Carlie Haeffner Qualitative Analysis March 20‚ 2015 The purpose of this lab is to identify unknown ions in a solution by using a type of chemical reaction called precipitate reactions. The key to finding which ions are present in a solution is to form a precipitate which makes the ions “come out” in a reaction (McNeil‚ 2013-2014). Water is used in these experiments to act as a solvent. Since water is a polar molecule‚ the slightly positive and negative charges will sometimes pull apart molecules
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dihydrate‚ BaCl2(2H2O‚ has two waters of crystallization‚ or two waters of hydration. Other hydrates have waters of hydration ranging from one to twelve. Upon heating‚ a hydrate decomposes and produces an anhydrous salt and water (in the form of steam). BaCl2(2H2O (s ) ( BaCl2 (s) + 2 H2O (g) Examples and Problems Problem 1-Theoretical Percentage Calculate the theoretical percentage of water in barium chloride dihydrate. Solution: The formula mass of BaCl2(2H2O is
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EXPERIMENT 1 IDENTIFICATION OF UNKNOWN COMPOUNDS Date of experiment : 7th August 2012 Venue: ME204 INTRODUCTION Chemical reactions are regularly categorized into 3 types: oxidation-reduction (redox reaction)‚ precipitation (double displacement) and acid-base reaction (double displacement) Type 1: Oxidation-Reduction Reactions Oxidation-reduction processes include the movements of electrons form oxidants to reductants‚ which lead to increases in oxidation
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cations and anions‚ as well as observing‚ and documenting the chemical reactions. We will be demonstrating the reaction between a solution of Lead Nitrate with a chemical formula of PbNO3 2‚ and a Potassium Chromate solution with a chemical formula of K2CrO4. The end result from mixing the two solutions should have a combined set of either the Pb2+ or K+ cation and likewise with the NO3 2- or CrO4 2- anion in its chemical formula. This experiment will demonstrate the chemical reaction between the cations
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Selective Precipitation of the Barium Magnesium Group ABSTRACT The purpose of this lab was to identify the cations from the barium magnesium group present in an assigned unknown solution through selective precipitation. This was a qualitative lab where the theory of the common ion effect was used in several steps. Once the experiment was completed‚ it was determined that unknown solution #4 contained Ba2+‚ Sr2+‚ and Mg2+ ions. INTRODUCTION Selective precipitation is a part of chemistry
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Qualitative Observations of Double Displacement Reactions Lab Table 1.0 Qualitative Observation of Products Formed |Balanced Chemical Equations |Qualitative Observations | |BaCl2 (aq) + 2NaOH (aq)( BaOH2(aq) + 2NaCl(s) |An aqueous solution formed | | |Precipitate
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In which case van’t Hoff factor is maximum ? (A) KCl‚ 50% ionised (B) K2SO4‚ 40% ionised (C) SnCl4‚ 20% ionised (D) FeCl3‚ 30% ionised 5. Solution having osmotic pressure nearer to that of an equimolar solution of K4[Fe(CN)6] is: (A) Na2SO4 (B) BaCl2 (C) Al2(SO)3 (D)C12 H22O11 6.(a) Two aqueous solutions‚ one of the NaCl in water (A) and the other of C8H15O2Na in water (B) are isotonic. If wA and wB are weight fractions of NaCl and C8H15O2Na in solution A and B respectively‚ then (assuming that
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original sample and their formula weights (to create a gravimetric factor)‚ the percent of the species to be determined can be calculated. In the analysis for sulfate‚ the sample to be analyzed is brought into solution and reacted with a solution of BaCl2‚ a source of Ba2+‚ to yield BaSO4 as a white precipitate. In the procedure‚ the solution is first acidified with HCl(aq) to: a) prevent the precipitation of BaCO3 and Ba(OH)2‚ and b) aid the formation
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formation of a precipitate. Materiel needed: Test tubes Rack of test tubes Plastic droppers Beakers Procedure: We prepare 7 beakers of 7 different solutions (that we mark from 1→ 7). We put separately around 50 ml of: HCl NaOH Na2CO3 K2CrO4 CaCl2 CuSO4 Unknown substance Using plastic droppers we mix 10 drops of one solution with 10 drops of another solution in a test tube‚ to get all in all 20 different test tubes. We then note the observation for each test tube. Name of the unknown
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ppt and centrifuged again. 3) I added 2mL of H2O‚ put the test tube in the hot water bath and stirred for 3 minute with a stirring rod. 4) I then decanted the solution into another test tube. 5) I added one drop of 6M acetic acid and 3 drops of 1M K2CrO4‚ which formed a positive confirmation where yellow ppt was formed‚therefore it contained Pb+2 Identifying Hg2+2: 1) I took the white ppt formed formed from the first test and added 10 drops of 6M NH3. 2) I stirred the contents and then centrifuged
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