Identification of Metallic Ions Peter Jeschofnig‚ Ph.D. Version 42-0160-00-01 Kellie Long Purpose: To observe the different flames of alkali and alkaline metals. Procedure: Place a little bit of each element into the well plate. Then you soak a tip of a cotton swab in each solution. Then you place the cotton swab over the Bunsen burner until the flame changes color. observations The color of the flame is expected to be as follows: Metallic ion Flame color
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Cold H2O Hot H2O Litmus Test Dilute HCl Dilute NaOH Mg Small silver‚ metallic‚ shards No smell Shriveled up and turned white. Produced gas insoluble Boiled fast‚ some sample floated to top of H2O‚ and sample jumped around test tube Red= got damp‚ turned dark pink Blue= turned dark blue/purple and light blue/gray where drop hit paper Became very hot‚ bubbled‚ produced gas No reaction‚ not soluble Cu Bronze metallic balls No smell Turned grey and moved around tube insoluble Insoluble
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Testing for Ions Analysis Chemical Changes of Test Solutions Test Solution Silver Nitrate Barium Chloride Potassium Thiocyanate Sodium Sulfate - Stayed white in color - Turned cloudy in color - Precipitation formed in solution - Stayed white in color Potassium Chloride - Turned cloudy in color - Precipitation formed in solution - Stayed white in color - Stayed white in color Iron (III) Nitrate - Stayed orange in color - Stayed orange in color - Changed color from orange
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Name: |Date:| Exp 1: Observations of Chemical Changes|Lab Section: | Data Tables: Part 1: |Chemicals|Well No.|Observations of the Reaction| A.|NaHCO3 + HCl| H12|White and bubbled slightly and settled down to smaller smaller bubbles| B.|HCl + BTB| H11|Golden yellow; looked darker under the black paper| C.|NH3 + BTB|H10 |Dark blue| D.|HCl + blue dye| H9|Greenish color| E.|Blue dye + NaOCl| H8|Blue and lighter than NH3+BTB solution color| | with the 1 drop of HCl| H8|Turned blue green
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Chemistry F332 Notes Ions in solids and solutions: Structure of an ionic lattice (Sodium Chloride): * Consists of sodium ions (Na+) surrounded by six chloride ions (Cl-) * Chloride ions also surrounded by six sodium ions. * Held together by attraction of oppositely charged ions. * Giant ionic lattice. * Electrostatic bonds hold lattices together. * Structure is simple cubic. * Some ionic crystals contain water. * Known as water of crystallisation. * These crystals
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Metallic Bench Vise Date :- 1/10/2011 GC Hafiz Muddassir Bhatti GC Saqlain Musharraf GC Shahid Iqbal PC Zeeshan Raza DE-31 Mechanical Syn (A) Dedicated to all those who accept their errors and use them as their ladder to reach the best Table of Contents ABSTRACT 1 AGENDA 2 UNIT I | INTRODUCTION 3 CHAPTER 1| METALLIC BENCH VISE 3 CHAPTER 2 | APPLICATIONS 4 CHAPTER 3 | OTHER TYPES OF VISES AND THEIR USES 5 Machinist’s Bench
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table List of Polyatomic Ions that Must be Memorized for General Chemistry Polyatomic Cation: NH4+ ammonium ion Polyatomic Anions Ionic Charge: Oxyanions: ClO4– perchlorate ion ClO3– chlorate ion – ClO2 chlorite ion ClO– hypochlorite ion -1 Ionic Charge: Oxyanions that Contain Hydrogen: HCO3– bicarbonate ion or hydrogen carbonate ion HSO4– bisulfate ion or hydrogen sulfate ion NO3– NO2– nitrate ion nitrite ion MnO4– permanganate ion H2PO4– Others: CN–
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Acknowledgement Introduction & Objective Theory Requirements Procedure Observation & Calculation Result Acknowledgement I __________ of class _______ thereby declare that this investigatory project of chemistry on “Study of presence of Oxalate Ion content in Guava fruit at different stages of ripening” is made by my own hard work and efforts under the supervision of our Chemistry Teacher__________________ Signature:___________________ Introduction & Objective Guava is a
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HC2O4−. A salt with this anion is sometimes called an acid oxalate‚ monobasic oxalate‚ or hydrogen oxalate. The equilibrium constant (Ka) for loss of the first proton is 5.37×10−2 (pKa = 1.27). The loss of the second proton‚ which yields the oxalate ion has an equilibrium constant of 5.25×10−5 (pKa = 4.28). These values imply that‚ in solutions with neutral pH‚ there is no oxalic acid‚ and only trace amounts of hydrogen oxalate.[1] The literature is often unclear on the distinction between H2C2O4‚
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