sublimates; principle of flame test‚ borax-bead test‚ cobalt nitrate test‚ fusion test‚ chromyl chloride test; analytical reactions for the detection of nitrate‚ nitrite‚ halides‚ phosphate‚ arsenate‚ arsenite‚ sulphide‚ thiosulphate‚ sulphate‚ thiocyanate‚ borate‚ boric acid‚ carbonate. Analytical reactions for the detection of Cr3+‚ Fe3+‚ Ni2+‚Cu2+‚ As3+‚ Mn2+‚ Importance of common-ion effect in the separation of Group II cations‚ and Group III cations. Unit II. Basic inorganic chemistry III
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Chloride in Urine in Different Circumstances Aim: To determine the chloride content by titrating mixtures of urine against potassium thiocyanate under in different circumstances. Research Question: How do different conditions of urine samples collected affect its concentration of chloride which is measured by titrating the mixture of urine with potassium thiocyanate until it turns red? Hypothesis: The greater the consumption of food‚ the higher the chloride concentration in urine. This can
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f (water) Hv (water) 334 J/g 2‚260 J/g J for ice‚ 2.02 J for steam‚ g°C g°C J for liquid 4.18 g°C 2.05 Specific heat of water C p (water) Metal Specific Heat J g°C Density (g/cm3) Melting Point (°C) Aluminum Copper Gold Iron Lead Magnesium Mercury Nickel Titanium Zinc 0.897 0.385 0.129 0.449 0.129 1.023 0.140 0.444 0.523 0.388 2.702 8.92 19.31 7.86 11.3437 1.74 13.5939 8.90 4.5 7.14 660 1083 1064 1535 328 649 —39 1455 1660 420 NCDPI Reference Tables for Chemistry
Free Hydrogen Oxygen Chlorine
ion Te2¯ telluride brom-. strontium ion barium ion Ag + silver ion N 3¯ nitride radium ion Ni2+ nickel ion P 3¯ phosphide 3+ 3¯ zinc ion Al aluminum ion As arsenide Systematic name (Stock system) copper(I) copper(II) iron(II) iron(III) tin(II) tin(IV) chromium(II) chromium(III) manganese(II) manganese(III) Common name cuprous cupric ferrous ferric stannous stannic chromous chromic manganous manganic Symbol Hg22+ Hg2+ Pb2+ Pb4+ Co2+ Co3+ Au
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1. Disposing of Waste - Teachers should be aware of the appropriate method of disposal for any chemical used in the school laboratory. When in doubt‚ refer to the MSDS‚ a disposal manual‚ or the source of the chemical. a. Classification of Hazardous Waste The Environmental Protection Agency classifies wastes as: Ignitable: has a flash point below 140°C‚ is an oxidizer‚ or is an ignitable compressed gas. Corrosive: has a pH equal to or below 2.0 or a pH equal to or greater than 12.5. Reactive:
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silver iodide 7783-96-2 AgIO3 silver iodate 7783-97-3 AgMnO4 silver permanganate 7783-98-4 AgN3 silver azide 13863-88-2 AgNO3 silver nitrate 7761-88-8 Ag2O silver oxide 1301-96-8 AgONC silver fulminate 5610-59-3 AgSNC silver thiocyanate 14104-20-2 Ag2C2 silver acetylide 7659-31-6 Ag2CO3 silver(I) carbonate 534-16-7 Ag2C2O4 silver oxalate 533-51-7 Ag2Cl2 silver(II) dichloride 75763-82-5 Ag2CrO4 silver chromate 7784-01-2 Ag2Cr2O7 silver dichromate Ag2F silver
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Chemical Thermodynamics Chapter 19 Lecture Worksheet Homework: 19.29‚ 19.31‚ 19.37‚ 19.39‚ 19.41‚ 19.43‚ 19.47‚ 19.51‚ 19.53a‚ 19.55‚ 19.61‚ 19.73‚ 19.75‚ 19.77 Recall from Chapter 5 - 1st Law of Thermodynamics o Energy is neither ____________________________________________. o Energy of the universe is constant. o Enthalpy Change ▪ Heat energy transferred at _____________________________________ ▪ Negative
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forward and backward reactions are the same‚ it is said to be in a state of dynamic equilibrium. The position of this dynamic equilibrium can be moved forward by changing the conditions the reaction is done in. This follows Le Chatelier’s Principle which says changes to a system in equilibrium will move it in an opposite direction. Condition (Dependent Variables) | Effect (Independent Variables)-Yield‚ Equilibrium Time‚ Net Profit | Pressure | Increasing this will improve the yield because the
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Testing for Cation and Anions OBJECTIVE: • Determine the presence of a cation or anion by a chemical reaction • Determine the cation and anion in an unknown solution All salt solutions have both positive (Cations) and negative (Anions) ions dissolved in it. In this experiment you will observe chemical reactions to determine the presence of specific anions and cations. Compare your observations with the reactions of the known solutions and the unknown solution to determine the ions present
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the mixed sample. 8 Estimation of Sugar by Lane-Eynon method. 9 Estimation of acid concentration using conductometry. 10 Estimation of copper in brass. 11 Estimation of lead as lead Sulphate. 12 Estimation of Iron using colorimeter. INSTRUCTIONS 1. Get your Completed observation book signed‚ on the day of the experiment itself or maximum by the next day. 2. Write the procedure in your record note book in “PAST PASSIVE SEANTENCES ONLY” 3. Concerned
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