Experiment 2 – Identification of Inorganic Solids Jesse Galina CHM 101 Lab Monday October 1‚ 2012 Unknown Solid – 2 Identifying my cation was rather easy because of the color of the powder when it was first given to me. It was pinkish/slight red when solid and when it was grounded up even further. This observation ruled out every cation except for some hydrated Co (II) salts. After being dissolved in water‚ the solution turned pink which agrees with the statement that the cation was Co
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carbonate from the mixture. In the second reaction we use the product of the first reaction (CaCl2) and change it back to calcium carbonate (CaCO3) by mixing CaCl2 with potassium chloride (2KCl). Objective To separate the components of mixture of sand‚ sodium chloride and calcium carbonate. Materials and Equipment 1. Two beakers 2. Experimental mixtures 3. Distilled water 4. Funnel 5. Filter paper 6. Evaporating dish 7. Buchner funnel 8. Weighing machine 9. Conical flask 10. Hydrochloric acid(HCl) 11
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According to the table A in the procedure‚ it stated that for formulation 1‚ we were using Sodium Carbonate with sodium chloride as the alkaline salt solution while formulation 2 with Soda Ash with sodium chloride and formulation 3 with Potassium Carbonate with sodium chloride . However for formulation 4‚ we were not using any alkaline solution to make it become as the control product and only used sodium chloride. According to the result in table 1‚ we found that the highest moisture content of
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M10/4/CHEMI/HP2/ENG/TZ1/XX/M+ MARKSCHEME May 2010 CHEMISTRY Higher Level Paper 2 18 pages –2– M10/4/CHEMI/HP2/ENG/TZ1/XX/M+ This markscheme is confidential and for the exclusive use of examiners in this examination session. It is the property of the International Baccalaureate and must not be reproduced or distributed to any other person without the authorization of IB Cardiff. –5– Subject Details: M10/4/CHEMI/HP2/ENG/TZ1/XX/M+ Chemistry HL Paper 2 Markscheme
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was a chemical change? I viewed my other test tubes to see if it there was a chemical change in those. C. Give at least two examples of chemical changes you observed. Zn and MgO when I Diluted HCL D. Classify the following properties of sodium metal as physical or chemical: • Silver metallic color: Physical • Turns gray in air:chemical • Melts at 98ophysical • Reacts explosively with chlorine gas: chemical E. Classify the following changes as physical or chemical: • Water freezes
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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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Qualitative Cation Tests Peter Jeschofnig‚ Ph.D. Version 42-0194-00-01 Lab Report Assistant This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions‚ diagrams if needed‚ and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing
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____1.1______g Mass of Filter Paper plus Benzoic Acid after complete drying: ___1.9_______g Mass of Benzoic Acid: _____0.8_____g 4. Separating out the Salt: Mass of Paper Cup plus Sodium Chloride after complete evaporation of water: ___4.7_______g Mass of Sodium Chloride (use Mass of Paper Cup from #3 to calculate): ___2.2_______g Mass (g) Percent in Mixture* Iron filings 1.9 g 1.9/6.8*100= 28% Sand 1.9 g 1.9/6.8*100= 28% Table Salt 2.2 g 2.2/6
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color change. To tube 3‚ add 5 drops of 1 M ammonium thiocyanate. Mix. Record color change. To tube 4‚ add 5drops of 1 M ammonia solution. Mix. Record color change. B. Calcium oxalate equilibrium Put 5 mL of .1 M calcium chloride and 5 mL of .1 M sodium oxalate into 6 inch test tube. Mix by stoppering and inverting. Equilibrium is established by formation of white precipitate. Add concentrated HCl. Shake after each drop. Record any changes. C. Cobalt chloride equilibrium Heat 2 mL of saturated
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Procedure: Melting point of RCO2H Before observing the melting point of the unknown sample‚ the melting apparatus had to be standardized with a standard substance having the melting point of 151°C-153°C. After placing a small sample of the standard in a capillary tube and inserting the tube into the sample tube holder‚ the plateau on the device was set to 15°C below the expected melting point. After its temperature reached the plateau‚ the temperature increment was set at 1°C per minute‚ and the
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