium sulfite, Na2SO3.6H2O 0.1 M, 23.4 g in water
Sodium sulfite, Na2SO3 (anhydrous) 0.1 M, 12.6 g in water
Sodium thiosulfate, Na2S2O3.5H2O 0.1 M, 24.8 g in water
Strontium (II) chloride, SrCl2.6H2O 0.1 M, 26.7 g in water
tri-Sodium phosphate, Na3PO4.12H2O 0.1 M, 38 g in water
Tin (II) chloride, SnCl2.2H2O
 0.5 M, 113 g in 170 mL conc. HCl, dilute to 1 litre + tin foil
Tin (IV) chloride, SnCl2.5H2O 0.1 M, 35 g in water
Zinc sulfate, ZnSO4.7H2O 0.1 M, 28.8 g in water
5.4.0 Prepare known concentration solutions
Experiments
5.4.1 Ammonium molybdate
5.4.2 Calcium hydroxide, limewater
5.4.3 Dipotassium hydrogen orthophosphate
5.4.4 di-Sodium hydrogen phosphate
5.4.5 Ethanoic acid (acetic Acid)
5.4.6 Hydrochloric acid
5.4.7 Hydrogen peroxide
5.4.14 Oxalic acid (ethanedioic acid)
5.4.15 Phenolphthalein indicator
5.4.16 Sodium chlorate (V)
5.4.17 Sodium dihydrogen phosphate
5.4.9 Sodium hydrosulfite
5.4.10 Sodium hydroxide
5.4.11 Starch solution
5.4.12 Sulfuric acid
5.4.18 Tin (II) chloride
5.4.1 Ammonium molybdate (NH4)6Mo7O24.4H2O Add 45 g to water containing 120 mL 10% ammonia.
Add 120 g NH4NO3 then dilute.
5.4.2 Calcium hydroxide Ca(OH)2
Saturated (limewater ) Ca(OH)2		 Add 10 g to water, shake, let settle, then decant clear liquid.
Calcium hydroxide Ca(OH)20.02 M Add 1.48 g to water, add excess, filter off precipitate.
5.4.3 Dipotassium hydrogen orthophosphate, K2HPO4 0.1 M Add 17.4 g to water.
.
5.4.4 di-Sodium hydrogen phosphate, Na2HPO4.l2H2O 0.1 M Add 35.8 g of Na2HPO4.l2H2O to water.
.
Na2HPO4.2H2O 0.1M Add 17.8 g Na2HPO4.2H2O to water.
5.4.5 Ethanoic Acid, (AceticAcid,) CH3COOH 17M Use as supplied.
.
Ethanoic Acid (Acetic Acid) CH3COOH 2 M (approx.) Dilute 120 mL concentrated (glacial) or use 360 mL 33% acid.
Ethanoic Acid (Acetic acid) CH3COOH 2 M Dissolve 117 mL of 17.15 M acid (99% w / w 1.048 g / mL).
5.4.6 Hydrochloric Acid HCl concentrated 10 M Use as supplied.
.
Hydrochloric acid HC 2 M Dissolve 173 mL of 11.55 M acid (36% w / w 1.17 g / mL).
5.4.7 Hydrogen peroxide H2O2
For laboratory use only.		 To 20 volume solutions (6%) add twice the volume of water.
5.4.9 Sodium hydrosulfite Na2S2O4.2H2O
.
 100 mL solution for use as oxygen gas absorber, 16 g Na2S2O4.2H2O + 13 g NaOH to 100 mL water, + 4 g B-anthraquinone sulfonate to improve reagent.
5.4.10 Sodium hydroxide NaOH Approximately 2M
.
 Add 80 g to water and leave to cool.
Store in a bottle with a rubber stopper.
Use safety glasses and nitrile chemical-resistant gloves.
Sodium hydroxide NaOH
2 M
.
 Add 81.6 g (98% NaOH) to water and leave to cool.
Store in a bottle with rubber stopper.
Use safety glasses and nitrile chemical-resistant gloves.
Sodium hydroxide (for CO2 absorption) Add 330 g to water.
5.4.11 Starch solution,
1%
.
 Add 10 g starch to cold water to make a paste.
Then dilute to 100 mL with boiling water.
Let it boil, stir then leave to stand.
5.4.12 Sulfuric acid concentrated H2SO4 18 M Use as supplied.
.
Sulfuric acid
2 M
.
 Add 113 mL of 17.75 M acid (97% w/w 1.83 g / mL) slowly to water with stirring.
Use safety glasses and nitrile chemical-resistant gloves.
5.4.14 Oxalic acid (COOH)2.2H2O 0.1 M Add 12.6 g of crystals to water.
.
5.4.15 Phenolphthalein indicator Add 5 g to 500 mL of ethanol, add 500 mL water, then stir.
5.4.16 Sodium chlorate (V) NaClO3
0.1 M		 Dilute 10% solution with equal volume water.
.
5.4.17 Sodium dihydrogen phosphate NaH2PO4.2H2O 0.1 M Add 15.6 g to water
.
5.4.18 Tin (II) chloride SnCl2.2H2O
0.1 M		 Add 22.6 g to 100 mL conc. HCl, dilute with water.
Add pieces of tin.
12.0 Prepare serial dilutions
100% solution: Prepare 100 mL of saturated solution, then filter.
0.5% solution: 0.5 mL of saturated solution, add water to 100 mL.
0.1% solution: 20 mL of 0.5% solution, add water to 100 mL.
0.05% solution: 50 mL of 0.1% solution, add water to 100 mL.
0.01% solution: 20 mL of 0.05% solution, add water to 100 mL.
0.005% solution: 50 mL of 0.01% solution, add water to 100 mL.
0.001% solution: 20 mL of 0.005% solution, add water to 100 mL.
12.6.0 Prepare salts
A salt compound is formed when the hydrogen ions in an acid are replaced by metal ions or ammonium ions.
A salt compound is formed by the combination of an acid radical or positive ions with a basic radical or negative ion.
A salt compound is formed by the replacement of all or part of the hydrogen in an acid by a metallic element.
12.6.1 Prepare salts by neutralization of a soluble acid and a base
12.6.2 Prepare salts by acids + metals
12.6.6 Prepare salts by precipitation reactions
12.6.7 Prepare salts by direct union of elements
12.6.8 Prepare salts by bases + non-metallic oxides
12.6.9 Prepare salts by acids + salts
12.6.10 Prepare salts by chemical reactions
12.6.1 Prepare salts by neutralization of a soluble acid and a base
Acid-base neutralization: Acid + Base (Alkali) --> Salt + Water
H + (aq) + OH - (aq) --> H 2 O.
12.6.2 Prepare salts by acids + metals
Acid + metal --> salt + hydrogen gas
(Metals that displace hydrogen from an acid may be called "active metals", e.g. Zn, Fe)
12.6.6 Prepare salts by precipitation reactions
Precipitation reactions, double decomposition reactions, double displacement reactions
Mixing two soluble compounds to prepare an insoluble salt.
Solution 1 + Solution 2 --> Insoluble solid 3 + Solution 4
12.6.7 Prepare salts by direct union of elements
Direct union of elements to form compounds: 8.0.0
12.6.8 Prepare salts by bases + non-metallic oxides
12.17.3.1 Carbon dioxide with sodium hydroxide solution
CO2 (g) + 2NaOH (aq) --> Na2CO3 (aq)+ H2O (l)
12.6.9 Prepare salts by acids + salts
sulfuric acid + sodium chloride --> sodium sulfate
H2SO4 (aq) + NaCl (s) --> NaHSO4 (s) + HCl (g)
H2SO4 (aq) + MgCl2 (s) --> Mg(HSO4)2(s) + HCl (g)
12.6.10 Prepare salts by chemical reactions
Salts can be prepared by the action of acids with alkalis, carbonates, metals, metal oxides, and by replacement and double decomposition reactions.
A salt contains a metal and part of an acid, e.g. copper sulfate from sulfuric acid, sodium chloride from hydrochloric acid.
A salt is a compound formed when the hydrogen of an acid is replaced by a metal.
For example, when zinc reacts with hydrochloric acid it replaces the hydrogen and forms the salt, zinc chloride.
The hydrogen comes away as hydrogen gas.
Zn + 2HCl --> ZnCl2 + H2.
Experiments
1. Add silver nitrate solution to sodium chloride solution.
A silver chloride precipitate forms that can be separated from the sodium nitrate solution.
AgNO3 (aq) + NaCl (aq) --> AgCl (s) + NaNO3 (aq)
silver nitrate + sodium chloride --> silver chloride + sodium nitrate
Be careful! Silver nitrate is expensive!
2. Add silver nitrate solution to potassium chloride solution.
A silver chloride precipitate forms that can be separated from the potassium chloride solution.
AgNO3 (aq) + KCl (aq) --> KNO3 (aq) + AgCl (s)
silver nitrate + potassium chloride --> silver chloride + potassium nitrate
Be careful! Silver nitrate is expensive!
9.2.2 Prepare oxalic acid
See diagram 16.4.3: Melting point of fat or oil
Ethanedioic acid-2-water, C2H2O4, oxalic acid, colourless crystals (HOOC-COOH.2H2O).
It occurs in many plants, e.g. rhubarb that can be used as a laxative.
Experiment
Be careful! This experiment must be done in a fume cupboard.
The reaction will be violent, so use very small quantities of chemical.
Add concentrated nitric acid to sucrose in a beaker.
The sucrose starts dissolving.
Heat the mixture in a fume cupboard.
All the sucrose gradually dissolves.
Meanwhile, the nitric acid decomposes to turn the solution yellow, and produces much white smoke.
With the temperature rise, solution colour becomes deeper and a large amount of reddish brown gas is released.
By controlling heating, evaporate the solution nearly to dryness, and volatilize the reddish brown gas as thoroughly as possible.
Cool the beaker in water and snowflake like crystals of ethanedioic acid-2-water (oxalic acid) appear.
Do not use an excessive quantity of nitric acid.
Otherwise, the time for heating would be overlong and the nitric acid would not decompose completely, leading to a yellow product.
sucrose + concentrated nitric acid --> dehydrated ethanedioic acid-2-water, (oxalic acid).
12.6.22 Prepare sodium carbonate
What was known "alkali", soda ash (sodium carbonate) and potash (potassium carbonate), were vital chemicals in the glass, textile, soap, and paper industries.
It could be obtained from potash, from wood ashes using the ashes of large northern forests, (Salicornia europoea), or from kelp.
It could also be obtained from Natron, (Na2CO3·10H2O, in dry lake beds.
The Leblanc process involved two stages:
1. Making sodium sulfate from sodium chloride.
Sodium chloride is mixed with concentrated sulfuric acid and the mixture exposed to low heat.
The hydrogen chloride gas bubbles off, leaving a fused mass.
H2SO4 (aq) + NaCl (s) --> HCl (g) + NaHSO4 (s)
This reaction produces sodium sulfate ("salt cake") and hydrogen chloride.
2NaCl + H2SO4 --> Na2SO4 + 2 HCl.
2. Reacting the sodium sulfate with coal and calcium carbonate to make sodium carbonate.
A mixture of the salt cake and crushed limestone (calcium carbonate) was reduced by heating with coal.
In this carbothermic reaction the coal, as a source of carbon, reduces the sulfate to sulfide.
Na2SO4 + 2 C --> Na2S + 2 CO2
In the second stage, is the reaction to produce sodium carbonate and calcium sulfide, ("black ash).
Na2S + CaCO3 --> Na2CO3 + CaS
The soda ash is extracted from the black ash with water.
Evaporation of this extract yields solid sodium carbonate.
The noxious calcium sulfide can be converted into calcium carbonate.
CaS (s) + CO2 (g) + H2O (l) --> CaCO3 (s) + H2S (g) This mass is heated, then heated with coal, then limestone. then washed, then carbon dioxide bubbled through it, then zinc hydroxe added, all done to remove impurities.
By the 1870s, the British soda output of 200,000 tons annually exceeded that of all other nations in the world combined.
Solvay process
It is a more direct process for producing soda ash from salt and limestone through the use of ammonia.
The Leblanc process plants were quite damaging to the local environment, because of the gases released leaving and insoluble smelly solid waste, which weathered to release hydrogen sulfide.
The Leblanc process remained more wasteful and more polluting than the Solvay process.
16.6.4.1H">16.6.4.1 Prepare ethane gas
Heat a mixture of sodium propionate and soda lime, and heat in a boiling tube.
Collect the gas by downward displacement of water.
C2H5COONa + NaOH -> N2CO3 + C2H6
9.2.1 Prepare ethanoic acid
Ethanoic acid (acetic acid, CH3COOH), is a weak acid.
Only a small proportion of it breaks into ions in aqueous solution, Ka = 1.76 × 10-5.
Put sodium acetate-3-water in a Pyrex test-tube.
Add 1 mL of concentrated sulfuric acid and heat gently.
Test any vapour with moist litmus paper - blue litmus turns red.
Cautiously smell the vapours and note the characteristic odour of acetic acid.
Ionization reaction, Ka = 1.76 × 10-5
CH3COOH + H2O <--> H3O+ + CH3COO-
However, although acetic acid is only partly dissociated in water, in a more basic solvent, e.g. liquid ammonia, it is completely dissociated.
CH3COOH + NH3 --> NH4+ + CH3COO-.
16.6.3 Prepare glucose with starch
Boil a 2 mL of starch with half a test-tube of dilute sulfuric acid or sodium hydrogen sulfate (sodium bisulfate), solution for two minutes.
Then pour off drops of the liquid into another test-tube, cool it under the tap, and test it by adding a drop of iodine solution.
The liquid turns red.
The starch has been changed into dextrin, a substance, which, like starch, is given the same formula.
In this case, however, z (number of amylose units) is supposed to be a much smaller number than for starch.
Continue boiling the remainder of the liquid for another three minutes to convert the dextrin into glucose.
To show that glucose has been formed, cool the liquid and neutralize it in an evaporating basin with dilute sodium carbonate or sodium hydroxide solution, (test with litmus paper).
Add 2 cm of the neutralized solution to a precipitate of copper hydroxide made from solutions of copper sulfate and sodium hydroxide.
If the test-tube is warmed, a yellow precipitate, which turns red, of cuprous oxide forms.
Dry heat breaks down starch to dextrins ("pyrodextrins") to give the brown colour of toast.
16.6.4 Prepare glucose with sugar
Boil a 2 mL of sugar in a test-tube with 2 cm of dilute sulfuric acid or sodium hydrogen sulfate (sodium bisulfate), solution.
Keep the liquid boiling for two or three minutes and then cool the test-tube under the tap.
To show that the solution now contains glucose, first neutralize the remaining acid with sodium carbonate or dilute sodium hydroxide solution, (test with litmus paper).
Then apply the copper hydroxide test.
16.1.2 Prepare gases from coal
Organic matter in a state of advanced decay, passes through the stages of compost and peat before becoming lignite (coal).
It is composed of a heterogenous mixture of compounds including phenolic radicals and acids that polymerize and are not easily separated nor analyzed.
When a substance is heated in the absence of air, its structure may be destroyed, so this process is called "destructive distillation".
Producer gas is a mixture of carbon monoxide and nitrogen.
Producer gas forms when air passes over hot coke or carbon.
2C (s) + O2 (g) + N2 --> 2CO (g) + N2 (g).
The mixture gases called coal gas forms when coal is heated strongly in the absence of air.
It is a slow process, which cannot be done in the school science laboratory.
Experiments
1. Use bituminous coal, because it contains mainly volatile hydrocarbons.
Grind the coal with a mortar and pestle.
Transfer 3-5 g of the crushed coal to the bottom of a sidearm test-tube.
Insert a stopper and clamp the sidearm test-tube with its side arm downwards and its mouth inclined down.
Connect the sidearm to a straight delivery tube inserted into a one-hole stopper in another sidearm test-tube.
Attach a glass tube to the sidearm of the second sidearm test-tube.
Heat the crushed coal in the upper test-tube with an alcohol lamp.
The heated coal decomposes to produce coal tar oil that flows down into the lower test-tube.
Hold a lighted match to the outlet of the glass tube to ignite volatile gas.
The gas burns with a light blue flame.
2. Grind bituminous coal with a mortar and pestle and put it in a Pyrex test-tube.
Fit the tube with a one-hole cork carrying a glass delivery tube.
Make a gas reservoir by punching two holes in the bottom of a large tin can.
Insert a one-hole stopper with a short glass tube in each hole.
Seal between the stopper and edge of the holes.
Use rubber tubing to connect one of the short glass tubes to the delivery tube.
Connect the other short tube to a medicine dropper tube and attach a screw type pinch clamp Hofmann clip to the rubber tubing.
Fill the can with water and invert it in a large jar of water so that it sinks to the bottom.
Heat the test-tube containing coal with a Meker burner.
The coal decomposes into several substances.
Gases from the decomposition leave the tube and fill the reservoir can by driving out the water.
As the can fills with gas, it rises in the large jar.
At first the coal gas pushes air out of the can through the second tube attached to the medicine dropper.
Close the Hofmann clip and collect the gas.
To test the gas, open the Hofmann clip and hold a lighted match to the end of the medicine dropper tube.
The gas burns until the contents of the tin can are almost exhausted.
Some volatile tar floats on the water in the can.
The remaining products of the destructive distillation, e.g. coke, remain in the test-tube.
16.6.4.1, Prepare butane
13.3.0: Prepare gases with gas generation apparatus
This experiment was called the "wet asbestos method", because asbestos wool was used to soak up the ethyl iodide in the test-tube.
However, asbestos wool is not allowed in schools.
Pour 2 cm ethyl iodide in a test-tube.
Add 5 g of copper turnings and push it down firmly with a spatula.
Set up the gas generation apparatus and heat the mixture.
2C2H5I + 2Cu --> C4H10 + Cu2I2
ethyl iodide + copper --> butane + copper (I) iodide

16.5.8 Prepare sugar crystals
Cut a length of string longer than the depth of a tall jar and wind the end around a pencil.
Attach a paper clip to the bottom of the string so that it hangs straight down 2 cm from the bottom of the tall jar.
Wet the string and roll it in granulated sugar and leave it to dry.
Slowly add one cup of sugar to three cups of water in a pan while stirring.
Heat the solution until it boils.
Be careful! The boiling point of a sugar solution < 100 oC!
Leave the sugar syrup to cool, then pour it into the tall jar.
Place the pencil with attached sugared string across the top of the tall jar.
In a few hour sugar crystals will start to form and will continue forming for days.
19.3.6 Prepare camphor oil
1. Crush camphor cake.
Add salad oil, 5 mL eucalyptus oil, and a few drops of turps.
Put ingredients in a small bottle.
Put bottle in saucepan containing water.
Slowly bring water to boil.
Use camphor oil when cool.
19.3.7 Prepare soap
1. Add to a tin can half full with water, 2.27 kg dripping (animal fat) free from salt, 0.45 kg resin.
Boil for 30 minutes then add 1 tablespoon borax or kerosene and 0.45 kg caustic soda.
When bubbling stops (from adding the caustic soda) boil for two hours.
Leave in tin for two days then cut into slabs with a tight wire.
BE CAREFUL! Add caustic soda gradually to avoid boiling over!
19.3.8 Prepare preserving agents for cut flowers
The bacteria in water will rot the cuts on stems of cut flowers, causing the block of capillaries, a decline in water absorbability and the deficiency in biogenic nutrition, and finally withering up the flowers.
Water with a certain amount of a preservative agent added can prolong the life of cut flowers.
Preservative agents usually contain the following:
1. Nutritious substances: Sucrose and oxime are usually used.
Both serve as source of energy and bring stomas to shut up to weaken transpiration.
2. Bactericide: Silver nitrate, copper (II) sulfate or sodium hypochlorite can be used.
3. Ethylene inhibitor: Silver nitrate or silver thiosulfate is commonly used.
4. Acidified water: The pH value is kept to 3 to 4.
Also, people crush the ends of the stems of cut flowers and put concentrated sugar solution or vodka into the flower vase.
Experiments
1. Use a small quantity of alcohol and water to dissolve 0.1 g of oxime in a large beaker and then pour more water in to dilute he solution to 500 mL (the mass percentage of oxime is about 0.02%).
Add a few drops of dilute sulfuric acid to adjust the pH value of the solution to pH 5 to pH 6.
While stirring, dissolve 0.025 g of silver nitrate (the mass percentage is about 0.005%) and 10 g of sucrose.
After mixing this prepared preservative solution, use it for cut flowers.
2. Test quality of the preserving agent for cut flowers.
Pour 500 mL of tap water into another large beaker.
Put the same number of cut flowers as those in the above experiment in the water.
Under the same conditions make a comparison, every three days, about the number of flowers and the water absorbing quantity.
Pour 500 mL of tap water into another large beaker.
Put the same number of cut flowers in the water.
Under the same conditions, make a comparison, every three days, between the two cases about the number of flowers and the water-absorbing quantity.
3. Some people claim that the best preservative for cut flowers is a solution of 11/2 teaspoons of sucrose in 200 mL of water.
Other people recommend a very dilute solution of household bleach.
4. Dissolve small amounts of ammonium chloride, potassium nitrate, and sodium carbonate or camphor in water.
These substances are supposed to keep flowers from losing their turgidity by stimulating cells and preventing growth of bacteria.
Wilted flowers may revive if the cut stems are placed in a dilute solution of camphor.