Chemistry Practicals For Class IX (Science Group) - Experiment No. 7: To test the passage of an electric current through electrolytic and non-electrolytic solutions.

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EXPERIMENT NO.7

TO TEST THE PASSAGE OF AN ELECTRIC CURRENT THROUGH 7 ELECTROLYTIC AND NON.ELECTROLYTIC SOLUTIONS.

APPARATUS:

• Two copper strips
• Electrolytic pot or beaker
• Connecting wire
• Bulb holder
• Ammeter
• Dry cell or a battery
• Hanger
• Torch bulb
• Key

CHEMICALS:

• Copper sulphate solution
• Sodium hydroxide solution
• Benzene
• Sodium chloride solution
• Sugar solution

THEORY:

ELECTROLYTES:
Those liquids which conduct electricity are called electrolytes .e.g. solutions of copper sulphate, sodium chloride, sodium hydroxide etc.

NON- ELECTROLYTES:
Those liquids which do not conduct electricity are called non electrolytes .e.g. benzene, sugar solution etc.

METHOD:

• Put given solution (sodium chloride solution) into the electrolytic pot.
• Connect one copper strip to the positive terminal of the cell (battery) through a bulb and a key.
• Connect the second electrode (copper plate) to the negative terminal of the battery through an ammeter.
• Now hang copper strips (electrodes) by a hanger into the pot of given solution.
• Complete the circuit by inserting key in key hole.
• If the current flows across the solution between the two electrodes, the bulb will start glowing and ammeter show deflection. This indicate that the given substance is an electrolyte and if the current does not flow across the solution between the two electrodes, the bulb will not glow and ammeter show no deflection. This indicates that the given substance is a non - electrolyte.
• Repeat the experiment by taking different solutions. Wash electrodes with distilled water for each test.

S.No.	Name Of Solution	Condition Of Bulb Glowing / Not Glowing	Condition Of Ammeter Deflecting / Not Deflecting	Nature Of Solution Electrolyte / Non electrolyte
1	Sodium chloride solution	Glowing	Deflecting	Electrolyte
2	Caustic soda solution	Glowing	Deflecting	Electrolyte
3	Sugar solution	Not Glowing	Not Deflecting	Non-electrolyte
4	Ethyl alcohol	Not Glowing	Not Deflecting	Non-electrolyte

RESULT:
1. Sodium chloride and Caustic soda solutions are electrolytes.
2. Sugar and Ethyl alcohol solutions are non-electrolytes.

REASON:
Glowing of bulb and deflection of ammeter in case of Sodium chloride and Caustic soda solutions indicate that these solutions conduct electricity, hence these solutions are electrolyte. The bulb will not glow and ammeter will not deflect in case of Sugar and Ethyl alcohol solution. This Indicate that these solutions are non-electrolytes.

PRECAUTIONS:

• Connections should be tight.
• Electrodes should be separated from each other in electrolytic pot.
• Dilute solutions should be used.
• The electrodes should be washed with distilled water after each test.

Special Thanks to Sir Sajjad Akber Chandio

Chemistry Practicals For Class IX (Science Group) - Experiment No. 6: To standardize the given solution of sodium Hydroxide using Oxalic acid solution.

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EXPERIMENT NO. 6

TO STANDARDIZE THE GIVEN SOLUTION OF SODIUM HYDROXIDE USING OXALIC ACID

APPARATUS:

• Burette
• Beaker
• Indicator bottle
• Pipette
• Burette stand
• Conical flask
• Funnel

CHEMICALS:

• Sodium hydroxide solution
• Phenolphthalein Indicator
• Oxalic acid solution of known molarity (0.1M)

THEORY:
Titration is the method of quantitative analysis used for determining the concentration of a solution of unknown concentration using a standard solution.

EQUATION:

METHOD:

• Wash all the apparatuses thoroughly with water. Rinse burette with a little quantity of sodium hydroxide solution.
• Rinse the pipette with oxalic acid solution.
• Clamp the burette in an iron stand vertically.
• With the help of funnel, fill the burette with sodium hydroxide solution.
• Remove the air bubbles by drawing some solution from the burette.
• Fill the burette again and assuring that the lower meniscus coincide the zero mark.
• Pipette out 10 ml of oxalic acid solution in a conical flask.
• Start the addition of alkali (NaOH) solution from the burette into the conical flask drop by drop with constant shaking until very faint pink colour persists. This is the end point.
• Record the final reading of the lower meniscus in the burette.

FIND OUT THE DIFFERENCE BETWEEN INITIAL AND FINAL READING

• Find volume of NaOH by subtracting initial reading from final reading to neutralize.
• 10 ml of oxalic acid.
• Throw the contents of conical flask and wash with water.
• Take final reading of first step as initial reading of next step.
• Repeat the procedure of titration in the same manner till three similar readings (Concordant obtained)

OBSERVATIONS:
Solution in the burette (NaOH)
Molarity of NaOH solution M₁ = ?
Volume of NaOH solution (Concordant volume) V₁ = ?
Number of Moles od NaOH (from equation) n₁ = ?

SoIution in the conical flask (Oxalic acid)
Molarity of Oxalic acid M₂ = 0.1 M
Volume of oxalic acid used for each burette reading V₂ = 10 ml
No. of Moles of oxalic acid (from balanced equation) n₂ = 1
Indicator used = Phenophthalein
Colour change • Colourless to light pink
Amount of NaOH in grams /litre = ?

BURETTE READING

S.No.	INITIAL BURETTE READING (mI)	FINAL BURETTE READING (mI)	VOLUME OF NaOH SOLUTION USED (mI)	CONCORDANT VOLUME (mI)

CALCULATION OF MOLARITY:

CALCULATION OF AMOUNT OF NaOH / Liter
Molar mass of NaOH = 40 g

FORMULA:
Amount of NaOH / Liter = Molarity of NaOH x Molar mass of NaOH
= M₁ = 40
= ________

RESULT:
The molarity of given NaOH solution M₁ = _______ M
Amount of NaOH / Liter = __________ g

PRECAUTIONS:

• Note the lower meniscus of alkali solution in the burette.
• Remove air bubble from the jet of the burette.
• Rinse the burette and The pipette with NaOH and oxalic acid respectively.
• All the should be thoroughly washed.
• Only 1 or 2 drops of indicator should be used.
• The pipette should not be down to dropout the solution.
• The lower meniscus of the solution should be read.
• The pipette should not be blown to dropout the solution.
• The flask should be shaken after each addition of the solution.

Special Thanks to Sir Sajjad Akber Chandio

Chemistry Practicals For Class IX (Science Group) - Experiment No. 4: To purify the given sample of Copper Silphate by crystallization.

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EXPERIMENT NO. 4

TO PURIFY THE GIVEN SAMPLE OF COPPER SULPHATE BY CRYSTALLIZATION.

APPARATUS:

• Beaker
• Funnel
• Glass rod
• Watch glass
• Tripod stand
• Wire gauze
• Bunsen burner (Spirit lamp)
• Filter paper
• Iron stand
• Stirrer

CHEMICALS:

• Impure copper sulphate and distilled water.

CHEMICAL EQUATION:

CuSO₄ + 5H₂O ⇒ CuSO₄.5H₂O

Anhydrous (white)    Penta hydrated (blue)

THEORY:
A solution that cannot dissolve more solute is called saturated solution. If saturated solution is further heated and more solute is added, it dissolves. Now on cooling slowly, at roorn temperature, crystals of pure compound obtained, while impurities remain in solution.

METHOD:

• Take about 40 ml distilled water in the beaker.
• Add small quantity of pulverized impure copper sulphate into the beaker containing water.
• Stir it with glass rod to dissolve it.
• Keep on stirring until whole salt dissolve it.
• Keep on adding and stirring until the time will come when no more salt would be dissolved.
• Pour the solution through filter paper to remove insoluble impurities.
• Now decant the solution into another beaker to separate it from undissolved salt.
• Concentrate the solution by boiling the solution until the volume becomes half.
• Allow the solution to cool at room temperature.
• Decant off supernatant liquid.
• Dry the crystals in a fold of filter paper.

RESULT:
Pure crystals of copper sulphate are obtained.

PRECAUTIONS:

• Saturated solution should be prepared at room temperature.
• Cooling process should be as slow as possible.
• During cooling don't disturb the beaker.

Special Thanks to Sir Sajjad Akber Chandio

Chemistry Practicals For Class IX (Science Group) - Experiment No. 2: To determine the melting point of a given solid

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EXPERIMENT 2

TO DETERMINE THE MELTING POINT OF A GIVEN SOLID.

APPARATUS:

• Thermometer
• Beaker
• Test tube
• Rubber band
• Stirrer
• Tripod stand
• Iron stand
• Wire gauze
• Spirit lamp (Bunsen burner)

CHEMICALS:

• Candle wax (using urea, stearic acid and acetamide Or any other solid)
• Water

THEORY:
The temperature at which a solid becomes a liquid at standard atmospheric Pressure is called melting point.

OR

The temperature at which a solid and its liquid are in equilibrium, at any fixed pressure is called melting point.

OR

The melting point of a solid is the temperature at which it changes state from solid to liquid.
The melting is a physical property of a substance. It is the temperature at which the crystals of a pure substance are in equilibrium with the liquid phase at atmospheric pressure.
A pure solid will generally melt sharply because the forces of attraction between its particles are the same. An impure solid melts at a lower temperature and over a wider range. Thus, a solid's melting point is useful not only as an aid in identification but also as an indication of purity.

1^st. METHOD:

• Fill one quarter of test tube with candle wax.
• Tie it to a thermometer in such a way that the wax portion is close to the thermometer bulb. Suspend the thermometer onto the clamp.
• Take some water in a beaker.
• Put the beaker on a wire gauze, over a tripod stand.
• Lower the thermometer along with the test tube by adjusting the clamp.
• Fix the clamp on iron stand.
• The bulb of thermometer should be dipped in the water.
• Heat the beaker slowly by means of Bunsen burner with constant stirring the water with stirrer.
• Note the temperature when ³/₄^th of wax melted.
• Stop heating and note the temperature of wax when it starts freezing.
• Find average of both temperatures.

2^nd. METHOD:

• Fill one quarter of test tube with candle wax.
• Clamp the test tube with iron stand and put it into the beaker which is already placed on a tripod stand and filled with water such that candle wax remains in water.
• Now clamp a thermometer with an iron stand and dip it into the candle wax in such a way that its bulb remains in candle wax.
• Heat the beaker slowly by means of Bunsen burner with constant stirring the water with stirrer.
• Note the temperature when ³/₄^th of wax melted.
• Stop heating and note the temperature of wax when it starts freezing.
• Find average of both temperatures.

OBSERVATIONS:

INITIAL TEMPERATURE	FINAL TEMPERATURE	MEAN TEMPERATURE
Temperature at which wax starts melting	Temperature at which liquid wax starts freezing	Melting point t = t1 + t2/2
_____ °C	_____ °C	_____ °C

RESULT:
Melting point of given candle wax is ___________ °C.

NOTE: Repeat the experiment by using urea, stearic acid and acetamide or any other solid and record their melting points.

PRECAUTION:

• Water should be heated gently.
• Stirring should be constant.
• Thermometer bulb should not touch the walls and base of the beaker.
• Too much or too little sample can be a cause of error.
• Adjust flame size so that the temperature rises no more than 2-3 degree per minute.
• A sample is only used once for melting point determination.
• The graduated side of thermometer should face you.

Special Thanks to Sir Sajjad Akber Chandio

Chemistry Practicals For Class IX (Science Group) - Experiment No. 3: To determine the boiling point of a given liquid.

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EXPERIMENT NO.3:

TO DETERMINE THE BOILING POINT Of A GIVEN LIQUID

APPARATUS:

• Beaker
• Thermometer
• Test tube
• Capillary tube
• Tripod stand
• Wire gauze
• Spirit lamp (Bunsen burner)
• Stirrer
• Rubber band

CHEMICALS:

• Ethyl Alcohol (carbon tetra-chloride and paraffin liquid or any given liquid)
• Water

THEORY:
Temperature A which the vapour pressure of liquid becomes equal to the atmosphere pressure is called boiling point.
The boiling point is a physical property of a substance. It can be defined in terms of the vapour pressure of the solvent. It is the temperature at which the vapour pressure of the liquid Of solvent in a solution is equal to external pressure (i.e. atmospheric pressure). This means liquids can boil at almost any temperature if the external pressure is adjusted. When the pressure on a liquid is increased the boiling point goes up, and if the pressure on a liquid is reduced so it lowers the boiling point. Boiling point is also a characteristic constant, a pure liquid boils at a higher temperature whether the liquid contains a non-volatile or volatile impurities.

1^st. METHOD:

• Seal a small capillary glass tube at one end.
• Take a small quantity (2 ml) of ethyl alcohol in a small test tube.
• Insert the sealed capillary tube upside down into the small test tube, inside the ethyl alcohol.
• Tie the small test tube with a thermometer in such a way that its lower encl remain near the bulb.
• Suspend the thermometer on a clamp.
• Take it beaker half filled with water and place it over a wire gauze which is placed over a tripod stand.
• Lower the thermometer along with the small test tube into the water without touching the wall base by adjusting the clamp on the stand.
• Fix the clamp.
• Now slowly heat the beaker with a Bunsen burner or spirit lamp with constant stirring the water.
• When bubbles come out rapidly from the lower end of capillary tube, the temperature on thermometer is noted.
• Stop heating by removing the burner or spirit lamp.

2^nd. METHOD:

• Seal a small capillary glass tube at one end.
• Take a small quantity (2 ml.) of ethyl alcohol in a small test tube.
• Insert the sealed capillary tube upside down into the test tube, inside the ethyl alcohol.
• Clamp the test tube with iron stand and put it into the beaker which contains water and placed on a tripod stand such that ethyl alcohol remain In water.
• Now clamp a thermometer with an iron stand and dip it into the ethyl alcohol in such a way that its bulb remain in ethyl alcohol.
• Now slowly heat the beaker with a Bunsen burner or spirit lamp with constant stirring the water.
• When bubbles come out rapidly from the lower end of capillary tube, the temperature on thermometer is noted.
• Stop heating by removing the burner or spirit lamp.

OBSERVATIONS:
Boiling point of ethyl alcohol is 78 °C.

RESULT:
Boiling point of given sample of ethyl alcohol (C₂H₅OH) is 78 °C.

PRECAUTIONS:

• Water should be heated gently.
• Stirring should be constant.
• Bulb of thermometer should not touch the walls and base of the beaker.
• Too much or too little sample can be a cause of error.
• Adjust flame size so that the temperature rises no more than 2-3 degree per minute.
• A sample is only used once for boiling point determination.
• The graduated side of thermometer should face you.

Note: Result may be vary depending on the purification of ethyl alcohol.
Special Thanks to Sir Sajjad Akber Chandio

Chemistry Practicals For Class IX (Science Group) - Experiment No. 1: To cut and bend a glass tube and draw a Jet.

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EXPERIMENT NO. 1

TO CUT AND BEND A GLASS TUBE AND DRAW A JET

APPARATUS:

• Glass Tube
• Small Triangular file
• Knife
• Match Box
• Meter stick
• Glass marking pencil
• Bunsen burner / Spirit lamp

CUTTING OF A GLASS TUBE

METHOD:

• Place a glass tube horizontally on a table (or any solid support) as given in the figure.
• Measure the desired length by the meter stick.
• Mark the length with a glass marking pencil.
• Make a single sharp transverse scratch with a triangle file at the mark.
• Hold the tube with both hands in a way that thumbs remain below (opposite to) the mark.
• Exert a little force to break the tube into two pieces with a quick jerk.
• Keep the tube away from your face.
• The tube breaks evenly at the scratched place.
• Round the rough edges of cut tubes by rotating in flame (fire-glazing).
• Allow the tube to cool by placing it over an asbestos sheet.

BENDING OF A GLASS TUBE

METHOD:

• Hold a tube horizontally in your both hands over a Bunsen flame at the ptace where it is to be bent as shown in the figure.
• By rolling and moving the tube back and forth, heat the 2 inches part of the tube evenly, that has to be bent.
• Keep it rotating until it softens.
• When glass becomes soft.
• Bend it at the desired angle, keeping it a bit up from the tip of the flame.
• Hold until the glass hardens.

MAKING OUT A JET

METHOD:

• Hold the tube in your both hands as given in the figure.
• Put it over the flame in a way that only one and half inch of the tube remains in the flame.
• Slowly rotate the tube about its axis, keeping it in the flame until it softens.
• When soft, remove it from the flame and immediately draw the two ends apart carefully till it forms a fine capillary of desired diameter.
• After cooling, cut the tube to separate the two ends by means of a knife.
• Round the rough edges of cut tubes by rotating in flame (fire-glazing).
• Each piece of the tube has a jet.

PRECAUTIONS:

• The scratch on the tubes should be sufficiently deep.
• Pressing of thumbs should be with a uniform force.
• Avoid too much heating, it may cause poor bends.
• The tube should be continuously rotated while heating.
• Do not keep the hot tube on the table.
• Pull the ends of the tube by taking it out of the flame.
• Heat the tube in the upper portion of the flame and continue rotating.
• While drawing a jet the pulling apart of the glass tube should be immediate and carefully.
• Never try to break the tube with simple bare hands.

Special Thanks to Sir Sajjad Akber Chandio