CHEMISTRY PRACTICALS CLASS XII SESSION – 2023-24 Designed By SARWAN KUMAR PGT CHEMISTRY KV NO. 1 AJMER EXPERIMENT ­ 1 AIM - To prepare M/20 solution of Mohr’s salt and, using this solution find out the molarity and strength of the given potassium permanganate (KMnO4) solution. THEORY –Mohr’s salt titration with potassium permanganate is also a redox titration. In this titration, Mohr’s salt acts as a reducing agent and potassium permanganate works as the oxidising agent. MOLECULAR EQUATIONS ­ REDUCTION HALF REACTION - 2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5O OXIDATION HALF REACTION - (FeSO4(NH4)2SO4.6H2O +H2SO4 +O→ Fe2(SO4)3 + 2(NH4)2SO4 +13H2O) x 5 ---------------------------------------------------------------------------OVERALL REACTION2KMnO4+10FeSO4(NH4)2SO4.6H2O+8H2SO4→K2SO4+2MnSO4+5Fe2(SO4)3+10(NH4)2SO4+68H2O IONIC REACTIONS – Oxidation half – [Fe2+→Fe3+ + e-]5 Reduction half - MnO4- + 8H+ + 5e- → Mn2++4H2O Overall equation - MnO4- + 8H++5Fe2+→ Mn2+ + 5Fe3+ + 4H2O MATERIALS REQUIRED ­ APPARATUS REQUIRED – weighing bottle, weight box, volumetric flask, conical flask, burette, pipette, clamp stand, chemical balance, beakers, burette stand, funnel, measuring flask, white tile, burnet and wire gauge. distilled water, dilute sulphuric acid, potassium permanganate solution. INDICATOR – KmnO4 is a self indicator. END POINT -- colour change of KMnO4 from colourless to light pink. PROCEDURE A. Preparation of 250ml of M/20 solution of Mohr’s salt – 1. weigh 4.9g of Mohr’s salt using a chemical balance and watch glass. 2. dissolve weighed Mohr’s salt conc H2SO4 (5 ml) and 100 ml distilled water in a beaker. Dissolve the salt and pour in into in 250 ml volumetric flask. Now fill the volumetric flask with distilled water according to the required volume. B. Titrating potassium permanganate solution against standard ferrous ammonium sulphate (Mohr’s salt) 1. Wash the pipette and the burette with distilled water and then rinse burette with KMnO4 and pipette with Mohr salt solution. 2. Fill the burette with potassium permanganate solution. Fix the burette in the burette stand. 3. Take out 20 ml of standard more Mohr salt solution in the conical flask. Add 10ml of sulfuric acid to prevent the oxidation of manganese to form manganese dioxide. 4. Note the initial reading of the burette before starting that experiment. 5. Now against the potassium permanganate solution start the titration and slowly still the flask gently. 6. Initially, the purple colour of KMnO4 will be discharged with ferrous ammonium sulphate. The appearance of the permanent pink colour indicates the endpoint. Repeat the for 3 time unless Concordant value is obtained. CALCULATION: For Mohr salt preparation molarity Molarity = Given mass x 1000 Molar mass x V ! "# X = $ & '((( )*+ & '(( !"# % & % #' = &' = 1.96 g. Part -A. Molarity of KMnO4 From the balanced ionic equation 1 mole KMnO4 is reacting with 5 mole of mohr’s salt solution. M KMnO4 x V KMnO4 & MMohr x V Mohr = ( MKMnO4 x 20.0 ml 0.05 x 20.0 = & ( OBSERVATION TABLE: The volume of Mohr’s salt solution taken – 20ml. (by Pippette) Burette Reading The volume of KMnO4 S.No. used in ml Initial Final 1. 2. 3. 0 ml 0 ml 0 ml 19.9 ml 20.0 ml 20.0 ml 19.9 ml 20.0 ml 20.0 ml RESULT – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l MKMnO4 = 0.01 M Part -B Strength of KMnO4 solution = Molarity x Molar mass = 0.01 x 158u = 1.58 g/l Result – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l PRECAUTIONS – 1. Always rinse the burette and pipette before use. 2. Clean all apparatus with distilled water. 3. Use dilute H2SO4 acid in the experiment. 4. Strength of KMnO4 solution should be taken at least 2 decimal. 5. Don’t use a rubber cork burette as it is can be attacked by KMnO4. Concordant Value 20.0 ml EXPERIMENT ­ 2 AIM - To prepare M/30 solution of Mohr’s salt and, using this solution find out the molarity and strength of the given potassium permanganate (KMnO4) solution. THEORY –Mohr’s salt titration with potassium permanganate is also a redox titration. In this titration, Mohr’s salt acts as a reducing agent and potassium permanganate works as the oxidising agent. MOLECULAR EQUATIONS ­ REDUCTION HALF REACTION - 2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5O OXIDATION HALF REACTION - (FeSO4(NH4)2SO4.6H2O +H2SO4 +O→ Fe2(SO4)3 + 2(NH4)2SO4 +13H2O) x 5 ---------------------------------------------------------------------------OVERALL REACTION2KMnO4+10FeSO4(NH4)2SO4.6H2O+8H2SO4→K2SO4+2MnSO4+5Fe2(SO4)3+10(NH4)2SO4+68H2O IONIC REACTIONS – Oxidation half – [Fe2+→Fe3+ + e-]5 Reduction half - MnO4- + 8H+ + 5e- → Mn2++4H2O Overall equation - MnO4- + 8H++5Fe2+→ Mn2+ + 5Fe3+ + 4H2O MATERIALS REQUIRED ­ APPARATUS REQUIRED – weighing bottle, weight box, volumetric flask, conical flask, burette, pipette, clamp stand, chemical balance, beakers, burette stand, funnel, measuring flask, white tile, burnet and wire gauge. distilled water, dilute sulphuric acid, potassium permanganate solution. INDICATOR – KmnO4 is a self indicator. END POINT -- colour change of KMnO4 from colourless to light pink. PROCEDURE A. Preparation of 250ml of M/20 solution of Mohr’s salt – 1. weigh 4.9g of Mohr’s salt using a chemical balance and watch glass. 2. dissolve weighed Mohr’s salt conc H2SO4 (5 ml) and 100 ml distilled water in a beaker. Dissolve the salt and pour in into in 250 ml volumetric flask. Now fill the volumetric flask with distilled water according to the required volume. B. Titrating potassium permanganate solution against standard ferrous ammonium sulphate (Mohr’s salt) 1. Wash the pipette and the burette with distilled water and then rinse burette with KMnO4 and pipette with Mohr salt solution. 2. Fill the burette with potassium permanganate solution. Fix the burette in the burette stand. 3. Take out 20 ml of standard more Mohr salt solution in the conical flask. Add 10ml of sulfuric acid to prevent the oxidation of manganese to form manganese dioxide. 4. Note the initial reading of the burette before starting that experiment. 5. Now against the potassium permanganate solution start the titration and slowly still the flask gently. 6. Initially, the purple colour of KMnO4 will be discharged with ferrous ammonium sulphate. The appearance of the permanent pink colour indicates the endpoint. Repeat the for 3 time unless Concordant value is obtained. CALCULATION: For Mohr salt preparation molarity Molarity = Given mass x 1000 Molar mass x V ! ,# X = $ & '((( )*+ & '(( !"# % & % !' = &' = 1.3 g. Part -A. Molarity of KMnO4 From the balanced ionic equation 1 mole KMnO4 is reacting with 5 mole of mohr’s salt solution. M KMnO4 x V KMnO4 & MMohr x V Mohr = ( MKMnO4 x 12.0 ml 0.03 x 20.0 = & ( OBSERVATION TABLE: The volume of Mohr’s salt solution taken – 20ml. (by Pippette) Burette Reading The volume of KMnO4 S.No. used in ml Initial Final 1. 2. 3. 0 ml 0 ml 0 ml 11.9 ml 12.0 ml 12.0 ml 11.9 ml 12.0 ml 12.0 ml RESULT – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l MKMnO4 = 0.01 M Part -B Strength of KMnO4 solution = Molarity x Molar mass = 0.01 x 158u = 1.58 g/l Result – Molarity of given KMnO4 solution 0.01M Strength 1.58 g/l PRECAUTIONS – 1. Always rinse the burette and pipette before use. 2. Clean all apparatus with distilled water. 3. Use dilute H2SO4 acid in the experiment. 4. Strength of KMnO4 solution should be taken at least 2 decimal. 5. Don’t use a rubber cork burette as it is can be attacked by KMnO4. Concordant Value 12.0 ml AIM- To prepare M/50 solution of oxalic acid .Using this solution find out the molarity and strength of the given potassium permanganate (KMnO4) solution. EXPERIMENT ­ 3 AIM- To prepare M/50 solution of oxalic acid .Using this solution find out the molarity and strength of the given potassium permanganate (KMnO4) solution. THEORY –Oxalic acid titration with potassium permanganate is also a redox titration. In this titration, Oxalic acid acts as a reducing agent and potassium permanganate works as the oxidising agent. MOLECULAR EQUATIONS ­ REDUCTION HALF REACTION 2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5[O] OXIDATION HALF REACTION (COOH)2.2H2O +[O]→ 2CO2 + 3H2O )x 5 ---------------------------------------------------------------------------OVERALL REACTION2KMnO4 + (COOH)2.2H2O + 3H2SO4 → K2SO4 +2MnSO4 + 10CO2 +18H2O IONIC REACTIONS – OXIDATION HALF – [C2O42-→2CO2 + e-]5 REDUCTION HALF MnO4- + 8H++5e- → Mn2++4H2O} X 2 OVERALL EQUATION - 2MnO4-+ 16H+ + 5 C2O42-→ 2 Mn2+ + 10CO2 + 8H2O MATERIALS REQUIRED ­ Apparatus Required – weighing bottle, weight box, volumetric flask, conical flask, burette, pipette, clamp stand, chemical balance, beakers, burette stand, funnel, measuring flask, white tile, burnet and wire gauge. distilled water, dilute sulphuric acid, potassium permanganate solution. Indicator – KMnO4 is a self-indicator. End point - Colour change of KMnO4 from colourless to light pink. PROCEDURE A. Preparation of 250ml of M/50 solution of Oxalic acid – 1. weigh 0.63g of Oxalic acid using a chemical balance and watch glass. 2. dissolve weighed Oxalic acid in con H2SO4(5 ml) and 100 ml distilled water in a beaker. Dissolve the salt and pour in into in 250 ml volumetric flask. Now fill the volumetric flask with distilled water according to the required volume. B. Titrating potassium permanganate solution against standard ferrous ammonium sulphate (Mohr’s salt) 1. Wash the pipette and the burette with distilled water and then rinse burette with KMnO4 and pipette with Oxalic acid salt solution. 2. Fill the burette with potassium permanganate solution. Fix the burette in the burette stand. 3. Take out 20 ml of standard Oxalic acid salt solution in the conical flask. Add 10ml of sulphuric acid to prevent the oxidation of manganese to form manganese dioxide. 4. Note the initial reading of the burette before starting that experiment. 5. Now against the potassium permanganate solution start the titration and slowly still the flask gently. CALCULATION: part -A. Molarity of KMnO4 From the balanced ionic equation 2 mole KMnO4 is reacting with 5 mole of Oxalic acid salt solution. ! MKMnO4 x VKMnO4 =" M Oxalic acid x VOxalic acid MKMnO4 x 8.0 ml 0.05 x 10.0 = 2 5 MKMnO4 = 2 x 10.0 x 0.05 8.0 x 5 MKMnO4 = 0.025 M Part -A Strength of KMnO4 solution = Molarity x Molar mass = 0.025 x 158u = 3.95 g/l Result – Molarity of given KMnO4 solution 0.025 M Strength 3.95 g/l 6. Initially, the purple colour of KMnO4 will be discharged with ferrous ammonium sulphate. The appearance of the permanent pink colour indicates the endpoint. Repeat for 3 time unless Concordant value is obtained. OBSERVATION TABLE: The volume of Oxalic acid salt solution taken – 10ml. (by Pippette), M S.N. .lo9;; 2. 3. Burette Reading Initial Final 0 ml 0 ml 0 ml 7.89 ml 8.00 ml 8.00 ml The volume of KMnO4 used in ml 7.89 ml 8.00 ml 8.00 ml Concordant Value 8.00 ml RESULT – Strength of KMnO4 solution = Molarity x Molar mass = 0.025 x 158u = 3.95 g/l Molarity of given KMnO4 solution 0.025 M Strength 3.95 g/l PRECAUTIONS – 1. Always rinse the burette and pipette before use. 2. Clean all apparatus with distilled water. 3. Use dilute H2SO4 acid in the experiment. 4. Strength of KMnO4 solution should be taken at least 2 decimal. 5. Don’t use a rubber cork burette as it is can be attacked by KMnO4. AIM- IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – A RESULT – The experimental observation shows the presence of Alcoholic group – OH . Equations – ( write on white side of paper) a) C2H5OH + Na → C2H5ONa + ½ H2 b) C2H5OH + (NH4)2Ce (NO3)6→ (C2H5OH)2Ce (NO3)4 + (NH4)2NO3 c) C2H5OH + CH3COOH → CH3COO C2H5 + H2O EXPERIMENT -04 AIM- IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – A PART- A - PHYSICAL PROPERTIES a. Colour - colourless b. Odour – order of sprit or wine c. Solubility in Water - soluble in water d. Solubility in dil HCl – soluble in Dil Hcl PART- B - CHEMICAL PROPERTIES S.N. 1. Experiment Observation Inference Unsaturation test- To the given KMnO4 get organic compound add alkaline decolourised KMnO4 solution Test for carboxylic group- Add a No CO2 evolve pinch of NaHCO3 to the given sample Compound is saturated (-) 3 Litmus Test – Put a drop of sample on blue litmus and red litmus No change is observed 4. Test for phenol – to the given sample add 2- 3 ml of Neutral FeCl3 soln Sodium metal test- drop a piece of dried sodium in the given sample . NO VOILET PPT obtained Alcoholic or carboxyl group is absent Phenolic group absent Ceric ammonium nitrate test- Add the drops of ceric ammonium nitrate solution to the given sample Red PPT formation 2. 5 6 Evolution colourless gas Carboxylic group absent of Alcoholic group – OH confirm Alcoholic group – OH confirm 7 Ester test- to the 1 ml of given Fruity smell Alcoholic group – sample add 1 ml acetic acid and few OH confirm drops of Con. H2SO4 and heat on water bath RESULT – The experimental observation shows the presence of Alcoholic group – OH . Equations – ( write on white side of paper) a) C2H5OH + Na → C2H5ONa + ½ H2 b) C2H5OH + (NH4)2Ce (NO3)6→ (C2H5OH)2Ce (NO3)4 + (NH4)2NO3 c) C2H5OH + CH3COOH → CH3COO C2H5 + H2O AIM -IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – B EXPERIMENT - 05 RESULT – The experimental observation shows the presence of Phenolic group AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – B Ar-OH confirmed PART- A - PHYSICAL PROPERTIES a. Colour - colourless b. Odour – order of sprit or wine c. Solubility in Water - soluble in water d. Solubility in dil HCl – soluble in Dil Hcl EQUATIONS – (write on white side of paper) a) C6H5OH + FeCl3 b) → [(C6H5O) 6Fe]3- + 3HCl PART- B - CHEMICAL PROPERTIES S.N. Experiment 1. 2. 3. 4. 5. Observation Inference Unsaturation test- To the given organic compound add alkaline KMnO4 solution Test for carboxylic group- Add a pinch of NaHCO3 to the given sample Litmus Test – Put a drop of sample on blue litmus and red llitmus KMnO4 get decolourised Compound is saturated (-) No CO2 evolve Test for phenol – to the given sample add 2- 3 ml of Neutral FeCl3 soln Azo dye test:-Compound + NaNO2 + conc. HCl and add aniline VOILET PPT obtained Carboxylic group absent Alcoholic or carboxyl group is absent Phenolic group confirm No change is observed Orange red dye Phenolic group confirmed RESULT – The experimental observation shows the presence of Phenolic group Ar-OH confirmed Equations – (write on white side of paper) a) C6H5OH + FeCl3 b) → [(C6H5O) 6Fe]3- + 3HCl AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – C RESULT – The experimental observation shows the presence of aldehyde group -CHO confirmed. EQUATION - EXPERIMENT - 06 AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – C PART- A - PHYSICAL PROPERTIES a. Colour - colourless b. Odour – order of sprit or wine c. Solubility in Water - soluble in water d. Solubility in dil HCl – soluble in Dil Hcl PART- B - CHEMICAL PROPERTIES S.N. Experiment Observation 1. 2. 3 4. 5. 6. 7. Unsaturation test- To the given organic compound add alkaline KMnO4 solution Litmus Test – Put a drop of sample on blue litmus and red llitmus Test for carboxylic group- Add a pinch of NaHCO3 to the given sample Test for phenol – to the given sample add 2- 3 ml of Neutral FeCl3 soln Test for carbonyl group – Add 1 ml of sample add 2-3 ml of 2,4 DNP (dinitro phenylhydrazine) Test for aldehyde group: Added 1ml Fehling solution to given organic compound & heated on water bath. Added Tollen’s reagent to organic compound and warm it in water bath KMnO4 get decolourised Inference Compound is saturated (-) No change is observed Alcoholic or carboxyl group is absent No CO2 evolve Carboxylic group absent NO VOILET PPT obtained Phenolic group absent. Orange yellow Carbonyl group may ppt formed be an aldehyde or ketone. Red ppt formed -CHO group confirmed Silver mirror on -CHO group inside wall of confirmed the test tube RESULT – The experimental observation shows the presence of aldehyde group -CHO confirmed. EQUATION - AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – D RESULT – The experimental observation shows the presence of ketonic group > C=O confirmed. EXPERIMENT - 07 AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – D PART- A - PHYSICAL PROPERTIES a. Colour - colourless b. Odour – order of sprit or wine c. Solubility in Water - soluble in water d. Solubility in dil HCl – soluble in Dil Hcl EQUATION - PART- B - CHEMICAL PROPERTIES S.N. Experiment 1. Observation Inference Unsaturation test- To the given KMnO4 get Compound is organic compound add alkaline decolourised saturated (-) KMnO4 solution 2. Test for carboxylic group- Add a No CO2 Carboxylic group pinch of NaHCO3 to the given evolve absent sample 3 Litmus Test – Put a drop of sample No change is Alcoholic or carboxyl on blue litmus and red llitmus observed group is absent 4. Test for phenol – to the given NO VOILET Phenolic group sample add 2- 3 ml of Neutral FeCl3 PPT obtained absent. soln 5. Test for carbonyl group – Add 1 ml Orange Carbonyl group may of sample add 2-3 ml of 2,4 DNP yellow ppt be an aldehyde or (dinitro phenylhydrazine) formed ketone. 6. Test for Ketonic group: Added 1 Red colour Ketonic group appeared confirmed ml sodium nitroprusside solution to given organic Compound & then added NaOH solution dropwise 7. Add 1ml finely powdered mViolet Ketonic group colour confirmed dintrobenzene to given organic appeared Compound & then added NaOH soln. RESULT – The experimental observation shows the presence of ketonic group > C=O confirmed. AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – E EXPERIMENT - 08 AIM-IDENTIFY THE FUNCTIONAL GROUP FROM GIVEN SAMPLE – E RESULT – The experimental observation shows the presence of Carboxylic group – COOH . PART- A - PHYSICAL PROPERTIES Equations:- a)CH3COOH + Na2CO3 → CH3COO Na + H2O +CO2 a. Colour - colourless b. Odour – order of sprit or wine c. Solubility in Water - soluble in water d. Solubility in dil HCl – soluble in Dil Hcl b) C2H5OH + CH3COOH → CH3COO C2H5 + H2O. PART- B - CHEMICAL PROPERTIES S.N. Experiment 1 2 3 4 Unsaturation test- To the given organic compound add alkaline KMnO4 solution Litmus Test – Put a drop of sample on blue litmus and red llitmus Test for carboxylic group: a.- Sodium bi carbonate test: Added a pinch of NaHCO3 to small amount of Organic compound b.- Ester test: Added ethanol to organic Compound and then added 2-3 drops of conc. H2SO4 to it and warmed in water bath for few min Observation Inference KMnO4 get decolourised Compound is saturated (-) change is observed, blue litmus turn red Effervescence with evolution of colour less and odourless gas which turns lime water milky Pleasant fruity smell Alcoholic or carbonyl group may be present Carboxylic group present Carboxylic group present RESULT – The experimental observation shows the presence of Carboxylic group – COOH . Equations:- a)CH3COOH + Na2CO3 → CH3COO Na + H2O +CO2 b) C2H5OH + CH3COOH → CH3COO C2H5 + H2O. AIM- To detect one cation and one anion radical from given salt RESULT- The given salt is NH4 Cl in which NH4+ is cation and Cl- as anion radical EXPERIMENT - 09 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- NH4+ may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TESTS.N. EXPERIMENT OBSERVATION 1 Heat a pinch of No redish brown gas salt in dry test Sublimation occurs tube No crackling sound INFERENCE NO3- absent Halide may be present Pb(NO3)2 may be absent B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT 1. Dil H2SO4 test Take a pinch of salt in a test tube add Dil H2SO4 OBSERVATION No effervasence of CO2 No rotten egg smell of H2S No S02 gas ( turn K2Cr2O7 green) No reddish Brown gas make FeSO4 solution black HCl gas (suffocating smell) Give white PPT with AgNO3 (soluble in NH4OH) 2. Conc. H2SO4 test Take a pinch of salt in a test tube add Conc H2SO4 3. CONFIRMATORY TEST a.To the salt solution add White PPT – soluble in NH4OH conc HNO3 and AgNO3 soln b.To the salt add MnO2 and Cl2 gas evolves Conc H2SO4 and heat . Red vapours- add NaOH ( yellow c.Salt + solid K2Cr2O7 + solution obtained) add acetic acid Conc H2SO4 & heat & lead acetate - Yellow PPT INFERENCE CO32- absent S2- absent SO32- absent NO2- absent Cl- may be present Cl- Confirm Cl- Confirm Cl- Confirm C. TEST FOR BASIC RADICAL 1. 2. 3. To the salt solution add NaOH solution and heat Bring a glass rod dipped in Dil HCl over the test tube Smell of ammonia Add Nessler’s reagent Brown PPT formed White fumes appears NH4+ may be present NH4+ may be present NH4+ confirm RESULT- The given salt is NH4 Cl in which NH4+ is cation and Cl- as anion radical AIM- To detect one cation and one anion radical from given salt RESULT- The given salt has NH4+ is cation and C2O42- as anion radical EXPERIMENT - 10 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- NH4+ may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TESTS.N. EXPERIMENT 1 Heat a pinch of salt in dry test tube OBSERVATION No redish brown gas Sublimation not occurs No crackling sound INFERENCE NO3- absent Halide may be absent Pb(NO3)2 may be absent B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT OBSERVATION 1. Dil H2SO4 test No effervasence of CO2 No Take a pinch of salt in a test rotten egg smell of H2S tube add Dil H2SO4 No S02 gas ( turn K2Cr2O7 green) No reddish Brown gas make FeSO4 solution black INFERENCE CO32- absent S2- absent SO32- absent NO2- absent 2. Conc. H2SO4 test Colorless odourless gas (CO2) Take a pinch of salt in a test tube add Conc H2SO4 C2O42-(oxalate) may be present 3. CONFIRMATORY TEST a.To the salt solution add acetic acid and calcium chloride C2O42-(oxalate) Confirm White PPT Pink colour of KMnO4 discharged C2O42-(oxalate) Confirm Dil H2SO4 and warm add 23 drops of KMnO4 solution b.To the salt solution add C. TEST FOR BASIC RADICAL 1. To the salt solution add Smell of ammonia NaOH solution and heat 2. Bring a glass rod dipped in White fumes appears Dil HCl over the test tube NH4+ may be present NH4+ may be present 3. NH4+ confirm Add Nessler’s reagent Brown PPT formed RESULT- The given salt has NH4+ is cation and C2O42- as anion radical AIM- To detect one cation and one anion radical from given salt. RESULT- The given salt is has Pb++ is cation and NO3- as anion radical. EXPERIMENT - 11 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- No characteristic pungent smell- NH4+ may be absent SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TESTS.N. EXPERIMENT 1 Heat a pinch of salt in dry test tube OBSERVATION Reddish brown gas NO Sublimation occurs Crackling sound INFERENCE NO3- may be present Halide may be absent Pb(NO3)2 may be present B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT 1. Dil H2SO4 test Take a pinch of salt in a test tube add Dil H2SO4 2. Conc. H2SO4 test Take a pinch of salt in a test tube add Conc H2SO4 3. CONFIRMATORY TEST a.To the salt solution add conc H2SO4 and Cu chipps then heat. b.To the salt solution add FeSO4 soln and Conc H2SO4 by the side of test tube . C. TEST FOR BASIC RADICAL 1. To the salt solution add NaOH solution and heat 2. To the salt add dil HCl 3. CONFIRMATORY TEST To the above solution I. add KI soln (one part) II. add K2CrO4 soln OBSERVATION No effervasence of CO2 No rotten egg smell of H2S No S02 gas ( turn K2Cr2O7 green) No reddish Brown gas make FeSO4 solution black NO2 gas (reddish brown)- turn FeSO4 solution black INFERENCE CO32- absent S2- absent SO32- absent NO2- absent Reddish brown gas NO3- Confirm Dark brown ring NO3- Confirm No Smell of ammonia Zero group NH4+ absent Pb++ may be present White PPT NO3- may be present Yellow PPT formed Pb++ confirm Yellow PPT formed Pb++ confirm RESULT- The given salt is has Pb++ is cation and NO3- as anion radical. AIM- To detect one cation and one anion radical from given salt. RESULT- The given salt is (CH3COO)2Pb in which Pb++ is cation and CH3COO- as anion radical EXPERIMENT - 12 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- CH3COO- may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TESTS.N. EXPERIMENT 1 Heat a pinch of salt in dry test tube OBSERVATION No redish brown gas Sublimation not occurs No crackling sound INFERENCE NO3- absent Halide may be absent Pb(NO3)2 may be absent B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT 1. Dil H2SO4 test Take a pinch of salt in a test tube add Dil H2SO4 2. Conc. H2SO4 test Take a pinch of salt in a test tube add Conc H2SO4 3. CONFIRMATORY TEST To the solid salt add oxalic acid and 2-3 drops of water- Rub with finger ESTER TEST- To the salt solution add ethanol and Conc H2SO4 and heat C. TEST FOR BASIC RADICAL 1. To the salt solution add NaOH solution and heat 2. To the salt add dil HCl 3. CONFIRMATORY TEST To the above solution I. add KI soln (one part) II. add K2CrO4 soln OBSERVATION No effervasence of CO2 No rotten egg smell of H2S No S02 gas ( turn K2Cr2O7 green) No reddish Brown gas make FeSO4 solution black Colorless vapours of vinegar smell Vinegar smell Fruity smell of ester No Smell of ammonia White PPT INFERENCE CO32- absent S2- absent SO32- absent NO2- absent CH3COO(acetate) may be present CH3COO(acetate) Confirm CH3COO(acetate) Confirm Zero group NH4+ absent Pb++ may be present Yellow PPT formed Pb++ confirm Yellow PPT formed Pb++ confirm RESULT- The given salt is (CH3COO)2Pb in which Pb++ is cation and CH3COO- as anion radical AIM- To detect one cation and one anion radical from given salt RESULT- The given salt is NH4 (CO3)2 in which NH4+ is cation and CO32- as anion radical EXPERIMENT - 13 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- NH4+ may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TESTS.N. EXPERIMENT OBSERVATION INFERENCE May be CO32- present 1 Heat a pinch of Colourless odourless gas which turns lime water milky salt in dry test tube No Sublimation occurs Halide absent No crackling sound Pb(NO3)2 may be absent B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT OBSERVATION 1. Dil H2SO4 test Effervesence of CO2, Take a pinch of salt in a test which turns lime water milky tube add Dil H2SO4 2. CONFIRMATORY TEST a.To the salt solution add Dil INFERENCE CO32- may be present CO2 Gas evolved with brisk effervescence CO32- Confirm White PPT CO32- Confirm HCl b.To the salt solution add MgSO4 solution. C. TEST FOR BASIC RADICAL 1. To the salt solution add Smell of ammonia NaOH solution and heat NH4+ may be present 2. Bring a glass rod dipped in Dil HCl over the test tube White fumes appears NH4+ may be present 3. Add Nessler’s reagent Brown PPT formed NH4+ confirm RESULT- The given salt is NH4 (CO3)2 in which NH4+ is cation and CO32- as anion radical AIM- To detect one cation and one anion radical from given salt RESULT- The given salt has Al2 (SO4)3 in which A+++ is cation and SO42- as anion radical EXPERIMENT - 14 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- NH4+ may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TESTS.N. EXPERIMENT OBSERVATION INFERENCE 1 Heat a pinch of salt in No redish brown gas NO3- absent dry test tube Sublimation not occurs Halide may be absent No crackling sound Pb(NO3)2 may be absent B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT OBSERVATION Dil H2SO4 test No effervescence of CO2 1. Take a pinch of salt in a test tube add Dil H2SO4 No rotten egg smell of H2S No S02 gas ( turn K2Cr2O7 green) No reddish Brown gas make FeSO4 soln black 2. Conc. H2SO4 test Take a pinch of salt in a test tube add Conc H2SO4 3. Special group test Add dil HCl and filter add BaCl2 No Colorless odourless gas (CO2) No smell of vinegar No colourless pungent smell gas No brown colour gas of pungent smell No voilet vapour of pungent smell No reddish brown gas of pungent smell White PPT C. TEST FOR BASIC RADICAL 1. To the salt solution add NaOH solution INFERENCE CO32- absent S2- absent SO32- absent NO2- absent C2O42-absent CH3COO- absent Cl- absent Br- absent I- absent SO42-(sulphate) Confirm No Smell of ammonia NH4+ is absent (group 0 absent) 2. To the salt solution add Dil HCl No White PPT appears 3. Pass H2S gas to above solution No Black PPT formed or any PPT White PPT formation Pb++ is absent (group 1 absent) Cu++ , Pb++ absent (group 2nd absent) Al+++ may be present and heat 4. To the salt solution add solid NH4Cl, Con HNO3, and NH4OH till smell of NH3 5. To the white PPT add dil HCl few drops of Blue litmus + NH4OH soln in excess A white PPT (suspended Al+++ may be present in colourless medium) called a lake, RESULT- The given salt has Al2 (SO4)3 in which A+++ is cation and SO42- as anion radical AIM- To detect one cation and one anion radical from given salt RESULT- The given salt is Sr(NO3)2 in which Ba ++ is cation and SO42- as anion radical EXPERIMENT - 15 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- NH4+ may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TEST- S.N. EXPERIMENT OBSERVATION INFERENCE 1 Heat a pinch of salt in Reddish brown gas NO3- may be present dry test tube NO Sublimation occurs Halide may be absent B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT OBSERVATION INFERENCE 1. Dil H2SO4 test Take a No effervasence of CO2 CO32- absent pinch of salt in a test No rotten egg smell of H2S S2- absent tube add Dil No SO2 gas ( turn K2Cr2O7 green) No SO32- absent reddish Brown gas make FeSO4 black H2SO4 NO - absent 2 No Colorless odourless gas (CO2) No smell of vinegar No colourless pungent smell gas No brown colour gas of pungent smell No voilet vapour of pungent smell No reddish brown gas of pungent smell 3. Special group test White PPT obtained a. To the salt add dil HCl and filter. To the filtrate add BaCl2 C. TEST FOR BASIC RADICAL 1. To the salt solution add NaOH No Smell of ammonia solution and heat 2. To the salt solution add Dil No White PPT appears HCl 3. Pass H2S gas to above No Black PPT formed or any PPT solution 4. To the salt solution add No change is observed NH4Cl and NH4OH in excess 5 Pass the H2S gas to above soln No change is observed C2O42-absent CH3COO- absent Cl- absent Br- absent I- absent 6 (group 5th present) Ba2+,Sr2+Ca2+may be prsent 2. Conc. H2SO4 test Take a pinch of salt in a test tube add Conc H2SO4 To the salt solution add solid NH4Cl , NH4OH , (NH4)CO3 White PPT formation SO42- (sulphate) Confirm NH4+ is absent (group 0 absent) Pb++ is absent (group 1 absent) Cu++ , Pb++ etc absent (group 2nd ) (group 3nd absent) Al3+, Fe3+ absent (group 4th absent) Zn2+,NI2+,Co2+ abs. 7 Dissolve the white PPT in CH3COOH and make it 2 parts 8 PART – A + K2CrO4 soln YELLOW PPT formed Ba2+ Confirmed 9 Performed Flame test grassy green flame Ba2+ confirmed Result- The given salt is Sr(NO3)2 in which Ba ++ is cation and SO42- as anion radical AIM- To detect one cation and one anion radical from given salt RESULT- The given salt is Sr(NO3)2 in which Sr++ is cation and NO3- as anion radical EXPERIMENT - 16 AIM- To detect one cation and one anion radical from given salt A. PHYSICAL EXAMINATION COLOUR- White and Crystalline – Cu++,Ni++,Fe+++, Fe++, Mn++, Co++ Ni++ absent ODOUR- characteristic pungent smell- NH4+ may be present SOLUBILITY- Soluble in water , Soluble in Dil. HCl DRY HEATING TEST- S.N. EXPERIMENT OBSERVATION 1 Heat a pinch of salt in Reddish brown gas dry test tube NO Sublimation occurs B. TEST FOR ACIDIC RADICAL S.N. EXPERIMENT Dil H2SO4 test 1. 2. 3. INFERENCE NO3- may be present Halide may be absent OBSERVATION CONFIRMATORY TEST a.To the salt solution add conc H2SO4 and Cu chipps then heat. b.To the salt solution add FeSO4 soln and Conc H2SO4 by the side of test tube . CO32- absent S2absent SO32- absent NO2absent NO3- may be present Reddish brown gas NO3- Confirm Dark brown ring NO3- Confirm C. TEST FOR BASIC RADICAL To the salt solution add NaOH 1. No Smell of ammonia 2. solution and heat To the salt solution add Dil HCl No White PPT appears 3. Pass H2S gas to above solution No Black PPT formed or any PPT 4. To the salt solution add NH4Cl and NH4OH in excess Pass the H2S gas to above soln No change is observed 5 INFERENCE No effervescence of CO2 Take a pinch of salt in a test tube No rotten egg smell of H2S add Dil H2SO4 No S02 gas ( turn K2Cr2O7 green) No reddish Brown gas make FeSO4 solution black Conc. H2SO4 test - Take a pinch of NO2 gas (reddish brown)- turn salt in a test tube add Conc H2SO4 FeSO4 solution black No change is observed 6 To the salt solution add solid White PPT formation NH4Cl , NH4OH , (NH4)CO3 7 Dissolve the white PPT in CH3COOH and make it 2 parts NH4+ is absent (group 0 absent) Pb++ is absent (group 1 absent) Cu++ , Pb++ etc absent (group 2nd ) (group 3nd absent) Al3+, Fe3+ absent (group 4th absent) Zn2+,NI2+,Co2+ abs. (group 5th present) Ba2+,Sr2+Ca2+may be PART – A + K2CrO4 soln NO change or No PPT formed Ba++ absent 8 PART – B + (NH4)2SO4 soln White PPT obtained Sr ++ confirmed 9 Crimson red flame Sr ++ confirmed 10 Performed Flame test Result- The given salt is Sr(NO3)2 in which Sr++ is cation and NO3- as anion radical AIM- Preparation of lyophilic sol of starch. EXPERIMENT - 17 AIM- Preparation of lyophilic sol of starch. THEORY: When water is used as a dispersion medium, starch has the ability to form sol. This formation is enhanced with the help of heating. To prepare sol the mixture of water and starch is heated to about 100° C. MATERIALS REQUIRED: Tripod stand, Beaker of about 50 to 250 mL, Funnel, Distilled water, Wire gauze, Glass rod, Pestle and mortar, Burner, Filter paper, 500 mg starch. PROCEDURE: 1. Take a mortar and add 500 mg of starch to it. 2. Pour a few drops of distilled water and pestle the starch into a thin paste. 3. Transfer the grinded paste to a 50 ml beaker. 4. Take a 250 mL beaker and pour 100 mL of distilled water to it and heat the water to boiling. 5. Slowly pour the paste into the boiling water and constantly keep stirring with the help of glass rod. 6. Let it boil for 10 minutes after you have transferred all the paste into the beaker. 7. Allow it to cool. 8. With the help of a filter paper attached to a funnel you can filter out the contents. 9. Label the filtrate as starch sol. PRECAUTIONS TO BE TAKEN DURING THE EXPERIMENT: 1.The apparatus used for the experiment should be washed with distilled water and dried before conducting the experiment. 2.Use of distilled water to prepare starch sol. 3.Make sure to convert starch into a smooth paste before adding to the boiling water beaker. 4.Keep constantly stirring the mixture while preparing starch sol. AIM: The aim of this experiment – to prepare ferric hydroxide sol. EXPERIMENT 18 AIM: The aim of this experiment – to prepare ferric hydroxide sol. THEORY: Ferric hydroxide (Fe(OH)3) has the ability to form a lyophobic sol. Sulphides or metal hydroxides which colloidal solution, when treated with water, are termed as lyophobic colloids. Fe(OH)3 sol is obtained by hydrolysis of ferric chloride with boiling distilled water. The reaction is as follows: FeCl3(aq) + 3H2O(l) --------------> Fe(OH)3(s) + 3HCl(aq) The hydrochloric acid formed during the hydrolysis destabilizes the ferric hydroxide sol and therefore must be removed through the process of dialysis. MATERIALS REQUIRED: The apparatus and materials required for this experiment are as follows: Glass rod, round bottom flask, Boiling tube, Conical flask of 250 mL volume, Tripod stand, Funnel, Beaker of 250 mL volume, Burette, Wire gauze, Dropper, Burner, Wire gauze, Iron stand with clamp, Boiling tube, Distilled water, Solution of ferric chloride PROCEDURE: 1.Take a conical flask of volume 250 mL and steam clean it. 2.To clean the conical flask by steaming out process take the help of the figure. 3.Prepare 2% solution of ferric chloride by taking 2 g of pure ferric chloride in 100mL of distilled water. 4.Take the conical flask cleaned by steaming out process and add 100mL of distilled water. 5.Boil the water on a wire gauze. 6.Drop by drop pour 10 mL of ferric chloride solution with the help of a dropper or burette. 7.Constantly keep stirring the boiling water mixture while adding ferric chloride solution. 8.Heat the conical flask containing a mixture of distilled water and ferric chloride solution until you see a brown or deep red coloured ferric hydroxide solution. 9 Allow the mixture in the conical flask to settle at room temperature. 10. Label the flask containing mixture as ferric hydroxide sol. PRECAUTIONS TO BE TAKEN DURING THE EXPERIMENT: 1.Fe(OH)3 sol gets affected due to the presence of impurities. Therefore, to avoid this conical flask is cleaned by steaming out process. 2.The FeCl3 solution is added drop wise. 3. Heat the mixture of distilled water and ferric chloride solution until brown or deep red colour is obtained. 4. The hydrochloric acid (HCl) formed is removed by the process of dialysis to avoid destabilization of sol.