Solution of Sodium Thiosulfate Looks like a clear liquid Granular Zinc Looks like shredded pieces of silver Iodine Crystals Looks like small silver balls Zinc Ion and Iodine-Iodide-Triiodide ion in water Looks like a brown liquid Solid Zinc Iodide Looks like a white powder Mineral Oil Looks like a clear liquid Silver Nitrate Looks like a clear liquid Magnesium Turnings Looks like a small silver curved figure 3M Hydrochloric Acid (HCL) Solution Looks like a clear liquid This table records the observations
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Schmoe Period 3 March 8‚ 2013 Lab Report: Empirical Formula of Zinc Chloride (ZnCl) * Purpose The purpose of this experiment was to learn how to determine the empirical formula. Empirical means “based on experimental evidence.” * Experimental Design The reaction that occurred was the reaction of the elements Zinc (Zn) and Chloride (Cl) by mixing a piece(s) of Zinc and 50mL of Hydrochloric Acid (HCl). The amount of Zinc was determined to be between 1.00g and 1.25g. As the reaction occurred
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its properties of high ductility and conductivity. Results Reagents | Appearance | Volume (or Mass) | Concentration (or Molar Mass) | Cu(NO3)2 (aq) | Light blue solution | 10 ml | 0.10 M | NaOH (aq) | Clear solution | 20 ml | 2 M | HCl (aq) | Clear solution | 20 drops | 6 M | NH3 (aq) | Clear solution | 7 drops | 6 M | H2SO4 (aq) | Clear solution | 15 ml | 1.5 M | Zn dust | Silvery substance | 0.15 g | | ethanol | Clear solution | 5 ml | | Volume
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[PARVATIBAI CHOWGULE COLLEGE(H.S.S)-MARGAO-GOA] Chemistry chart Std-XII Name______________________________________________ Class____________________________________ Div__________________ Roll No___________ Batch No_______ 1 [PARVATIBAI CHOWGULE COLLEGE(H.S.S)-MARGAO-GOA] Chemistry chart Std-XII VOLUMETRIC ANALYSIS REDOX TITRATIONS Experiment No:- 1 Date:--------------- Aim:- You are provided with two solutions as follows. Container A: -----------------M/N Stock Solution of Hydrated
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each clean dry test tube. For the first test 1 mL of 3 M of HNO3 was added. As soon as the acid came into with the solid‚ the pigment was observed to dissolve while also turning the solution into a pale clear colour. The same amount was used for the HCl reagent. As soon as the acid touched the pigment it yielded in a clear solution (solid dissolved after a few shakes). When the KI was added‚ the solution turned a pale yellow with white solid precipitate clumping together at the bottom of the test tube
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Revise the symbols and valency of metals and non-metals. Q1.What would you observe when you put a) Some zinc pieces into blue copper sulphate solution? b) Some copper pieces into green ferrous sulphate solution? c) An iron nail into blue copper sulphate solution? Q2.Complete and balance the following equations: a) Zn + O2 b) Pb + O2 c) Cu + O2 d) Mg + H2O e) Al + HCl f) MgO + H2O g) K2O + H2O h) Cu + HCl __________________ _____________________________ _____________________________ ______________________
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About 1.5 g zinc dust was slowly added to the solution in the previous activity with constant stirring. The chemical changes were observed and noted. It stirred until no reaction is occurring and then more zinc was added to make the solution color less. The completeness of the reaction was tested by adding a few drops of the solution in a test tube containing
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Ans: Add sodium hydroxide to the given substance‚ Calcium nitrate forms milky white ppt. which is insoluble in excess. Lead nitrate forms chalky white ppt. Which is soluble in excess. c)Zinc nitrate and lead nitrate using ammonium hydroxide solution Ans: Add ammonium hydroxide solution to the given substance Zinc nitrate forms gelatinous white ppt. which is soluble in excess. But lead nitrate forms chalky white ppt. With ammonium hydroxide which is in soluble in excess. Q5. Give a chemical test
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more milky with ammonium Zinc 2+ No precipitate Milky white precipitate Precipitate dissolves Unknown No precipitate No precipitate Name Test Tube 3: NH3 Excess Test Tube 4: Confirmation Aluminum 3+ Milky More milky Turns dark pink Ammonium + No precipitate Changes color of paper Calcium 2+ Milky white precipitate appears Copper 2+ Turned dark purple Iron 3+ Turns dark blue Lead 2+ Turns bright yellow Silver + Milky white‚ disappeared then reappeared Zinc 2+ Milky white precipitate
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equations Part I: Reaction between zinc and iodine Watch the Video. http://www.youtube.com/watch?v=xT9V7Y1iKYc Observations: Describe what happened when the water was added. A reaction happened and the iodine exploded into a purple gas Questions and conclusions: 1. Balance the equation‚ if necessary‚ for the reaction between zinc and iodine. Zn + I2 ZnI2 It is balanced 2. Classify the reaction that occurred between the zinc and iodine. redox 3. What evidence
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