Bsc 2nd Year Chemistry Practical Notes

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हम BSC Students को सभी प्रकार के नोट्स देते हैं ताकि वे आसानी से परीक्षा पास कर सकें। BSC 1st Year के रसायन विज्ञान के नोट्स बाजार में उपलब्ध हैं, लेकिन उनकी भाषा इतनी कठिन है कि उन्हें याद रखना बहुत मुश्किल है. इसलिए हम आपके लिए ऐसे Bsc 2nd Year Chemistry Practical Notes लाए हैं जिन्हें आप आसानी से याद रख सकते हैं।

Bsc 2nd Year Chemistry Practical Notes

Subject	Bsc 2nd Year Chemistry Practical Notes
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Organic Chemistry Practical Notes

Experiment 1: Preparation of Aspirin (Acetylsalicylic Acid)

Objective: To synthesize aspirin from salicylic acid.

Materials:

• Salicylic acid
• Acetic anhydride
• Concentrated sulfuric acid
• Distilled water
• Ice bath
• Filter paper

Procedure:

1. Weigh out 2 grams of salicylic acid and place it in a dry conical flask.
2. Add 4 mL of acetic anhydride to the flask.
3. Carefully add 5 drops of concentrated sulfuric acid to the mixture.
4. Swirl the flask gently and then place it in an ice bath for 15 minutes to cool.
5. Add 50 mL of distilled water to the flask to precipitate the aspirin.
6. Filter the mixture using filter paper to collect the aspirin crystals.
7. Wash the crystals with cold water and allow them to dry.

Observations: Note the appearance of the crystals and any changes during the procedure.

Conclusion: Confirm the formation of aspirin by melting point determination.

Experiment 2: Identification of Functional Groups

Objective: To identify the functional groups present in unknown organic compounds.

Materials:

• Unknown organic compounds
• Test tubes
• Sodium hydroxide solution
• Fehling’s solution
• Bromine water
• 2,4-Dinitrophenylhydrazine (DNPH) reagent

Procedure:

1. Alcohol Test:
   • Add a few drops of sodium hydroxide solution to the unknown compound in a test tube.
   • Warm the mixture and observe any changes.
2. Aldehyde Test:
   • Add Fehling’s solution to the compound and heat gently.
   • Observe for the formation of a red precipitate.
3. Alkene Test:
   • Add a few drops of bromine water to the compound.
   • Note any decolorization indicating the presence of double bonds.
4. Carbonyl Test:
   • Add DNPH reagent to the compound.
   • Observe the formation of a yellow or orange precipitate indicating the presence of a carbonyl group.

Observations: Record the results for each test and compare them with known standards.

Conclusion: Identify the functional groups present in the unknown compounds based on the observed reactions.

Experiment 3: Recrystallization of Benzoic Acid

Objective: To purify benzoic acid by recrystallization.

Materials:

• Crude benzoic acid
• Distilled water
• Hot plate
• Ice bath
• Filter paper

Procedure:

1. Dissolve the crude benzoic acid in the minimum amount of hot distilled water.
2. Filter the hot solution to remove insoluble impurities.
3. Allow the solution to cool slowly to room temperature, then place it in an ice bath to complete crystallization.
4. Filter the crystals using filter paper and wash with cold water.
5. Dry the recrystallized benzoic acid.

Observations: Note the appearance of the crystals before and after recrystallization.

Conclusion: Assess the purity of the recrystallized benzoic acid by comparing the melting point with the literature value.

Safety Precautions:

• Always wear protective equipment such as gloves, goggles, and lab coats.
• Handle chemicals with care, following proper disposal methods.
• Work in a well-ventilated area and be aware of the safety data sheets (SDS) for each chemical used.

Inorganic Chemistry Practical Notes

Experiment 1: Preparation of Potassium Trioxalatoferrate(III)

Objective: To synthesize potassium trioxalatoferrate(III) from ferric chloride and oxalic acid.

Materials:

• Ferric chloride (FeCl₃)
• Oxalic acid (H₂C₂O₄)
• Potassium oxalate (K₂C₂O₄)
• Distilled water
• Ice bath
• Filter paper

Procedure:

1. Dissolve 2 grams of ferric chloride in 20 mL of distilled water.
2. In another beaker, dissolve 3 grams of oxalic acid in 20 mL of distilled water.
3. Mix the two solutions slowly while stirring continuously. A yellow precipitate of ferric oxalate will form.
4. Add 4 grams of potassium oxalate to the mixture and heat gently to dissolve the precipitate.
5. Cool the solution in an ice bath to crystallize potassium trioxalatoferrate(III).
6. Filter the crystals and wash them with cold water.
7. Dry the crystals.

Observations: Note the color and appearance of the crystals.

Conclusion: Confirm the formation of potassium trioxalatoferrate(III) by chemical tests or spectroscopy.

Experiment 2: Gravimetric Estimation of Nickel

Objective: To determine the amount of nickel in a given sample by gravimetric analysis.

Materials:

• Nickel sulfate (NiSO₄)
• Dimethylglyoxime (DMG)
• Ammonia solution
• Distilled water
• Filter paper

Procedure:

1. Dissolve a known amount of nickel sulfate in distilled water.
2. Add ammonia solution dropwise until the solution is slightly alkaline.
3. Add dimethylglyoxime solution to the mixture while stirring. A red precipitate of nickel dimethylglyoxime will form.
4. Filter the precipitate using filter paper.
5. Wash the precipitate with distilled water and dry it.
6. Weigh the dried precipitate to determine the amount of nickel in the sample.

Observations: Record the weight of the precipitate and calculate the nickel content.

Conclusion: Calculate the percentage of nickel in the original sample based on the gravimetric analysis.

 Physical chemistry Practical Notes

Experiment 1: Determination of Surface Tension by Stalagmometer Method

Objective: To determine the surface tension of a liquid using a stalagmometer.

Materials:

• Stalagmometer
• Distilled water
• Test liquid (e.g., ethanol)
• Stopwatch
• Balance

Procedure:

1. Clean the stalagmometer thoroughly and rinse it with distilled water.
2. Fill the stalagmometer with distilled water up to the mark and count the number of drops formed until it empties between two marks.
3. Repeat the process with the test liquid.
4. Measure the mass of a known number of drops for both distilled water and the test liquid using a balance.
5. Calculate the surface tension using the formula:[ \gamma = \gamma_{water} \times \left(\frac{m_{test}}{m_{water}}\right) \times \left(\frac{n_{water}}{n_{test}}\right) ]where:
   • (\gamma) is the surface tension of the test liquid
   • (m_{test}) and (m_{water}) are the masses of the test liquid and water drops, respectively
   • (n_{test}) and (n_{water}) are the number of drops of the test liquid and water, respectively

Observations: Record the number of drops and their corresponding masses for both liquids.

Conclusion: Calculate and compare the surface tension of the test liquid with literature values.

Experiment 2: Determination of the Rate Constant of a Reaction

Objective: To determine the rate constant of the reaction between potassium permanganate and oxalic acid.

Materials:

• Potassium permanganate (KMnO₄) solution
• Oxalic acid (H₂C₂O₄) solution
• Sulfuric acid (H₂SO₄)
• Stopwatch
• Thermometer
• Conical flask

Procedure:

1. Prepare a reaction mixture by mixing known volumes of potassium permanganate, oxalic acid, and sulfuric acid in a conical flask.
2. Note the initial concentration of each reactant.
3. Start the stopwatch when the reactants are mixed.
4. Measure the time taken for the purple color of potassium permanganate to disappear, indicating the end of the reaction.
5. Repeat the experiment at different temperatures to study the effect on the rate constant.

Observations: Record the time taken for the reaction to complete at different temperatures.

Conclusion: Calculate the rate constant using the integrated rate equation and study the effect of temperature on the rate constant using the Arrhenius equation.

Experiment 3: Determination of Partition Coefficient

Objective: To determine the partition coefficient of acetic acid between water and n-butanol.

Materials:

• Acetic acid solution
• n-Butanol
• Distilled water
• Separating funnel
• Conical flask
• Pipette
• Burette

Procedure:

1. Mix equal volumes of acetic acid solution and n-butanol in a separating funnel.
2. Shake the funnel vigorously and allow the layers to separate.
3. Carefully separate the aqueous and organic layers into different conical flasks.
4. Titrate the aqueous layer with a standard sodium hydroxide (NaOH) solution to determine the concentration of acetic acid in water.
5. Similarly, titrate the organic layer to determine the concentration of acetic acid in n-butanol.

Observations: Record the volumes of NaOH used in each titration.

Conclusion: Calculate the partition coefficient (K) using the formula:

[ K = \frac{C_{organic}}{C_{aqueous}} ]

where (C_{organic}) and (C_{aqueous}) are the concentrations of acetic acid in the organic and aqueous layers, respectively.

Experiment 4: Determination of Molar Conductivity

Objective: To determine the molar conductivity of an electrolyte (e.g., KCl) at different concentrations.

Materials:

• Conductivity meter
• Standard KCl solution
• Distilled water
• Conductivity cell
• Volumetric flasks
• Pipettes

Procedure:

1. Prepare a series of KCl solutions of known concentrations.
2. Measure the conductivity of each solution using the conductivity meter.
3. Calculate the molar conductivity ((\Lambda_m)) for each concentration using the formula:[ \Lambda_m = \frac{\kappa}{C} ]where (\kappa) is the measured conductivity and (C) is the concentration of the solution.

Observations: Record the conductivity readings for each concentration.

Conclusion: Plot the molar conductivity against the square root of the concentration and determine the limiting molar conductivity.

Safety Precautions

• Always wear protective equipment such as gloves, goggles, and lab coats.
• Handle chemicals with care, following proper disposal methods.
• Work in a well-ventilated area and be aware of the safety data sheets (SDS) for each chemical used.

Also Read: 10 Important Organic Chemistry Chapters for BSC 3rd Semester Prepration

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