Conclusion: (Identity‚ % error‚ other evidence‚ how to improve) The identity of Unknown A is the compound cobalt(II) chloride hexahydrate (CoCl₂•6H₂O).This is justified by the similarities in color of red-purple crystal like grains‚ which is significant in identifying the product out of the eight suggested identities. Only two had similar characteristics which were CoCl₂•6H₂O and CoSO₄•6H₂O. Before unknown A was heated‚ there was a notable common physical property of the substance being red crystal
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having the copper (II) oxide solid used was washed with 6.00M H2SO4 thus having a reaction of: CuO(s) + H2SO4(aq) CuSO4(aq) + H2O(l) It was noted that from the colorless or clear filtrate‚ it changed into blue. Also‚ there was a formation of blue precipitate when 6.00M H2SO4 was added. The CuSO4 solution obtained was then added with zinc dust having a chemical equation as follows: CuSO4(aq) + Zn(s) ZnSO4(aq) + Cu(s) During the addition of more zinc dust‚ it was observed that there were bubbles
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2010 Objective: To determine the properties of colloids and how they function in physiological systems Materials: O.1 M CuSO4 * 10% skim milk mixture 3 M HAc 0.2 M K2Cr2O7 0.04 M AgNO3 0.02 M K2Cr2O7 * 1% Gelatin 0.01 M AgNO3 5 Test tubes Dialysis bag Observations: Part I. |Test Tube Number |CuSO4 Solution |Skim Milk |3 M HAc | |1 |4 mL
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Title: 03.09 Molar Mass of Compounds: Determining the Formula of a Hydrate Purpose: To determine the formula of a hydrate. Materials: * crucible * Bunsen burner * balance * CuSO4 hydrate Procedure: 1. Measure the mass of the clean‚ empty crucible‚ record the mass. 2. Add one or two scoops of the hydrate to the crucible‚ record the mass. 3. Heat the crucible and hydrate above a Bunsen burner for at least ten minutes to make sure that all of the water evaporates
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Procedure: 1. In the first table‚ write down a description of what KSCN and Fe(NO3)3 look like. 2. Clearly mark the 4 beakers‚ 1 thru 4‚ to ensure you know what substance is added to each beaker. 3. Observe a solution of potassium nitrate KNO3. Describe the appearance of the solution in the first table. 4. Put approximately 25 ml of 0.0020M potassium thiocyanate solution‚ KSCN‚ in
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Glucose (C6H12O6) | No | Nothing changes | Nothing changes | Dilute Sulfuric Acid (H2So4) | Yes | Bubbles | Bigger bubbles | Sucrose (C12H22O11) | Yes | Light bubbles | Light but more visible bubbles and light brown liquid | Copper Sulfate (CuSo4) | Yes | Light bubbles | Changes color to brown and oxidation is observed | Ethanol (c2H5OH) | No | Nothing changes | Nothing changes | Calcium Hydroxide (Ca(OH)2) | Yes | Light bubbles | Light bubbles but more than in anode | Potassium Bromide
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scientists inadvertently produce undesired products that must be filtered or decanted out of solution (Petrucci et al‚ 2007). Beginning with pure copper wire‚ this experiment will exhibit its transformation to substances including Cu(NO3)2‚ Cu(OH)2‚ CuO‚ CuSO4 . 5H2O and finally returning to pure copper (Cu). The experiment objective is to successfully complete these conversions and then calculate the percentage of recovered copper using the initial and final mass data obtained. Procedure Please refer
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of moles of the reactants Dependent Variable: The limiting reagent Constant Variable: The volume of reactants added Equipment: 2 100 ml beaker 2 measuring cylinders 10 ml of 0.1 molL-1 HCL(aq)‚ NAOH(aq) 20 ml of 0.1 molL-1H2SO4(aq)‚ CuSO4(aq) 30 ml of 0.1 molL-1 Ba(NO3)2(aq) Universal indicator Filter Paper Funnel 4 test tubes Reaction A- Method: 1) Measure 10 ml of 0.1 molL-1 of Hydrochloric Acid using a measuring cylinder. 2) Measure 10 ml of 0.1 molL-1
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o.oo5 moles of it was used. The heat generated by the reaction is 55.8 kJ. The sign of T of the reaction used for calibration is opposite to that of H. In the determination of heats of reaction‚ the reaction of 15 mL 1 M CuSO4 + 0.05 g Zn produced a net ionic equation of CuSO4 + Zn ZnSO4 + Cu. The limiting reactant of the reaction is Zn and 0.05 moles of it was used. The sign of T of the reaction used for calibration is opposite to that of H. WORKING EQUATIONS: H+(aq) + OH-(aq) H2O(l)
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with plenty of water and clean your equipment. 6. Add your results to the class data and record the class data in the chart. 7. Copy the following chart into the data and observations section of your lab report. IV. Data g of KNO3 in 100 grams of water Temperature (Celsius) V. Post lab questions Postlab Questions 1. Describe the graph. How does solubility change with temperature? As Temperature increases the solubility increases. 2. What
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