Manuals Science Lab Manual Class 10 Pdf


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NCERT Class 10 Science Lab Manual Materials. Download NCERT Chapters and Books in pdf format. Easy to print and read. Copies of these textbooks may be. Basic concepts of each experiment has been covered for better understanding. The matter is presented in simple and lucid language under main-headings and . This Manual of Secondary Science Kit for Classes IX and X not as a portable laboratory whereas the manual supplements the science M.P; Mr. R.P. Sharma , Education Officer Science, CBSE, Siksha 10 per cent composition by volume.

Science Lab Manual Class 10 Pdf

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NCERT CLASS 10 SCIENCE LAB MANUAL PDF PEELDZSURG | PDF | 63 Pages | KB NCERT CLASS 10 SCIENCE LAB MANUAL. CBSE CLASS 10 SCIENCE LAB MANUAL DOWNLOAD PDF The main topic of the following eBook is focused on CBSE CLASS 10 SCIENCE. Class 10 Science Lab Manual Features: Experiments for Class 10 CBSE; Chemistry Practicals for Class 10; Physics Practicals for Class 10;

Take about 20 mL of dilute sulphuric acid in each of remaining four beakers. Prepare about 50 mL. A B C D Colour of the cloth or flower petal dipped in the solution of sample chemical Colour of cloth or flower petal dipped in sample solution and then in dil. Thus the bleaching powder can be identified. Dip a small piece of coloured cloth or flower petal in beaker A. Take out the cloth or flower petal from the beaker A and dip it in dil.

Repeat steps 3 and 4 with other three samples of given chemicals and dil. Label these beakers as A. Does the cotton cloth or flower petal decolourise? In this case. Sample 1. These must not touch your skin. Why does the bleaching powder known as a mixture? What happens when bleaching powder is exposed to air? How does the bleaching powder help in the purification of water? What is the chemical name of bleaching powder?

Carbonates and hydrogencarbonates react with dilute acids and produce carbon dioxide gas which turns lime water milky. It is soluble in water and forms a colourless solution. Their aqueous solutions are alkaline and turn red litmus blue. Materials 9 AIM To identify washing soda or baking soda among given samples of chemicals. Does it again become colourless? This reconfirms that the liberated gas is CO2.

Pass the liberated gas evolved through the lime water in a test tube. Note the change in colour of the litmus paper. Add about 5 mL distilled water in each boiling tube. Wash the glass rod used for one sample before using it for other sample. Continue passing the liberated gas through the lime water. Take about 1 g each of the four given samples separately in four boiling tubes and label them as A.

Repeat the lime water test on all samples that give effervescence in step 4. For performing lime water test. Add 1 mL of dil. Gently shake the contents of the tubes. Do not forget to wash the boiling tube when you change the sample in it for performing the lime water test. Does the lime water turns milky? Do you see any effervescence from any test tube? If the addition of dil. Handle hydrochloric acid and washing soda carefully.

Colour Solubility in water Action on red litmus paper Action of dil. Discuss about the litmus paper and lime water tests performed. These salts liberate either CO2 or SO2. Sample No. Preparation of lime water: Shake 5 g calcium oxide CaO. Sulphur dioxide also turn lime water milky. These should not touch your skin. The remaining samples of salts should not be carbonates. What will happen if crystalline washing soda is left open in air?

CO2 and SO2 both turn lime water milky and their aqueous solutions turn blue litmus paper red. How can you then distinguish between these? Why should carbon dioxide be soluble in aqueous solution of potassium carbonate?

Materials 10 AIM To show that crystals of copper sulphate contain water of crystallisation.

Take some crystals of copper sulphate CuSO4. These crystals dehydrate on heating to lose water of crystallisation at a particular temperature and also change their colour. Do you see any difference in them? Look at the dehydration reaction of copper sulphate. Thus the hydration and dehydration is the precise cause of colour change.

Keep the watch glass in open atmosphere for some time and allow it to cool. Do not bring your face near to hot spatula. What shall be the total action of heat on copper sulphate? It is regarded that each molecule of copper suphate crystals at room temperature contains five water molecules as water of crystallisation.

Note the change in colour of the copper sulphate crystals during the heating. Heat these crystals on a burner by keeping the spatula directly over the flame of the burner.

Do you find a change in the colour of copper sulphate crystals. Stop heating when it becomes complete white.

This dehydrated copper sulphate regains water of crystallisation on cooling and it again becomes blue. Does it show a bluish white colour? Transfer the content white powder to a watch glass. The blue colour of copper sulphate solution will gradually fade and finally. A more reactive metal displaces a less reactive metal from its salt solution.

For example. The metals. Displacement reactions can be used to find out the relative reactivities of metals. Some metals are more reactive than others.

Materials 11 AIM To study the interaction of metals such as magnesium. Laboratory Manual Science four beakers mL. Metal Metal displacement and colour change of solution Solution to which metal is added Zinc sulphate solution.

C Lead nitrate solution. Take zinc. Fig Take 10 mL of each solution in four different test tubes and label them as tubes A. Note that these are the salt solutions of the four metals taken for studying the interaction.

Label these beakers as W. Put zinc metal strip in all the nitrate D solutions four test tubes. Repeat the above experiment with other metal strips by dipping them in fresh salt solutions of metals and observe for displacement reactions. B Iron II sulphate solution. Zinc metal dipped in Zinc sulphate A. Wash the test tubes after every set of observations of interaction of a particular metal with the four salt solutions.

BX is a salt of metal B. Give reason. What is your observation when copper is added in iron II sulphate solution? Which is the most and the least reactive metal in the above experiment?

H2SO 4 may be added during the preparation of salt solutions to avoid the hydrolysis of sulphate salts. A and B are metals. For obtaining granuels of different metals. Name any two metals that are more reactive than iron? Why did the colour of copper II sulphate solution. Metals like aluminium. The reaction is so violent that the liberated hydrogen immediately ignites. But all metals donot react with water. Metals like lead. Metals like potassium and sodium react violently with cold water.

It reacts with hot water to form magnesium hydroxide and hydrogen. Take seven test tubes each half filled with cold water. Boil about mL Fig. How fast these tube metals react with cold water? Do all metals Gas jar react at the same rate? The order of reactivity Metal Clamp in different test tubes can be compared by Burner carefully observing the rate of formation of bubbles of liberated hydrogen gas in the Trough test tubes. Put these metallic pieces in test tubes half filled with hot water.

Did you find any metallic substance reacting neither with cold water nor hot water? These may or may not react with steam. Also observe that which metal reacts fast with hot water? Also compare their order of reactivity by observing the bubbles of liberated hydrogen gas in the test tubes. Put small samples of clean metallic substances in these seven test tubes. Materials In this experiment we shall study reactions of some metals with water under different conditions.

Take out the metallic pieces from the test tubes that did not react with cold water in steps 2 and 3. Action of steam on a metal water in a beaker. Place them in a test tube stand. Observe the test tubes to identify the metals Stand that react with cold Glass wool H2 gas Deleivery Boiling tube water. Take such samples out from the test tubes. Observe the test tubes to identify the metals that react with hot water.

Science text book “Lab Manual” Hindi Medium E-book for class 10, CBSE , NCERT.

Iron 6. All metals except sodium should be cleaned by rubbing with a sand paper. Zinc Lead 5. Arrange the metals in the decreasing order of reactivity with water under different conditions. Also list the metals that do not react with water. Laboratory Manual Science 9. Metals Reaction conditions cold water 1.

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Aluminium 7. To see the reaction of metallic substances as identified in step 8 with steam. Sodium Magnesium 3. The exposed surface area of all samples of metallic substances under observations should be same. Also arrange the metals in the order of decreasing reactivity in each list.

NCERT Class 10 Science Lab Manual Materials

Did any metal produce fire in water? Which metals did not react with cold water at all? Why should we use glass-wool soaked in water for action of sodium on cold water? Which metal did not react with water even in the form of steam? HNO3 to liberate hydrogen gas. In this reaction hydrogen gas is evolved. HCl or dil.

The metal replaces the hydrogen atoms from the acid to form a salt. It is because HNO3 is a strong oxidising agent.

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It oxidises the hydrogen produced to water and r educes to any of oxides of nitrogen such as N2 O. Hydrogen gas is rarely evolved when metal reacts with nitric acid. D and E respectively. H 2SO 4 and dil. Materials five test tubes. Arrange the metals in the decreasing order of reactivity with dil. Place these metals in test tubes A. Take small pieces of sample metallic substances magnesium.

Also arrange the metals A. H2SO4 dil. Repeat the experiment steps 1 to 6 with dil. Metal Intensity of reaction with dil.

Take five test tubes in the test tube stand and label them as A. These bubbles are of the hydrogen gas. Add about 10 mL dil. Wash the test tubes with water. Put them in a test tube stand. Clean their surfaces by rubbing with a sand paper. Record your observations as vigrous. Observe carefully the rate of formation of bubbles in the test tubes. HNO3 separately.

Take out the metallic samples from the test tubes. Which metal did not react with dil. Which metals reacted vigorously with dil. Can we use dil. HCl in this experiment? Why would iron dust reacts vigorously as compared to iron filings with dil.

Can you suggest any test to verify that evolved gas. Metal reacts with dil.

Clean the metal surface with sand paper. Materials 14 AIM To prepare sulphur dioxide gas and study its physical and chemical properties. It decolourises acidified potassium permanganate KMnO4 solution. Place the cork in its position on the flask again and heat the contents gently. Add The gas formation starts after sometime. Collect the gas in the gas jar and study its properties as per the steps given in the observation table.

Preparation of sulphur dioxide gas Thistle funnel Delivery tube Conc.

Place few pieces of copper turnings about 5 g in a round bottom flask and arrange the apparatus as shown in Fig. Concentrated sulphuric acid should be handled carefully. On the basis of observations mention the physical and chemical properties of the liberated sulphur dioxide gas.

Avoid adding large quantity of acid at a time. Remove the lid carefully. Solubility of SO2 in water is a chemical property on account of the following reaction.

Take about 2 mL of potassium Reaction with permaganate solution in a test potassium tube. Invert it in water contained in a trough. Chemical Properties Acidic or basic Insert damp or wet litmus paper nature in the jar filled with sulphur dioxide. Do not inhale sulphur dioxide. It should not touch your skin.

Care should be taken while handling hydrochloric acid. It should not touch the skin. What type of reaction oxidation or reduction does sulphuric acid undergo during the laboratory preparation of sulphur dioxide? What happens when sulphur dioxide is passed through acidified potassium permanganate solution? How will you prove that sulphur dioxide is acidic in nature? Why is sulphur dioxide collected by upward displacement of air? What are the different roles of H2SO4 in chemical reactions?

Justify your answer with an example of each? Identify the role oxidant or reductant of each gas in the following reaction: Calcium carbonate is usually taken in the form of marble chips. It is also an oxidising agent. It turns a red litmus paper blue and turns lime water [Ca OH 2 aq ] milky. Add, dropwise, 10 mL of dil.

Do you see any gas formation? Collect the liberated gas in gas jar to perform the colour, odour, solubility in water, combustibility and acidic tests. Record your observations in the observation table. Pass the liberated gas through Fig. Do you see any gas bubbles in the lime water? Does the colour of lime water turns milky? Intr oduce a lighted candle in the gas filled jar Insert a moist or wet r ed litmus paper in the gas filled jar.

Excessively pass the liberated gas thr ough the lime water. On the basis of observations mention the properties of liberated gas. The apparatus should be airtight. Avoid adding large quantity of acid at a time, otherwise a vigorous reaction may occur.

While collecting the gas in the jar, a piece of cardboard should be placed over the mouth of the gas jar. Shake about 5 g of calcium oxide, CaO, with mL water. Allow it to stand for 24 hours. Always use freshly prepared limewater. This set up is needed for collecting the gas in a jar. The reaction may also be carried out in a test tube. In this experiment dil. H2SO 4 may also be used in place of dil. It forms CaSO4 on reacting with marble chips. Sulphuric acid is not used for preparing the carbon dioxide gas in the laboratory.

What happens to the burning magnesium strip when introduced in the jar filled with carbon dioxide? Why is lighted candle put off when inserted in the jar of carbon dioxide? What is the effect of carbon dioxide gas on moist blue litmus paper? How can you prove that we exhale breathe out carbon dioxide? What happens when excess of CO2 is passed through lime water? Write the chemical equation for the reaction involved.

On passing an electric current from an external source. In this experiment. Materials 16 AIM To study the process of electrolysis.

Positive ions migrate to the negative electrode and negative ions to the positive electrode and they discharge at respective electrodes. When an electric current is passed through the aqueous solution of copper sulphate. This phenomenon is called electrolysis and the container in which electrolysis occur is called electrolytic cell. Observe the electrolytic solution after sometime. Add to it about 1 mL of dil.

An electr olysis process through a plug key as shown in Fig. Impur e Copper 5.

Do you find any change in the thickness es of the two copper strips? Note your observations. Take a beaker to use it as an electrolyic cell. If not. Connect two wires with the two copper strips to be considered as positive electrode impure copper strip and negative electrode pure Positive Negative electorde copper strip. Dissolve about 3 g of copper sulphate crystals in mL distilled water and pour this solution in the electrolytic cell. Connect the two copper sulphate copper strips with strip solution a combination Beaker of two dry cells in mud a cell holder Fig.

Immerse the two copper strips into the solution and cover the beaker with the cardboard. Insert the key into the plug to allow the electric current to pass through the electrolytic solution. Clean the ends of the connecting wires using a sand paper. The purpose of electrolysis is electroplating. That is how the thickness of impure copper strip keeps on decreasing and the thickness of pure copper strip keeps on increasing on passing the current through the electrolyte.

Never keep the two electrodes close to each other in the electrolytic cell. Oxidation is also described as loss of electrons and takes place at anode for example in the reaction under discussion. Actions Shares. Embeds 0 No embeds. No notes for slide. Cbse class 10 science lab manual download pdf 1. You can get the manual you are interested in in printed form or perhaps consider it online. You can begin from the Intro and Brief Description to get a glance about the subject.

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Observe the change in the colour of the filter paper. Was the length of foam formed same in each of the test tube containing soap solution? Successfully reported this slideshow.

What is the reason for this observation?