“One cation replaces another” and in an anion replacement reaction‚ “one anion replaces another from its solution.” When magnesium and copper sulfate react‚ a single replacement reaction occurs‚ and copper and magnesium sulfate are produced (Mg + CuSO4 MgSO4 + Cu). In this example‚ magnesium is above copper in the activity series so it is able to displace copper. An example of an anion replacement reaction is the reaction of bromine and potassium iodide‚ which produces potassium bromide and iodide
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CHM 256: BASIC ANALYTICAL CHEMISTRY TUTORIAL 1: INTRODUCTION: ANALYTICAL CHEMISTRY 1. What is chemical analysis? 2. Differentiate between qualitative and quantitative analysis (Oct 2008‚ 2009‚ Dec 2009‚ Apr 2010) 3. Give 7 steps in performing any chemical analysis (Apr 2010) 4. Briefly explain how to prepare the following solutions: a) 1.0 L 10.50 % (w/v) aqueous CH3CH2CH2OH (answer : 105 g) (Oct 2006‚ Oct 2007‚ Oct 2008) b) 500 mL 2.0 M H2SO4 from a commercial reagent‚ at 90% (w/w) purity
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identity. First we will place 0.5 mL of each solution in the 24-well plate. I placed the following solutions in the following locations: SOLUTION WELL PLATE LOCATION Sodium Nitrate NaNO3 A1 Strontium Nitrate Sr(NO3)2 B1 Potassium Nitrate KNO3 C1 Barium Nitrate Ba(NO3)2 A6 Cupric Nitrate Cu(NO3)2 B6 Lithium Nitrate LiNO3 C6 Calcium Nitrate Ca(NO3)2 D6 Unknown C4 I assembled my needed equipment‚ my burner fuel‚ my non-plastic middle cotton swabs and my well plate with the
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constructed by placing a piece of metal into a 1.0 M solution of its ions for each metal in the series. The metals are Cu‚ Fe‚ Pb‚ Mg‚ Ag‚ and Zn. The half-cells are connected by a salt bridge constructed of a strip of filter paper soaked in a solution of KNO3. The zinc half-cell is used as the reference standard and assigned an E of 0 volts‚ and all reduction potentials are measured with respect to the zinc electrode. In Part 2‚ the Nernst equations applied to the voltage measurement of a cell with nonstandard
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produce that visible sign‚ as observed by me and my partner in Reactant 3 Table B. b. Na2S(aq) + 2HCl(aq) H2S(g) + 2NaCl(aq) In this example we see that the dihydrogen sulfide is the gas the forms out of this reaction HNO3(aq) + KOH(aq) KNO3(aq) + H2O(l) In this example the acid and base react to form a salt and water 5. a. 2K2Cr2O7(aq) + 3AlBr3(aq) 1KBr(aq) + 6Al2(Cr2O7)3(s) b. I know that a precipitate forms because of the 1 aqueous solution as part of the product‚ and because
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WORKSHEET MOLE By Sir Shah Murtaza Q1. Potassium reacts with water as shown in the equation. a. Describe what you would see when potassium reacts with water. b. A sample of 0.195 g of potassium was added to 500 cm3 of cold water. When the reaction was finished‚ 100 cm3 of 0.100mol/dm3 hydrochloric acid was added to form solution X. (i) Calculate the number of moles of hydroxide ions formed when the potassium was added to water. (ii) Calculate the
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Source 1 Hotbox Food would like to present a line of delicious beverages in completely self heating cans. Thanks to these innovative containers called “Hotshots”‚ it is now possible to drink high quality beverages at any time and at any place. Neither an external heat source‚ nor any other cooking utensils are required. Drinks 2go recipes do not contain additives‚ preservatives‚ artificial colorings or any raw materials obtained from GMO (Genetically Modified Organisms). Source 2 In one version
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Chemical Reactions Lab Objectives: 1. To examine a variety of reactions including precipitation‚ acid-base‚ gas forming‚ and oxidation-reduction reactions. 2. To identify the products formed in these reactions and summarize the chemical changes in terms of balanced chemical equations and net ionic equations. 3. To identify the species being oxidized and reduced in oxidation-reduction reactions and determine which species is the oxidizing agent and the reducing agent. Chemical equations represent
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one should have graphed various known measurements of molarity versus absorbance of the copper(II) sulfate solution. Material: * 4-25 mL volumetric flasks * Cuvettes * Pipettes * Spectrophotometer 20 * Distilled water * CuSO4 Procedure: 1. Label 4-25 mL volumetric flasks with 0.1M‚ 0.2M‚ 0.3M‚ and 0.5M. 2. Pipette 5 mL of 0.5M solution into 0.1M flask and dilute to the mark‚ mix. 3. Pipette 10 mL of 0.5M solution into 0.2M flask and dilute to the mark‚ mix
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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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