PDF | complete principle knowledge and experimental in analytical chemistry. View: PDF | PDF w/ Links Practical Chemistry (For Intermediate Science Students). A Manual of Practical Inorganic Chemistry, Qualitative Analysis, and . The major goals of the practical courses are that you. • acquire basic chemical laboratory techniques and learn the safe manipulation of chemicals and chemical .
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CHEMISTRY / LABORATORY. Reference Material. Page # in. Lab Manual. • Goals for CHM & Laboratory Experiments and Reports. 1. A text-book of practical chemistry. April, ~92I.] BOOK NOTICES. 56~ the Faraday Society, the Royal Microscopical Society and the Photomicrographic Society. basic principles of chemistry resgoderfita.tk - Download as PDF File .pdf), Text File .txt) or read online.
A f t e r some reference to the state of the art, and reminders of the importance to both Britain and America of so cultivating the practical side that these nations may be independent of all others, the general history of the microscope is taken up.
It is shown by a quotation that Seneca knew that curved surfaces will magnify, and it is stated to be probable that the manuscript illuminators of the fifteenth century were familiar with moderate magnifyfilg apparatus. The first illustrated publication which gives definite evidence of the use of a magnifying glass appeared in I at Frankfort, bearing the name of George Hoefnagel.
It consisted of a series of plates engraved on copper illustrating common natural objects, but drawn with great skill and minute accuracy. Some of the drawings reveal details that are hardly distinguishable to the unassisted eye. A Dutchman, Zacharias, miscalled Jansen, and his son, made microscopes before the year I In I, Hooke published his famous book " Micrographia," in which he described using small drops or globules of glass.
A fac-simile of the title page of the book is given.
A good deal of space is given to the subject of metallography, which though comparatively recent in its extensive applications, and in the efforts to construct apparatus for its pursuit, yet is really over a century old, the method having been first used by Widmanstiitten in i8o8, who polished a specimen of meteoric iron and examined the surface.
His work is preserved in the title " WidmanstStten F i g u r e s " applied to the phenomenon. Years before, however, he had laid the foundation of one of the most important applications of microscopy--petrography--the extensive ramifications of which are now one of the most prominent features of mineralogy and geology.
The book is illustrated by a large number of excellent plates and many illustrations in the text. Necessarily, being made up of the contributions of many persons and of notes of extemporaneous discussions, the subject matter is somewhat disconnected, but the material presented is all of importance and value, and the book constitutes one of the best of recent publications in the field of pure and applied microscopy.
Hood, M. Carpenter, M. Philadelphia, P. Blakiston's Son and Co. To those whose first descriptions of laboratory manipulations were derived from Morfit's Chemical Manipulations, the contrast with the modern works in this field is sufficiently striking. Measure another 40cm3 of solution B.
Minutes and hours are also common. Some reactions are too slow to be determined e. Repeat the procedure by measuring 35cm3 of solution B and adding 5cm3 of water. Complete the table 1 below by using other values os solution B and water 18 All high school revision materials are available on www. This involve mainly identification of ionic compounds containing cations and anions. Temperature iii State another factor that would not alter the rate of the above reaction.
Surface area Pressure Catalyst b Temperature An increase in temperature increases the rate of reaction. Decrease in concentration decreases the rate of reaction. Increased temperature reverses the table I time results i. An increase in temperature increase the kinetic energy of reacting particles increasing their collision frequency Practically. The main precipitating reagents used are: Cl b If the white precipitate is added dilute nitric V acid: Cl21 All high school revision materials are available on www..
All the others are white precipitates. PbCl2 PbS is a black precipitate.. PbI2 is a yellow precipitate. Divide the mixture into five portions. Heat gently then strongly. Inorganic qualitative analysis require continous practice discussion Sample presentation of results You are provided with solid Y aluminium III sulphate VI hexahydrate.
Carry out the following tests and record your observations and inferences in the space provided. Shake thoroughly. Add about 10cm3 of distilled water. To the fourth portion. To the portion in iv I above. To the portion in iv II above. Observation White ppt.
This involve mainly identification of the functional group: C These functional groups can be identified by: The general philosophy of methods of presentation of chemistry practical data is therefore availability of evidence showing: This tabulated results is usually then put in a graph. Index No……………. Mathematical tables and electronic calculators may be used. This paper consist of 8 printed pages..
File:Chemistry Lab Practical for students of class XII.pdf
All working must be clearly shown where necessary. Name ……………….. Sign and write the date of examination in the spaces provided above Answer all questions in the spaces provided.
Candidates should check the question paper to ascertain that all the pages are printed and indicated and that no questions are missin For examiners use only Question Maximum Candidates score core 1 20 20 2 10 10 3 10 10 Total score 40 40 26 All high school revision materials are available on www..
Date done………………Date marked…………. Table 1 Repeat this procedure to complete table 1. Heat this solution to about 70oC but not to boil. Pipette You are provided with: Procedure 1 Fill the burette with solution M. Shake thoroughly during the titration. Titrate the hot solution L with solution M until a permanent pink colour just appears.
Table 1 1 Final burette reading cm3 Initial burette reading cm3 Volume of N used cm3 Heat the conical flask containing solution N to about 70oC. Titrate while hot with solution M. Repeat the experiment to complete table 2.
Fill the burette with sodium hydroxide solution P. Repeat the procedure to complete table 3. Titrate this solution N with solution P from Table 1 the burette. Pipette 25cm3 of solution N into a conical flask and add drops of phenolphthalein indicator. Calculate the number of moles of ethanedioic acid that were used in the reaction. You are to determine the molar mass of solid B.
You are provided with 5. Stir continuously using the thermometer and record the highest temperature change to the nearest 0.
After Table 2 seconds. Procedure Place cm3 of liquid L into a plastic beaker. To the first portion add three drops of universal indicator. Assume density of liquid L is 1. Observation Inference 1mark White ppt. To the second portion.
To the 1st portion. To the third portion. Heat to boil Observation Inference 1mark White ppt. Divide the mixture into 4 portions.
To the 3rd portion. To the 4th portion.
To the 2nd portion. Fill a burette with solution B and use it to titrate the mixture in the conical flask until it just turns orange yellow. Add 2cm3 of solution D to the mixture in the conical flask. Procedure 1 1. Record your results in table 1 below. Name ………………………………………………. Solution B. Using a pipette and pipette filter. Aqueous Potassium iodide. Repeat the procedure and complete table 1. Add 10cm3 of 2M sulphuric VI acid to the mixture and shake. Meassure 10cm3 of aqueous potassium iodide and add it to solution A in the conical flask.
Solution A containing an oxidizing agent A.
You are required to determined the: Concentration of solution A Rate of reaction between the oxidizing agent A and the reducing agent C. Solution D. Solution C containing a reducing agent C. Index Number……………. Continue titrating until the mixture just turns colourless.
Shake the mixture. Using the burette.
Using a clean burette. Using a burette.
Clean the burette and rinse it with about 5cm3 of solution C 5. Swirl the contents of the beaker. Using a 10ml measuring cylinder. Record the time taken for a blue colour to appear in table 2. Label six test tubes as 1. Repeat steps 5 to7 using the contents of test-tube 2. Use solution E for experiment i and ii i To 2cm3 of solution E in a test tube in each of experiment I.
Add 20cm3 of distilled water and shakeuntil all the solid dissolves. Write your observations and inferences in the spaces provided a Place all solid in a boiling tube. Label the solution as solution E.
File:Chemistry Lab Practical for students of class XII.pdf
III and IV add: You are provided with solid E. CO No white ppt IV. Carry out the experiments below. You are provided with solid F. Add about 10cm3 of distilled water and shake thoroughly.
Carry out the following test. Dry the residue between filter papers. Add about 20cm3 of distilled water and shake until all the solid dissolves. Add the piece of aluminium foil provided to the mixture and shake. Filter the mixture.
Write your observations and inferences in the spaces provided.Put 5cm3 of 2M sodium hydroxide solution into each test tube. The use of the measuring rod for extreme accuracy, which apparently is stressed by Prof. Your name. Some of the drawings reveal details that are hardly distinguishable to the unassisted eye. Interfacial Tension Micrometer Syringe Method Table 1 1 Final burette reading cm3 Initial burette reading cm3 Volume of N used cm3 Surface Tension using a Traube Stalagmometer III and IV add: Molecular Weight using van der Waals' Equation 2.