The purpose of this lab was to see which solutions are soluble and which are not. We were able to see this by mixing certain solutions together and observing changes that occurred. The procedure for this experiment included a few different steps. The first steps were to add the nitrate solutions into the lettered parts of the 96-well plate. Once you were done with that‚ you were supposed to add the sodium solutions to the numbered parts of the 96-well plate‚ so that the solutions were added together
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AP Chemistry Final Exam Review ESSAY. Write your answer in the space provided or on a separate sheet of paper. 1) Explain the difference between a qualitative and a quantitative measurement. Provide examples to illustrate this difference. Answer: A qualitative measurement is a measurement that gives descriptive‚ nonnumeric results; a quantitative measurement is a measurement that gives definite‚ usually numeric results. "The rock is heavy" would be a qualitative measurement. "The rock weighs 110
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10. Strong Bases: NaOH‚ KOH‚ Na2CO3‚ NaHCO3‚ Na3PO4‚ NaHPO4‚ Strong Acids: Fe(NO3)3‚ HCL‚ HNO3‚ Al(NO3)3‚ NiCl2‚ H2SO4 11. Acidic Neutral Basic NaCl KNO3 NaOH HC2H3O2 Na2CO3 NaC2H3O2 NaHCO3 Fe(NO3)3 NaNO3 Na3PO4 HCl MgSO4 KOH HNO3 Na2SO4 NaHPO4 CuSO4 NaNO2 CoCl2 Al(NO3)3 NiCl2 H2SO4 KCl NH4Cl 12. CuSO4 CuCO3.Cu(OH)2(s) + 2 H2SO4(aq) ----> 2 CuSO4(aq) + CO2(g) + 3 H2O(l) Na3PO4 Na3PO4 (aq) + 3H2O (l) --> H3PO4 (aq) + 3NaOH (aq) 13
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the copper Observations 1) The theoretical yield comes to 0.7435g of copper 3CuCl2-2H2O + 2Al -> 3Cu + 2AlCl3 + 6H2O Mass of CuCl2-2H2O | Mass of Clean Beaker | Mass of Copper created | Mole-to-Mole ratio | 2g | 113.5g | 0.8g | 1 : 1 (hydrate to copper) | 2g of CuCl2-2H2O CuCl2-2H2O = 170.55 g/mol 2 / 170.55 = 0.0117mol 1 : 1 0.0117 x 0.0117 moles of Cu Cu = 63.55g/mol
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Name: Allison Bynum Date:6/17/14 Exp 8: Ionic Reactions Lab Section: 75426 Data Table: Record your observations in the following table Na3PO4 NaI Na2SO4 NaCl NaHCO3 Na2CO3 NaOH Co(NO3)2 Created a musty looking cloud that later turned dye to a purple shade No change‚ brought out pink very slightly No change No change Created a cream looking liquid‚ did not mix with pink substance Darkened color‚ changing to more of a purple tint as time passes on. Immediately turned
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Yield of CuCl2.2DMSO Formula weight (Mr) of CuCl2 = 63.55 + (35.45 x 2) =134.45g/mol Formula weight of product CuCl2.2DMSO = 134.45 + 2[16 + 32.06 + (12.01 x 2) + (1.0079 x 6)] = 290.704g/mol Mass of CuCl2= 0.850g Equation for reaction CuCl2 + 2DMSO -> CuCl22DMSO Mole ratio between CuCl2 and CuCl22DMSO = 1:1 Mole of CuCl2 = Mass/ Mr = 0.850/134.45 = 0.00632 moles Since the ratio between CuCl2 and CuCl22DMSO = 1:1‚ mole of CuCl2DMSO is also 0.0063 moles. To find theoretical yield of CuCl2
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Step B: Determine the mass of a clean and dry 250 mL beaker. * Step C: Obtain a sample of CuCl2(s) (about 8 grams) from your instructor and add it to the beaker. Determine the accurate total mass of the beaker and the CuCl2(s). Caution – Copper (II) chloride is poisonous. Clean up any spills immediately. Get help from your instructor. Wash your hands after using it. * Step D: Dissolve the CuCl2(s) in about 50 mL of distilled water. * Step E: 1) Use the sand paper to clean the
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C: CuSO4 D) CuCl2 E) KCl Description how to identify solution: _ We have two blue solution which are CuSO4 and CuCl2 or C and D‚ according to chemical reaction experiment‚ C didn’t have any reaction with other solution like B and D beside A‚ so if we look at the solubility chart‚ SO2- have only one precipitation with Ba2-. So we come to conclusion that C is CuSO4 and A is Ba(NO3)2 _ So now that we know C is CuSO4‚ other blue solution must be CuCl2 which is D‚ so according
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Korleyfah Mouth Chem 331 Thursday 2:00pm Dr. Lijuan Li 20A Preparation of CuCl2~2DMSO 20B Preparation of RuCl2~4DMSO Abstract In order to synthesize our metal complexes‚ we were able to make both Copper and Ruthenium metals. From this‚ we combined each metal complex with DMSO by refluxing the compound. The metal complexes were analyzed through their melting point and IR spectroscopy to determine whether the metal bonded to a Sulfur atom or an Oxygen atom of the DMSO. After analyzing the IR spectrum
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2nd heat 30.657g Heating mass difference .004g Mass of anhydrate .394g Mass of H2O .108g Molar mass of CuCl2 135.0g/mol Molar mass of H2O 18.0g/mol Moles of anhydrous sample 2.92x10-3 moles CuCl2 Moles of H2O released 6.00x10-3 moles of H2O Mass % of H2O 21.5% of H2O % Absolute error 0% absolute error Mass of rehydrated sample .469g % of hydrate recovered 93.4% CuCl2 H2O The samples were placed in a desiccator instead of being left to cool on the lab bench between each heating
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