Samples | Physical State | Color | Appearance | Solubility in Water | | | | | | Group IA and Group IIA Elements | | | | Li2CO3 | Solid | White | Shiny Powder | Soluble | Na2CO3 | Solid | White | Refined Powder | Soluble | K2Co3 | Solid | White | Powder | Soluble | MgCO3 | Solid | White | Unrefined Powder | Insoluble | CaCO3 | Solid | White | Powder | Insoluble | BaCO3 | Solid | White | Crystalized Powder | Insoluble | | | | | | Some Group IVA Elements | | |
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equation was 2NaHCO3(S) > Na2CO3(s) + CO2(g) + H2O(g). The procedure consisted of gathering measurements and observing. The first step was to gather all the necessary materials. Next we had to have the accurate measurements of the crucible with and without the substance that is Sodium bicarbonate. The Crucible had a mass of 11.53g and then 13.94g with Sodium bicarbonate. Subtracting it to find out the
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r Lab Report 5 Introduction to the Classes of Chemical Reactions Course: Chem. 1151L‚ Tuesday & Thursday June 23‚ 2011 Mr. Nasir Uddin Pre Lab Questions: 1. CaBr2 (aq) + K3PO4 (aq) → CA(PO4)2(S) + KBr (aq) = Ca3(PO4)2 + 6 KBr Double Replacement 2. Li(s) + O2(g) = Li2O(s) =2 Li2O Decomposition 3. CH4 + O2 = CO2 + H2O = CO2 + 2 H2O Combination 4. AgBr(s) = Ag (s) + Br2(l) = 2 Ag + Br2 Combination 5. Mg(s) + H2SO4 (aq) = MgSO4 + H2
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water was evaporated 1.00 g of sodium carbonate and 1.00 g of lead II nitrate was given to start the lab out with. To calculate the percent yield of lead II carbonate‚ the limiting reactant must be identified first. 1.00 g Na2CO3 x 1 mole106 g = 0.00943 mole Na2CO3 1.00 g Pb(NO3)2 x 1 mole331 g = .00302 mole Pb(NO3)2 Limiting reactant: lead II nitrate Next‚ the theoretical yield of lead II
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of HCl is titrated with a known volume of NaOH‚ then one can gather enough data to determine the concentration of the unknown which is HCl. Procedure Standardization of ~0.10M HCI 1- Weigh duplicate ~0.15 g samples of previously dried standard Na2CO3 Dissolve samples in ~100-ml distilled water; if it does not dissolve quickly‚ you may warm the solution. 2 - Cool the solution to room temperature and add ~ 0.5 to 1 ml of bromocresol green indicator‚solution turns into blue. Titrate it with HCl until
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it was for only 3 of the results shown above. The average titre is shown below: 16.60 + 16.60 + 16.30 = 49.50 / 3 = 16.5cm3 Going back to the beginning the equation for the reaction that is taking place is as follows: Na2CO3 (aq) + H2SO4 (aq)  Na2SO4 (aq) + CO2 (g) + H2O (l) Concentration of sodium carbonate solution In this experiment‚ a solution carbonate had to be made. This was done by mixing sodium carbonate with distilled water
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Flame Tests The flame testing is a method used in chemistry to detect the presence of certain ions‚ primarily metal ions‚ based on each element’s characteristics emission spectrum. The colour of the flames normally depends on the temperature. Different types of Bunsen burner with flame types depend on the oxygen supply. The flame of rich fuel with no premixed oxygen produces a yellow diffusion flame. The flame of lean fully oxygen premixed flame produces no soot and the flame colour is produced
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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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Anionic | NaCl | Green | 8 | Neither | (NH4)Cl | Green- yellow | 7 | Neither | (NH4)2SO4 | Green- Yellow | 7 | Neither | AlCl3 | Red-orange | 3 | Cationic | Ca(NO3)2 | Murky green | 7 | Neither | Fe2(SO4)3 | Red | 2.5 | Cationic | Na2CO3 | Dark blue | 9.5 | Anionic | Na3PO4 | Orange-red | 3 | Cationic | K2SO4 | Green | 7 | Neither | KBr | Green | 8 | Anionic | (NH4)2C2O4 | Green | 8 | Anionic | NH4CH3COO | Blue green | 9 | Anionic | (NH4)2CO3 | Blue green | 9 | Anionic
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What’s in a Medicine? (WM) In this document you will find the following material to cover the new AS specification with your students. Notes for students and teachers Revised Chemical Ideas 13.4 part b Answers to problems for 13.4 part b Revised activity WM3 Answers to questions for revised activity WM3 Revised check your notes Revised map of the unit 2 3 6 7 9 10 11 WM © Harcourt Education Ltd 2004 Salters Advanced Chemistry These pages have been downloaded from www.heinemann.co.uk/science 1 Notes
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