PRINCIPLES OF CHEMISTRY LAB I Experiment 2 Separation Of Mixtures INTRODUCTION A mixture can simply be defined as a substance that is made up or consists of two or more elements and/or compounds that are physically combined but that have not reacted chemically to form new substances. A mixture may be a solid‚ liquid‚ gas‚ or some combination of those states. Mixtures can be found almost every wher in our everyday lifes and some common examples are * sand and water * salt and water
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Determination of the Equilibrium Constant for Ferric Thiocyanate In this laboratory exercise‚ the equilibrium constant(Kc) for the reaction between the Ferric Ion (Fe3+) and the Thiocyanate Ion (SCN-) was determined. After measuring the absorbance of the Ferric Thiocyanate‚ and carrying out some calculations; it was determined that Kc=130.81M Introduction: Chemical equilibrium is established when a reaction exists in a state where the forward reaction rate is equal to its reverse reaction
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interfere with the functions of that metal. Aim: the aim of this experiment is to evaluate the effect that sodium chloride has on the rate of corrosion of iron. 1. Experiment 1 2. Hypothesis: An increase in the level of sodium chloride in water will increase the rate of corrosion of an iron nail. 3. The independent variable is the amount of sodium chloride in the water 4. The dependent variable is the rate of corrosion; this will be measured by calculating the percentage
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Cesium (Cs) Pink – Potassium (K) Yellow/Green – Copper (Cu) Orange – Carbon (Ca) 3. Let’s say that the three bottles contain Fe(NO3)3‚ BaCl‚ and AgNO3. These are Iron (III) Nitrate‚ Barium Chloride‚ and Silver Nitrate. All of these are white solids that dissolve in water. We know that silver chloride is highly insoluble in water. So if we reacted an aqueous solution of each of the chemicals with a dilute solution of hydrochloric acid (HCI)‚ the one with Ag+ in it will form AgCl and precipitate
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(solute)‚ the vapour pressure above the liquid is reduced. You are to plan an experiment to investigate how the boiling point of an aqueous solution of potassium chloride depends on the concentration of the solution. (a) (i) By considering how the vapour pressure changes as the concentration of the aqueous potassium chloride increases‚ predict and explain how the boiling point of the solution will be affected by the concentration of the solution. Predict how the boiling point will change
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TABLE OF CONTENTS 1. IA (Alkaline Metals) 1.1. H………………………………………………………………………..2 1.2. Li………………………………………………………………………..2 1.3. Na………………………………………………………………………2 1.4. K………………………………………………………………………..3 1.5. Rb………………………………………………………………………3 1.6. Cs………………………………………………………………………3 1.7. Fr……………………………………………………………………….4 1. IIA (Alkaline Earth Metals) 2.8. Be………………………………………………………………………4 2.9. Mg………………………………………………………………………4 2.10. Ca………………………………………………………………………4
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the salt (NaCl) left from the perspiration on the friction ridge skin to form solid silver chloride (AgCl) and sodium nitrate. The silver chloride can then be converted to silver oxide (Ag2O)‚ which is dark in color and can be more easily seen. Challenge Suppose the fingerprint processing technique that uses silver nitrate to react with the salt from perspiration produced 5.8 x 10-2 grams of silver chloride. How many grams of salt was left by the initial latent fingerprint? Brainstorm the steps
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subsequently cooled either in open air‚ slowly in the furnace or quenched in furnace oil. Hardness of the heat treated and without heat treated specimen was measured in the Rockwell Scale. Corrosion resistance of the sample was evaluated in 3.5 % sodium chloride solution by weight loss method. It was found that specimen heat-treated at 500 °C showed higher hardness and corrosion resistance compare to that heat-treated at 300°C and 600 °C. Oil quenching specimen provided maximum hardness and corrosion resistance
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came very close to passing all the tests‚ but only one substance was able to pass all of them. I recommend using sodium carbonate as your substance. Of all the substances‚ only two were covalent and two were ionic. The ionic substances‚ sodium chloride‚ sodium carbonate‚ and salicylic acid‚ came close to the description you requested. The covalent substances‚ sucrose and salicylic acid‚ did not match the descriptions. The best substance would definitely be sodium carbonate‚ since it passed all
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acid with N‚N-dimethylaniline. Materials (Chemicals) Sulfanilic acid‚ 2.5% aqueous sodium carbonate solution‚ sodium nitrite‚ concentrated hydrochloric acid‚ N‚N-dimethylaniline‚ glacial acetic acid‚ 10% aqueous sodium hydroxide‚ saturated sodium chloride solution Apparatus 50 mL Erlemeyer flask‚ 250 mL beaker‚ test tube‚ hot plate‚ Buchner funnels Procedure In a 50 mL Elermenyer flask 1.2 g of sulfanilic acid and 12.5 mL of 2.5% aqueous sodium carbonate solution was placed. The flask was
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