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PCC CH 100 - Aqueous Chemical Reactions

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Negative Ions +Ch100: Fundamentals for Chemistry 1Instructor: Tony ZableExperiment: Aqueous Chemical ReactionsObjectives:- To write out the chemical formulas for a number of ionic compounds- Observe a large number of chemical reactions by mixing solutions of ionic compounds- To predict the precipitate product in these reactions using Solubility Rules- For each chemical reaction observed, determine:1. the molecular equation2. the complete ionic equation3. the net ionic equationPart 1. Naming Ionic Compounds in SolutionObtain a tray of 14 microburets from the instructor. Each microburet is labeled and contains a different solution. Let’s see how many chemical names you know. Complete the table below, matching the formula on the label on the microburet to the name in the table.Name Chemical Formula of SoluteConcentrationSulfuric acid 1 MSodium hydroxide 1MSodium phosphate 0.2 MSodium carbonate 0.2 MSilver nitrate 0.1 MPotassium iodide 0.2 MNitric acid 1 MLead (II) nitrate 0.2 MHydrochloric acid 1 MIron (III) chloride 0.1 MCopper (II) sulfate 0.2 MBarium chloride 0.1 MAmmonium hydroxide 1 MAluminum chloride 0.3 MCh100: Fundamentals for Chemistry 2Instructor: Tony ZablePart 2. Identifying Solids Formed in Reactions in Aqueous SolutionsProcedure:1. Place the plastic covered grid (with inserted grid matrix) in front of you. This grid will serve as your reaction surface during the activities in this worksheet.2. Obtain the microburet containing 0.2 M copper(II) sulfate and carefully place a drop of solution in the grid location along the row labeled CuSO4 and the column corresponding to NH4OH.3. Place a drop of 1M NH4OH into the same grid square containing CuSO4.4. Using the plastic stirrer provided, gently mix the two solutions. (i) Describe what occurred when the two solutions were mixed together?(ii) Write down the molecular equation for the chemical reactants and predict the products.(iii) Using the solubility rules from Chapter 7, predict which of the products might be expected to precipitate in water.(iv) Write down the complete ionic equation for the chemical reactants and predict the products.(v) Using this information, write down the predicted net ionic equation for this reaction.Ch100: Fundamentals for Chemistry 3Instructor: Tony Zable5. Now let’s try another reaction. Place a drop of CuSO4 solution in the grid location along the CuSO4 row and the column corresponding to BaCl2. Then add a drop of BaCl2 into this square. Gently mix the two solutions together using the plastic stirrer.(i) Describe what occurred when the two solutions were mixed together?(ii) Write down the molecular equation for the chemical reactants and predict the products.(iii) Using the solubility rules from Chapter 7, predict which of the products might be expected to precipitate in water.(iv) Write down the complete ionic equation for the chemical reactants and predict the products.(v) Using this information, write down the predicted net ionic equation for this reaction.6. Select two different reactants and observe a new reaction. Reactants:(i) Describe what occurred when the two solutions were mixed together?(ii) Write down the molecular equation for the chemical reactants and predict the products.(iii) Using the solubility rules from Chapter 7, predict which of the products might be expected to precipitate in water.(iv) Write down the complete ionic equation for the chemical reactants and predict the products.(v) Using this information, write down the predicted net ionic equation for this reaction.Ch100: Fundamentals for Chemistry 4Instructor: Tony Zable7. Select two different reactants and observe a new reaction. Reactants:(i) Describe what occurred when the two solutions were mixed together?(ii) Write down the molecular equation for the chemical reactants and predict the products.(iii) Using the solubility rules from Chapter 7, predict which of the products might be expected to precipitate in water.(iv) Write down the complete ionic equation for the chemical reactants and predict the products.(v) Using this information, write down the predicted net ionic equation for this reaction.8. Select two different reactants and observe a new reaction. Reactants:(i) Describe what occurred when the two solutions were mixed together?(ii) Write down the molecular equation for the chemical reactants and predict the products.(iii) Using the solubility rules from Chapter 7, predict which of the products might be expected to precipitate in water.(iv) Write down the complete ionic equation for the chemical reactants and predict the products.(v) Using this information, write down the predicted net ionic equation for this reaction.Ch100: Fundamentals for Chemistry 5Instructor: Tony ZableSolubility of Ionic Compounds in WaterNegative Ions + (anions) Positive Ions form (cations)Compoundswhich are:All Group 1 ions (Li+, Na+, K+, Rb+, etc.) SolubleAll Ammonium ion, NH4+SolubleNitrate, NO3-All SolubleAcetate, C2H3O2-All SolubleChloride, Cl-Bromide, Br-Iodide, I-Ag+, Pb2+, Hg22+, Cu+All OthersNot SolubleSolubleSulfate, SO42-Ca2+, Ba2+, Sr2+, Pb2+All OthersNot SolubleSolubleSulfide, S2-Group 1 ions, NH4+,Group 2 ions (Be2+, Mg2+, etc.)All OthersSolubleSolubleInsolubleHydroxide, OH-Group 1 ions, NH4+, Ba2+, Sr2+All othersSolubleNot SolublePhosphate, PO43-Carbonate, CO32-Sulfite, SO32-Group 1 ions, NH4+All othersSolubleNot SolubleNote: Soluble means more than 0.1 mole will dissolve per


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