"Bacl2 k2cro4" Essays and Research Papers

Involving Chromate and Dichromate Ions Steps 2 and 3 0.1 M K2CrO4 0.1 M K2Cr2O7 Initial Color 1 M NaOH added 1 M HCl added Step 4 0.1 M K2CrO4 0.1 M K2Cr2O7 Initial Color 1 M HCl added 1 M NaOH added Steps 5 and 6 INITIAL COLOR + 1 M NaOH + 0.1 M Ba(NO3)2 + 1 M HCl 0.1 M K2CrO4 Steps 7 and 8 INITIAL COLOR + 1 M HCl + 0.1 M Ba(NO3)2 + 1 M NaOH 0.1 M K2Cr2O7 Step 9 0.1 M K2CrO4 0.1 M K2Cr2O7 Add 0.1 M Ba(NO3)2 Table 5 Equilibrium

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Name ___________________________________________ Date ___________________________________ Block ____ Experiment 12A Investigating chemical equilibrium ABSTRACT 1. What is equilibrium and how can you tell it has been reached? __________________________________________________________________________________________ __________________________________________________________________________________________ __________________________________________________________________________________________

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1. | An experiment is carried out to determine the freezing point of naphthalene.Solid naphthalene is heated in a water bath until it melts completely. The initial temperature is recorded. Then molten naphthalene is left to cool. The reading of the temperature is recorded every 30 seconds. Figure below shows the recorded thermometer readings at 30 seconds intervals. Satu eksperimen dijalankan untuk menentukan takat beku naftalena. Pepejal naftalena dipanaskan di dalam kukus air sehingga melebur

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Investigating Chemical Equilibrium Date: 30th April 2013 Due Date: 15th May 2013 Prepared For: M. Seraji Prepared by: Andrea Odunze Abstract Many reactions proceed to a state of equilibrium. A chemical reaction at equilibrium‚ where the rates of the forward reaction and reverse reaction are equal‚ looks like this: A + B AB There are three factors‚ according to Le Chatelier’s principle‚ that affect the equilibrium position and equilibrium constant. These are the concentrations of products

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Barium Nitrate solution. (BaCl2 + 2AgNO3 -> Ba(NO3)2 + 2AgCl) Research Question: How will the amount of Barium Chloride and Silver Nitrate affect how much Silver Chloride is produced? Hypothesis: If there is one mole of BaCl2 in the reaction‚ then two moles of AgCl will be produced. Variables: Independent: Amount of the compound‚ BaCl2‚ in grams. Dependent: Amount product produced‚ AgCl‚ in grams. Materials: * 4 -grams of Barium Chloride (BaCl2) * 8 -grams of Silver

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sparker 2 -250mL beakers 10mL grad cylinder 0.2M FeCl3 0.2M KSCN 0.2M KCl 0.2M Fe(NO3)3 6.0M NaOH CoCl26H2O 6.0M HCl water 0.1M K2CrO4 0.1M K2Cr2O7 1M NaOH 1M HCl 0.1M Ba(NO3)2 Procedure PART I 1. Use a 10mL graduated cylinder to measure 1mL of 0.2M FeCl3 and pour it into a 250mL beaker. Using another 10mL graduated cylinder‚ measure

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GRAVIMETRIC DETERMINATION OF SULFATE Purpose You will be given a solid powder‚ which has been dried to constant mass. The sample is water soluble. The purpose of this experiment is to determine the concentration of sulfate in your solid sample using gravimetric analysis. Background Gravimetric Analysis The goal of most quantitative chemical analysis measurements is to estimate the relative abundance of an analyte in a chemical sample. For solid and liquid samples‚ a very common expression

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using stoichiometry. II. Materials: * 0.00500 moles of potassium chromate * 0.00500 moles of lead (II) nitrate III. Procedures/ Observations: IV. Observation & Data Balanced Equation: K2CrO4 + Pb(NO3)2 2KNO3 + PbCrO4 Mass of lead (II) nitrate used: 0.00500 mol Pb(NO3)2 × 331.2 g PbNO 1 mol Pb(NO ) = 1.7 g Pb(NO3)2 Mass of potassium chromate used: 0.00500 mol

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Chemistry 12 - Lab 19A Flow Chart (Investigating Chemical Equilibrium) PART 1: Put on safety goggles and lab apron Obtain 2 (Empty‚ Clean‚ AND DRY) 250mL Erlenmeyer flasks. Add approx. 100mL of DISTILLED water and 1mL of thymol blue solution to each flask Record the colour of this solution in note book FIRST FLASK: add a single drop of 0.1M HCl. Swirl the contents of the flask and continue drop-by-drop addition until a definite colour change is observed. SECOND FLASK: will serve as

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(aq) 2AgCl (s) d. Balanced equation: BaCl2 (aq) + FeSO4 BaSO4 (s) + FeCl2 (aq) Ionic equation: Ba2+ (aq) + Cl- (aq) + Fe2+ (aq) + 2SO4- (aq) 2BaSO4 (s) + Fe2+ (aq) + Cl- (aq) Net ionic equation: Ba2+ (aq) + 2SO4- (aq) 2BaSO4 (s) | | Reference solutions | | | KCl | Na2SO4 | NaOH | Na2CO3 | Test solutions | SrCl2 | No reaction | Reaction | Reaction | Reaction | | AgNO3 | Reaction | Reaction | Reaction | Reaction | | BaCl2 | No reaction | Reaction | Reaction | Reaction

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