Chemical Reaction Report

Topics: Test tube, The Tubes, Chemical reaction Pages: 8 (3018 words) Published: November 5, 2014
II. LEARNING OBJECTIVES - To perform different types of chemical reactions including acid-base, precipitation, gas forming, complex compound forming and oxidation-reduction reactions. - To identify some of the products in these reactions and describe the chemical changes. - To write and balance the chemical equations for the reactions observed. III. EQUIPMENT AND REAGENTS 1. EQUIPMENTThirty test tubes One test tube rack Two test tube holders Two spatulas Three 250 mL beakers One stirring rodOne medicine dropper IV. EXPERIMENTAL PROCEDURE 1. REACTIONS OF Cu2 - Prepare 3 test tubes, 10 drops of 0.5 M CuSO4 are added into each one-10 drops of the following reagents are added into the tubes 2 M NaOH 2 M NH4OH 0.5 M K4Fe(CN)6. - Record your observations. 2. REACTIONS OF SILVER HALIDES - Prepare 3 test tubes, 10 drops of 0.5 M KCl, 0.5 M KBr, and 0.5 M KI are added into each one- Add 10 drops of 0.1 M AgNO3 to each salt solution. Record your observations. - Each test tubes are divided into 2 test tubes and labeled 1-3 A and 1-3 B - Test tubes 1-3 A 5 drops of 2 M NH4OH are added to each of test tubes. Observe the change. - Test tubes 1-3 B 5 drops of 2 M KCN are added to each of test tubes. Record your observations. 3. REACTIONS OF H2O2 - 5 drops of 0.1 M KMnO4 solution are added into a test tube. 5 drops of 2 M H2SO4 are added to acidify the solution and then add 5 drops 0f 3 H2O2 solution. Observe the color change and the release of gas. - 5 drops of 0.1 M KI solution are added into a test tube. 5 drops of 2 M H2SO4 are added to acidify the solution and then add 5 drops 0f 3 H2O2 solution KI - Have a pinch of solid MnO2 added into 1 mL of 3 H2O2 solution. Observe the released gas. 4. REACTIONS OF NITRATE BROWN RING TEST - Add 1 mL of 1 M NaNO3 to the test tube and then 1 mL of saturated FeSO4- Pour concentrated sulfuric acid (96) carefully into the test tube. After waiting for a few seconds,observe the change of color at the interface between the solution and the acid. Note The nitric acid is reduced to nitrogen monoxide by the iron (II) ion and the brownish violet nitroso complex compound is then found by nitrogen monoxide with the excess iron (II) ions -Redo the reaction with NaNO2 instead of FeSO4,-Redo the reaction with acetic acid instead of H2SO4. Record your observations and compare with the system. 5. REACTIONS OF KMnO4 -Label 3 test tubes from 1 to 3- Tube 1 10 drops of 0.5 M Na2SO3 and 5 drops of 2 M H2SO4. - Tube 2 10 drops of 0.5 M Na2SO3 and 5 drops of 6N NaOH. - Tube 3 10 drops of 0.5 M Na2SO3 and 5 drops distilled water. - 5 drops of 0.1 M KMnO4are then added to each of test tubes. Record your observations. 6. REACTION OF POTASSIUM DICHROMATE - 10 drops of 0.5 M K2Cr2O7are placed into a test tube and then add 10 drops of 6 M H2SO4. - 5 drops of C2H5OH are added in the tube. Record your observations. 7. REACTIONS OF Fe3 and Fe2 - 1 mL of 0.5 M FeCl3 solution is placed in seven test tubes. - 5 drops of the following seven reagents 0.5 M KCN 0.1 M KSCN 2 N KOH 0.5 M K4Fe(CN)6 2M NH4OH are added into each tubes. Record your observations - Repeat using FeSO4 instead of FeCl3. 8. REACTIONS OF Al3 - 10 drops of 0.5 M Al2(SO4)3and 5 drops of 2 N NaOH are added into a test tube. - Divide the solution into another test tube and label 1-2 Test tube 1 add 10 drops of 2 M HCl. Test tube 2 add 10 drops of 2 N NaOH. - Record what you observe. 9. FLAME TEST - 1ml LiCl, NaCl, KCl, Cacl2, BaCl2 are added into 5 tubes.- Light the Bunsen burner (Alcohol lamp)- Dip a looped wire into one of the solutions, and then burn it in the flame - Record the flames color. - Using the wavelengths shown in the manual, calculate the frequency and energy of the photons of the flames. V. DATA AND OBSERVATIONS1. Reactions of Cu2 ReactionObservation NaOHLight blue liquid CuSO4at first. Dark blue precipitate is formed, liquid is more blue NH4OHLight blue liquid CuSO4 at first. Dark blue precipitate...
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