Abstract: The purpose of this lab was to use potentiometry to measure the concentration of a specific chemical species in a solution. This was conducted in 2 stages. The first stage involved making a solution of potassium iodide. The potassium iodide was then diluted to several different concentrations that were ran in potentiometer to find the mV of each solution which would then be used to find the PH of the solution. After analyzing a sample of each concentration an unknown solution was compared
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Reactivity of Halide Ions Michelle Faktor and Kelly Freas Date of Experiment: October 28‚ 2012 Period 2 Honors Chem Purpose: The purpose of this lab is to observe the reactions of halide ions with different reagents by mixing them together. Analyze data to determine characteristic reactions of each halide ion. Infer the identity of unknown solutions. Materials: * 0.1 M AgNo3 * 0.1 M NaCl * 0.1 M NaF * 0.2 M KBr * 0.2M Kl * 0.2 M Na2S2)3 * 0.5 M Ca(NO3)2
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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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Synthesis and Decomposition of Zinc Iodide Partners: Sonya Pasia and Kristen Kobayashi CH 085-01 20 September 2011 Zinc Iodide (ZnI2) was an interesting binary compound to experiment with. In this experiment‚ weakly acidified water (25mL distilled water with 18 drops 5M acetic acid solution) was used as an aid to bring molecules of the zinc and iodide atoms together‚ by dissolving iodine molecules‚ so that bonding would transpire to produce a reaction. Deprived of water‚ the Zn and I2
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exchange of positive and negative ions between reacting solutions of two ionic compounds. Thus‚ in this example the precipitate must be either silver chloride‚ AgCl or sodium nitrate‚ NaNO3. Sodium nitrate dissolves readily in water and is therefore soluble. Thus we can conclude that silver chloride is the insoluble precipitate. We can represent the formation of this precipitate by a net ionic equation: Ag+ +NO3 ̄ +Na++Cl ̄→AgCl+NO3 ̄+Na+ Net: Ag+ (aq)+Cl ̄ (aq)→AgCl(s) Ions present in the solution but
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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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The lab today was focused on finding the ratio of reactants to products to be either 1 to 1 or 1 to 2. In our case the reactants was Lead (II) Nitrate and Potassium Iodine. These two when mixed together make Lead Iodide and Potassium Nitrate. We also had to try and find if the number of moles of Lead(II) Nitrate was the same as the final number of moles for Lead Iodine after the experiment. Our data for the lab had pinpoint accuracy. Proved by the data table below Trials Volume of Pb(NO3)2 Mol
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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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