Instructions You must SHOW WORK AND PROBLEM SET-UP for CREDIT. You have to SUPPORT your answers by calculations and/or reasoning. If you do not understand something in the assignment or are not sure how to approach a question - EMAIL me before you submit. This assignment must be submitted no later than November 22nd‚ 2011. 1. What is a true solution? Explain why the solute does not settle out of a solution. Is it possible to have one solid dissolved in another? Explain. In metals it would
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information to efficiently find an unknown Halogen. Experimental Procedure: View pages 25-28 in the lab Manuel. Data and Observations: Relative Soluabilites of some Salts in Alkaline Earths | 1 M Na2CO3 | 1M H2SO4 | 1M (NH4)2C2O4 | 1M K2CrO4 & 1M HC2H3O2 | Ca(NO3)2 | 1/2 clear‚ 1/2 Milky | Clear | Milky White | Clear yellow hinge | Ba(NO3)2 | Milky White | Milky White | Milky White | Milky Yellow | Mg(NO3)2 | 1/2 clear‚ 1/2 Milky | Clear | Clear | Clear yellow hinge | Sr(NO3)2
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(sulphite)‚ S2(sulphide)‚ NO2- (nitrite): Salt + dil H2SO4 1. No reaction: Group I anion not present. Continue to group II. 2. Carbonate: Colourless and odourless gas (CO2) 1. WE 1 + MgSO4 = white ppt 3. Sulphite: Colourless gas with pungent smell 1. WE + BaCl2 (aq) = white ppt soluble in dil HCl 1 Water extract: Pinch of salt + water www.ankurb.info 3. Bromide: Reddish brown vapour 1. Silver nitrate
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Purpose: To observe the reactions of specific aqueous solutions with specific aqueous reagents. Introduction: A solution is as a homogeneous mixture containing two or more substances. Reagents are added to solutions to create a chemical reaction or added to see if anything occurs. Reagents can be added to solutions to see if there is a presence of other substances. For example‚ iodine added to a lead solution. Iodine would be the reagent and would cause a chemical reaction confirming the presence
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Worked solutions to student book questions Chapter 2 Analysis by mass Q1. a b Why was the soup sample in Worked Example 2.1 heated to 110°C? Why was it necessary to weigh the sample four times? A1. a b The soup was heated above 100°C to evaporate water from the sample. By repeatedly heating the sample until the mass remained unchanged‚ the analyst could be sure that all the water had been removed. Q2. Some laboratories use microwave ovens in place of conventional ovens to
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sulfate and calcium hydroxide are mixed. Al2(SO4)3(aq) + 3 Ca(OH)2(aq) 3 CaSO4(s) + 2 Al(OH)3(s) 2 Al3+ + 3 SO42- + 3 Ca2+ + 6 OH- 3 CaSO4(s) + 2 Al(OH)3(s) 6. Solutions of potassium chromate and lead acetate are mixed. K2CrO4(aq) + Pb(C2H3O2)2(aq) PbCrO4(s) + 2 KC2H3O2(aq) 2 K+ + CrO42- + Pb2+ + 2 C2H3O2- PbCrO4(s) + 2 K+ + 2 C2H3O2- 7. Solutions of silver nitrate and ammonium sulfide are mixed. 2 AgNO3(aq) + (NH4)2S(aq) Ag2S(s) +
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H 204 – Introduction to Chemical Practice Experiment # 1– Qualitative Analysis of Cations Rachel Sorrells Gretchen Diede TA: Kunal Punjabi February 16‚ 2017 RESULTS & DISCUSSION The purpose of this experiment was to utilize two different methods of qualitative analysis to determine the identity of two unknown cations in an unknown solution. The experiment required knowledge of solubility rules and demonstration of such in the laboratory setting for the first method of qualitative analysis. The
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Unit 2 Online Simulation-II (50 points) VLab: Precipitation Reactions: Data & Observations Navigate to: http://www.sascurriculumpathways.com/portal/#/search?searchString=&searchSubject=3&searchCategory=20 Enter the following username: job5circle (No password required) Enter 867 GO There are thirty-five combinations of aqueous solutions for you to investigate. (Note Table 1 on the Data Sheet.) Some of these combinations will produce precipitates; others will not. Step-by-step
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LE CHATELIER’S PRINCIPLE Castro‚ Lharize C. Experiment # 1 I. Introduction: In this experiment‚ using Le Chatelier’s principle‚ we will observe several responses of a system at equilibrium to various changes in external conditions. The experiment aims to investigate two equilibrium systems: (a) cobalt complexes and (b) chromate-dichromate equilibrium and explain observations in light of the Le Chatelier’s principle. II. Theory/Concepts: In 1884 the French chemist and engineer Henry-Louis
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Chapter 4 Fundamentals of Material Balances Material Balance-Part 1 Process Classification 3 type of chemical processes: 1. Batch process – Feed is charge to the process and product is removed when the process is completed – No mass is fed or removed from the process during the operation – Used for small scale production – Operate in unsteady state March 31‚ 2009 ChE 201/shoukat@buet.ac.bd 2 Process Classification 2. Continuous process – Input and output is continuously
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