evergreen chemistry lab manual class 12
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evergreen chemistry lab manual class 12Please try again.Thursday, July 8Wednesday, July 7Sign up for free Order delivery tracking to your doorstep is available.No customer signatures are required at the time of delivery. To pay by cash, place cash on top of the delivery box and step back. The subject has been presented in a simple, brief and easy to understand language. The book consists of a number of experiments provided with a brief theory, procedure, observations and precautions. Each experiment is followed by a number of relevant viva-voce and discussion questions from NCERT Lab manual to help the students prepare better for their assessment. A few investigatory projects have also been included. Show details Hide details Choose items to buy together. FREE Shipping on orders over ?499.00. Evergreen CBSE Lab Manual in Biology: For 2021 Examinations(CLASS 12 ) by Raman Soni Paperback ?330.00 In stock. Sold by Cloudtail India and ships from Amazon Fulfillment. FREE Shipping on orders over ?499.00. Then you can start reading Kindle books on your smartphone, tablet, or computer - no Kindle device required. Get your Kindle here, or download a FREE Kindle Reading App.To calculate the overall star rating and percentage breakdown by star, we don’t use a simple average. Instead, our system considers things like how recent a review is and if the reviewer bought the item on Amazon. It also analyses reviews to verify trustworthiness. Please try again later. Amazon Customer 4.0 out of 5 stars. Cash on Delivery available. Seller ManavBookDistributors 3.6 7 Days Replacement Policy. Working till perfection READ MORE Anmol 2003 Certified Buyer, Hamirpur District 4months ago 0 0 Permalink Report Abuse 5 Best in the market. JESSICA BOOKS Flipkart Seller 0 0 Report Abuse Q: Does it contains pages for writing, like half book and half notebook type? A: YES. JESSICA BOOKS Flipkart Seller 0 0 Report Abuse Q: Does it contains separate pages for writing? A: YES.http://erdemlirehberim.com/UserFiles/farfisa-intercom-manuals.xml
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JESSICA BOOKS Flipkart Seller 0 0 Report Abuse Q: it have list of parcticals. Easy returns. 100 Authentic products. These Chemistry Lab Manual may be freely downloadable and used as a reference book. Learning does not mean only gaining knowledge about facts and principles rather it is a path which is informed by scientific truths, verified experimentally. Keeping these facts in mind, CBSE Chemistry lab manual for Class 12 have been planned, evaluated under subject Improvement Activities. Check our CBSE Chemistry lab manual for Class 12. We are grateful to the teachers for their constant support provided in the preparation of this CBSE Chemistry Lab Manual. CBSE has included the practicals in secondary class intending to make students familiarised with the basic tools and techniques used in the labs. With the help of this, they can successfully perform the experiments listed in the CBSE Chemistry Lab Manual. Their basics will become solid as they will learn by doing things. By doing this activity they will also get generated their interest in the subject. Students will develop questioning skills and start studying from a scientific perspective. Here we have given all the necessary details that a Class 12 student should know about CBSE Chemistry Lab Manual. From CBSE practical to Chemistry Lab manual, project work, important questions and CBSE Chemistry lab kit manual, all the information is given in the elaborated form further in this page for Class 12 students. The matter is presented in the simple and lucid language under main-headings and sub-headings. The syllabus for the practical exam is designed by CBSE according to the CCE guidelines. With the help of this solution, determine the molarity and the concentration of KMnO 4 in the given solution. Find out the percentage purity of impure KMnO 4 sample 2.0 g of which have been dissolved per litre. With its help, determine 50 the molarity and strength of the given solution of potassium permanganate (KMnO 4 ).http://globalewastemanagement.com/gemsuserfiles/farfisa-intercom-user-manual.xml Determine volumetrically the atomic mass of the alkali metal.Using this solution, determine the normality and strength of the given potassium permanganate solution. Using this solution, find out strength and normality of the given potassium permanganate solution. Ask for your requirement. In qualitative analysis, the given compound is analyzed for the radicals, i.e., cation and the anion, that it contains. Physical procedures like noting the colour, smell or taste of the substance have very limited scope because of the corrosive, poisonous nature of the chemical compounds. Therefore, what one has to resort to is the chemical analysis of the substance that has to be carried out along with the physical examination of the compound under consideration. The common procedure for testing any unknown sample is to make its solution and then test this solution for the ions present in it. There are separate procedures for detecting cations and anions, therefore qualitative analysis is studied under cation analysis and anion analysis.The test is not much reliable, but is certainly helpful in identifying some coloured cations. Characteristic smell helps to identify some ions such as ammonium, acetate and sulphide. (See Table 12.1 on next page) Note: It may be corrosive to skin. Salts of arsenic and mercury are highly poisonous. Quite valuable information can be gathered by carefully performing and noting the observations here. On heating, some salts undergo decomposition, thus, evolving the gases or may undergo characteristic changes in the colour of residue. These observations are tabulated in Table 12.2 along with the inferences that you can draw. Table 12.2. Dry Heating Test Note: While drying a test-tube, keep it in slanting position with its mouth slightly downwards so that the drops of water which condense on the upper cooler parts, do not fall back on the hot bottom, as this may break the tube.http://www.liga.org.ua/content/db500a-manual In certain cases, the oxides formed partially undergo reduction to the metallic state producing metallic beads or scales. Examples: Procedure While performing charcoal cavity test, make a small cavity on a charcoal block with the help of borer as shown in Fig. 12.2. Mix small amount of salt with double its quantity of sodium carbonate. Place it in the cavity made on the block of charcoal. Moisten with a drop of water and direct the reducing flame of the bunsen burner on the cavity by means of a mouth blowpipe as shown in Fig. 12.3. Heat strongly for sometime and draw inference according to the Table 12.3. To obtain a reducing flame with the help of a mouth blow pipe, make the bunsen burner flame luminous by closing the air holes of the burner. Keep the nozzle of the blow pipe just outside the flame (Fig. 12.4) and blow gently on to the cavity. The test is based on the fact that cobalt nitrate decomposes on heating to give cobalt oxide, CoO. This combines with the metallic-oxides, present as white residue in the charcoal cavity forming coloured compounds. For example, when a magnesium salt undergoes charcoal cavity test, a white residue of MgO is left behind. This on treatment with cobalt nitrate and subsequent heating forms a double salt of the formula MgO.CoO which is pink in colour. In addition to metallic oxides, phosphates and borates also react with cobalt oxide to form CO 3 (PO 4 ) 2 and CO 3 (BO 3 ) 2 which are blue in colour. Some of the reactions involved are given below: Heat for one or two minutes by means of a blow pipe in oxidising flame. Observe the colour of the residue and draw inferences Note: Excess cobalt nitrate may decompose to give cobalt oxide which is black in colour. HCl from their chlorides, that are volatile in non-luminous flame. Their vapours impart characteristic colour to the flame. This colour cfan give reliable information of the presence of certain basic radicals. For proceeding to this test, the paste of the mixture with cone. HCl is introduced into the flame with the help of platinum wire (Fig. 12.5). HCl taken on a watch glass and then heating strongly in the flame. This process is repeated till the wire imparts no colour to the flame. Now prepare a paste of the mixture with cone. HCl on a deem watch glass. Place small amount of this paste on platinum wire loop and introduce it into the flame. Note the colour imparted to the flame. Borax, Na 2 B 4 O 7.10H 2 O, on heating gets fused and loses water of crystallisation. It swells up into a fluffy white porous mass which then melts into a colourless liquid which later forms, a clear transparent glassy bead consisting of boric anhydride and sodium metaborate. Procedure Borax, Na 2 B 4 O 7.10H 2 O is heated in the loop of platinum wire, it swells and forms transparent colourless glassy bead. When this hot bead is touched with small amount of coloured salt and is heated again, it acquires a characteristic colour. The colour of bead gives indication of the type of the cation present. The colour of the bead is noted separately in oxidising and in reducing flame (Fig. 12.6). Table 12.6. Borax Bead Test To remove the head from platinum wire, heat the head to redness. Tap the rod with finger stroke, till the bead jumps off (Fig. 12.7). The identification of the acid radicals is first done on the basis of preliminary tests. Dry heating test is one of the preliminary tests performed earlier which may give some important information about the acid radical present. The other preliminary tests are based upon the fact that: Take a small quantity of the salt in a test-tube and add 1-2 ml of dilute sulphuric add. Identify the gas and draw Note: H 2 SO 4 Test Dilute H 2 SO 4 (or dilute HCl) decomposes carbonates, sulphides and nitrites in cold to give gases. These gases on identification indicate the nature of the add radical present in the salt. Potassium permanganate test To a pinch of salt in test tube add about 2 ml of dilute sulphuric acid. Boil off any gas evolved, add little more of dilute acid and then potassium permanganate solution dropwise.Oil H 2 SO 4 acid is added to the salt and heated till sulphides, sulphites and nitrites are completely decomposed. Then KMnO 4 is added dropwise to cold solution. Identify the gas evolved in cold and then on heating. Draw inferences from Table 12.9 Note: On boiling, the acid may decompose to give SO 2 gas. When a paper pellet or copper chips is added, dense brown fumes evolve. Paper pellet acts as a reducing agent and reduces nitric acid to NO 2 (Reddish brown gas). H 2 SO 4 Test Tests for independent radicals (SO 4 2- and PO 4 3- ) As already diseussed these radicals are not detected by dilute or concentrated H 2 SO 4.They are tested individually. Filter the contents, and to the filtrate add few drops of BaCl2 solution. A white ppt. insoluble in cone. HCl indicates presence of sulphate. HNOs to the salt in a test tube. Boil the contents and add excess of ammonium molybdate solution. A yellow precipitate indicates presence of phosphate. H 2 SO 4 or cone. H 2 SO 4 tests is further confirmed by wet tests. The solution used for the purpose is any one of the following: Preparation of Sodium Carbonate Extract. Mix about 1 g of the salt with about 2 g of pure sodium carbonate and boil it for 10-15 minutes with 20-25 ml of distilled water in a small conical flask having a funnel in its mouth (Fig. 12.8). The funnel acts as a condenser. This arrangement prevents the loss of water due to evaporation. Filter the solution, cool it and label it as sodium carbonate extract or S.E. Alternatively, sodium carbonate extract can be prepared in a test tube. A pinch of salt is mixed with double the amount of sodium carbonate and is boiled with distilled water for sometime. The suspension obtained is filtered.The filtrate is sodium carbonate extract. p.g 12 8. Preparation of sodium carbonate extract. Theory of Preparation of Sodium Carbon-ate Extract. When the salts are boiled with strong solution of sodium carbonate, double decompo-sition takes place resulting in the formation of the carbonates of heavy metallic radicals and sodium salts of the acid radicals. The sodium salts of corresponding add radicals being soluble in water pass into the solution and carbonates of heavy metals are predpitated To do this, the extract is addified with some suitable acid and is boiled to expel carbon dioxide. The selection of add used for destroying excess Na 2 CO 3 depends upon the radical to be identified. Now we describe in detail the confirmatory tests for various add radicals discussed so far. Confirmation of Carbonate, CO 3 2- (Indicated in dilute acid test by occurrence of brisk effervescence and evolution of carbon dioxide). Note: Confirmation of Sulphide, S 2- (Indicated in dilute acid test by the evolution of hydrogen sulphide).HCl give CO 2 gas which turns lime water milky. In case of soluble carbonates this test is performed with water extract and in case of insoluble carbonates this test is performed with the solid salt. H 2 SO 4 with the evolution of HCl gas). H 2 SO 4 with the evolution of bromine vapours). Note. Chlorine water is prepared by adding dropwise cone. H 2 SO 4 with the evolution of vapours of iodine). H 2 SO 4 with the evolution of brown vapours of nitrogen peroxide). H 2 SO 4 with the evolution of CH 3 COOH vapours. H 2 SO 4 with the evolution of CO 2 and CO gas) Chemical Reactions Involved in the Confirmation of Chloride, Bromide, Iodide, Nitrate Acetate and Oxalate Confirmation of Sulphate, SO 4 2- (Not indicated in dilute and concentrated H 2 SO 4 acid tests). Confirmation of Phosphate, P O 4 3- (Not indicated in dilute and concentrated H 2 SO 4 acid test). Chemical reactions involved in the confirmation of SO 4 2- and P O 4 3- Wet tests for basic (cations) Preliminary tests such as dry heating test, charcoal cavity test, flame test and borax bead test may give us some indication about the cation present in the salt. However, the cation is finally detected and confirmed through a systematic analysis involving wet tests. For the sake of qualitative analysis the cations are classified into the following groups (Table 12.10). Before carrying out the wet tests for the analysis of cation, the salt has to be dissolved in some suitable solvent to prepare its solution. For this purpose, the under noted solvents are tried one after another in a systematic order. In case the salt does not dissolve in a particular solvent even on heating, try the next solvent. The following solvents are tried: Add some suitable solvent into it and shake. If it does not dissolve even after heating for sometime, take the fresh quantity of the salt again and treat it in a similar manner with next solvent. The clear solution thus obtained is labelled as Original Solution (O.S.). Gas must be completely expelled by heating. Proceed with group II. For example, if hydrochloric acid is added to a solution containing all cations, only the chlorides of lead, silver and mercury (ous) will precipitate, since all other chlorides are soluble. Thus, these cations form a group of ions which may be precipitated from solution by addition of group reagent HCl. Similarly, H 2 S is a group reagent for group II. The following Table 12.11 clearly shows the group reagents for different groups and the form in which cations of the particular group are precipitated out. Theory of precipitation of different groups The classification of cations into different groups in the inorganic qualitative analysis is based upon the knowledge of solubility products of salts of these basic radicals. On the basis of this knowledge these radicals are grouped together in group-I and are precipitated as their chlorides by adding dilute HCl to their solutions. For adjusting the conditions for precipitation, another concept called common ion effect plays very important role. Before we consider the precipitation of radicals of other groups, let us discuss in brief the concept of common ion effect. In their solutions, unionised molecules are in dynamic equilibrium with ions. The degree of ionisation of a weak electrolyte (weak acid or weak base) is further suppressed if some strong electrolyte which can furnish some ion common with the ions furnished by weak electrolyte, is added to its solution. This effect is called common ion effect. For example, degree of ionisation of NH 4 OH (a weak base) is suppressed by the addition of NH 4 Cl (a strong electrolyte). Therefore, according to Le-Chatelier’s principle equilibrium in equation (12.1) shifts in the backward direction in favour of unionised NH 4 OH. The suppression of the degree of ionisation of a weak electrolyte (weak acid or weak base) by the addition of some strong electrolyte having a common ion, is called the common ion effect. Solubility products of sulphides of group II radicals are very low. Therefore, even with low concentration of S 2- ions, the ionic products (Qs p ) exceed the value of their solubility products (KS p ) and the radicals of group II get precipitated. The low concentration of S 2- ions is obtained by passing H 2 S gas through the solution of the salts in the presence of dil. HCl which suppresses degree of ionisation of H 2 S by common ion effect. It is necessary to suppress the concentration of S 2- ions, otherwise radicals of group IV will also get precipitated along with group II radicals. But solubility products of their sulphides are quite high. In order that ionic products exceed solubility products, concentration of S2- ions should be high in this case. High concentration of sulphide ions is achieved by passing H 2 S gas through the solutions of the salts in the presence of NH 4 OH. Hence, concentration of S 2- ions increases. With this increased concentration of S 2- ions ionic products exceed solubility products and radicals of group IV get precipitated. The solubility products of hydroxides of group III radicals are quite low. NH 4 Cl suppresses the degree of ionisation of (NH 4 ) 2 CO 3 by common ion effect and hence decreases the concentration of CO 3 2- ions. During the analysis of cations NH 4 Cl and NH 4 OH are added in many steps.Evolution of NH 3 gas is confirmed by the following tests: HCl is brought near the mouth of the test tube. Group reagent for this group is dil.These are precipitated as their sulphides. If group I is absent, the tests for radicals of group II are carried out. Group reagent for this group is H 2 Sgas in the presence of dil. HCl. Make it acidic with dil. HCl and warm the contents. Through this solution pass H 2 S gas from the Kipp’s apparatus by turning the stop cock as shown in Fig. 12.10, Formation of the black or yellow precipitates indicates the presence of group II radical. If this is observed, pass more of H 2 S gas to ensure complete precipitation of the radical sulphide. Centrifuge and separate the precipitates. Identification of IIA and IIB Groups. Note the colour of the precipitate. Chemical Reactions Involved in the Analysis of Group II. These cations are precipitated as hydroxides by adding ammonium hydroxide in presence of ammonium chloride. Thus, group reagent for this group is NH 4 OH in the presence of NH 4 Cl. Procedure In case, first and second groups are absent proceed for group III with the original solution. Take about 5 ml of the original solution and add 4-5 drops of cone, nitric acid. Boil the solution for sometime. Add to it about 2 g of solid NH 4 Cl and boil again. Cool the solution under tap water. Add excess of ammonium hydroxide to it and shake. A ppt. shows the presence of some cation of group III. Filter the ppt. and wash with water. Analyse the ppt. and draw inferences as in Table 12.14. Note: These are precipitated as sulphides by passing H 2 S gas through the ammonical solution of the salt. The group reagent for this group is H 2 S gas in the presence of NH 4 Cl and NH 4 OH. Pass H 2 S gas through the solution. If some ppt. is formed, presence of some radical of group IV is indicated. Filter the ppt. and wash it with water. Note the colour of the ppt.Formation of black ppt. (CoS or NiS) indicates cobalt or nickel. Formation of buff-coloured ppt. (MnS) indicates manganese and dirty white ppt. (ZnS) indictes zinc 2.Ammonium thiocyanate ether test On addition of ether and a crystal of ammonium thiocyanate (shaking and allowing to stand), a blue colour due to the formation of ammonium cobhlti thiocyanate, is obtained in the ethereal layer. These cations are precipitated as their carbonates. Group reagent for this group is (NH 4 ) 2 CO 3 in the presence ofNH 4 Cl and NH 4 OH. Then add (NH 4 ) 2 CO 3 solution. Appearance of white ppt.Filter and wash the ppt. with water. Dissolve the ppt. in hot dil. acetic acid. Divide the solution into three parts and proceed as in Table 12.16. Note. Give an example. Answer. A homogeneous mixture of two substances, in which particles of both possess molecular dimensions (i.e., 10 -10 to 10 -9 m). For example, a solution of common salt in water. Give an example. Answer. A colloidal solution is a “two-phase heterogenous system in which a substance is distributed in colloidal state (particles having diameter between 1 to 1000 nm) in a medium”. The particles of the dispersed substance (of colloidal size) are called dispersed phase’, while the medium in which they are dispersed, is called dispersion medium. For example, milk, butter, smoke, etc. For example, starch sol is a lyophilic sol whereas sulphur sol is a lyophobic sol. In sol liquid is the dispersion medium and solid the disperse phase whereas in gel solid is the dispersion medium and liquid the disperse phase. In the presence of excess of electrolytes, the colloidal solutions get coagulated. When a colloidal sol containing impurities is kept in a parch-ment bag, the electrolytes pass through the membrane while colloidal particles are retained by parchment bag. The electrolyte used for this purpose, is called peptizing agent. Hence it is most effective in causing coagulation. Give two examples. Answer. Oil-in-water emulsion is that in which oil forms the dispersed phase and water the dispersion medium. For example, milk and vanishing cream. Give two examples. Answer. Water-in-oil emulsion is that in which water forms the dispersed phase and oil forms the dispersion medium. For example, cold cream and cod-liver oil. It envelopes the droplets of the dispersed phase and therefore they do not coalesce. If the droplets become coloured the emulsion is oil-in-water type and if the medium becomes coloured the emulsion is water-in-oil type. (ii) By dilution test. To the emulsion add a few drops of oil. If the oil forms a separate layer, the emulsion is oil-in-water type, otherwise it is water-in-oil type. In other words, the rate of reaction increases with the increase in the concentration of the reactants. The effect of concentration of reactants on rate of a reaction can be studied easily by the reaction between sodium thiosulphate and hydrochloric acid. Therefore, rate of reaction can be studied by measuring the time taken to produce enough sulphur to make some mark invisible on a paper kept under the conical flask in which the reaction is carried out. When half of the hydrochloric acid solution has been added. Shake the contents of the conical flask and place it on the tile with a cross mark as shown in Fig. Note down the time. It should be a straight sloping line. But y is a direct measure of rate of the reaction, therefore, rate of the reaction between Na 2 S 2 O 3 and HCl is directly proportional to the cone, of Na 2 S 2 O 3 solution taken. Hence, rate of this reaction is directly proportional to the concentration of Na 2 S 2 O 3, which is one of the reactants. Note. It may be noted that the reaction rate also increases when the amount of sodium thiosulphate is kept constant but the concentration of hydrochloric acid is increased. If the same conical flask is to be used again and again, it should be thoroughly washed with cone. HNO 3 and then with water. You must have JavaScript enabled in your browser to utilize the functionality of this website. Products are being added regularly as per availability. We will be available fully soon! It helps to understand the subject more precisely. This contain ample of experiments with proper space provided for writing observation of experiments. It is strictly based on Continuous and Comprehensive Evaluation (CCE). According to the latest syllabus issued by CBSE This course adheres to the guidelines of CCE. These books help students familiarize with the science laboratory and help them acquire the skills needed to perform experiments. Evergreen Publications’ books adjust to many state boards’ syllabi and are therefore widely read by students. Their products range from text books, children’s books, activity books, Manuals, e-Books, company books, magazines, catalogs, diaries and alternative instructional books.This is a platform wherein customers can find all kinds of Books, Stationery, Toys, Games, Sports Goods, Bags and Apparels. The platform enables customers to buy these items online from anywhere in India at a very reasonable price. 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