Lab 1: Observation of Chemical Changes Name: Tyler Lee Lab Partners: none Date of Experiment: Feb 26 2015 Location: My House Course Number: CHE111 Abstract: The point of this lab was to test and observe chemical changes when mixing chemicals together and also through heating chemicals. Experiment and Observations: The experiment performed in the first part of this lab was to mix various chemical solutions together and then observe and record the chemical changes‚ also if a chemical
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of Eleven Test Tubes Karen Radakovich Ph.D. Mohammad Farhad Brittany Cina CH 223‚ Spring 08 Abstract: Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4‚ 6M NH3‚ 6M HCl‚ 6M NaOH‚ 1M NaCl‚ 1M Fe(NO3)3‚ 1M NiSO4‚ 1M AgNO3‚ 1M KSCN‚ 1M Ba(NO3)2‚ 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9‚ ammonia which was identified by its pungent odor‚ was added‚ an inky dark
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Yes (1) NaOCl + KI No reaction No (2) NaOCl + KI + Starch No reaction No KI + Pb(NO3)2 Bright yellow‚ cloudy‚ precipitate Yes NaOH + C20H14O4 Purple‚ pink‚ opaque Yes HCl + C20H14O4 No reaction No NaOH + AgNO3 Clear pink‚ brown precipitate Yes AgNO3 + NH4OH Milky white‚ cloudy precipitate Yes AgNO3 + NH4OH +
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) reactions. Be sure to balance them. a. MgCl2 + Ba(NO3)2 → b. Al2(CrO4)3 + (NH4)2SO4 → c. K2SO4 + SrCl2 → d. FeCl3 + KOH → e. HCl + AgNO3 → f. K2SO4 + Ba(NO3)2 → 7. (Brown 4.21) Will precipitation occur when the following solutions are mixed? If so‚ write a balanced chemical equation for the reaction. a. Na2CO3 and AgNO3 b. NaNO3 and NiSO4 c. FeSO4 and Pb(NO3)2 8. (4.22 Brown) Identify the precipitate (if any) that forms when the following solutions are mixed
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Combination 4. AgBr(s) = Ag (s) + Br2(l) = 2 Ag + Br2 Combination 5. Mg(s) + H2SO4 (aq) = MgSO4 + H2 Decomposition Table Three: Formation of Salt via Double Replacement Reaction 0.1 KNO3 * (NO3)2 0.1 M AgNO3 0.1M NaCl Tube 1: KNO3+NaCl Tube 3: Fe(NO3)3+NaCl Tube 5: AgNO3+NaCl Prediction No change No change No change Observation Change:
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OBJECTIVE The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1. INTRODUCTION An unknown material can be determined by using simple chemical tests and separations which is called as inorganic qualitative analysis. The separation of cations depends on the difference in their propensity to form precipitates. Separation scheme is used to classify cation into five groups on the basis of their physical and chemical behavior opposed
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These two liquids create one solid. An example of this is the reaction between NaCl and AgNO3. When the two solutions (NaCl and AgNO3)‚ are mixed‚ a precipitate‚ AgCl‚ is formed. Though‚ all with their own differences‚ Combustion and Rodex often work together. Combustion is a chemical reaction which involves oxygen as one of the reactants that produce enough
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precipitate formed. h.NaOH & phenolphthalein. Observations of Chemical Changes i. HCI & phenolphthalein. With phenolphthalein & acid what color do you expect?-clear. What color do you expect with a base?-fuchsia j. NaOH and AgNO3 . k. AgNO3 and NH3 (ammonia). Absorb mixture onto paper towel‚ expose to intense light from a light bulb or the sun. Be patient and observe change. l. NH3 and CuSO4 Experiment Results Almost every solution made had some type of chemical reactivity
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Investigating the Determining Characteristics of Cations and Anions Chem 111 Sec 560 Introduction: The purpose of this lab was to study the specific characteristics of cations and anions‚ and ultimately to be able to identify an unknown substance based on our studies and tests using the logic trees developed through the experiment. A logic tree is a graphical display of the findings from this lab which‚ through a series of yes/no questions‚ elimination
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Initial temperature of silver nitrate‚ AgNO3 /oC y oC Average initial temperature for both solution Highest temperature for the solution z oC Temperature change z – (x + y) oC = Ө oC 2 Chemical equation for the reaction; AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq) Ionic equation for the reaction; Ag+ (aq) + Cl- (aq) AgCl (s) Calculation of heat of precipitation for AgCl; 1. Calculate the number of mole of precipitate formed No. of mol NaCl =
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