Ba(NO3)2 Milky ppt Milky ppt NR NR Yellow ppt Na2SO4 NR NR NR Peach ppt Al2(SO4)3 NR NR Orange ppt KOH NR Carrot Orange ppt MgCl2 Lemon yellow ppt FeCl3 Set #2 KCl MgCl2 Na2SO4 NaOH BaCl2 MgSO4 KCl NR NR NR NR NR MgCl2 NR NR Cloudy ppt NR Na2SO4 NR Cloudy ppt NR NaOH NR NR BaCl2 Cloudy ppt MgSO4 Questions: 1. On the attached sheet 2. A precipitate forms when
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Water bath One looped platinum or nichrome wire Label REAGENTS 0.5 M CaCl2 0.5 M BaCl2 M NaOH 0.1 M AgNO3 0.5 M KCl 0.5 M KBr 0.5 M KI 2 M NH4OH M KCN % H2O2 2 M H2SO4 MnO2 Saturated FeSO4 0.1 M NaNO3 CH3COOH 0.5 M Na2SO3 0.1 M KSCN 2 N KOH 0.5 M K4[Fe(CN)6] 0.5 M FeSO4 0.5 M FeCl3 0.5 M Al2(SO4)3 2 N HCl 0.5 M LiCl 0.5 M NaCl 0.5 M KCl 0.5 M K2Cr2O7 96% H2SO4 III. EXPERIMENTAL PROCEDURE 1. Reactions of Cu2+ 10 drops of 2 M NaOH‚ 2 M NH4OH‚ 0.5 M K4[Fe(CN)6]
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the computer. *PURPOSE: To learn which type of salt lowers the Freezing Point of water the greatest amount. *PROBLEM: Which type of salt lowers the Freezing Point of water to the lowest point? Blank 2 *HYPOTHESIS: The KCl will lower the water’s Freezing Point the most‚ because Potassium has the lowest ionization energy out of the five metals that are bonded with Chlorine‚ and perhaps it will bond more easily with the water molecules‚ keeping it from freezing. *MATERIALS:
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way does the temperature go up or down. Verses if the water is hot with salt. (15 points) 4. Use the data from Part 1 of the procedure to complete the data tables and graphs. Answer: Station 1: Potassium Chloride (KCl) Beaker Temperature of water (°C) Amount of KCl at saturation (g) A 5.0 25 B 30.0 12 C 54.8 20 D 70.1 32 Station 2: Potassium Chlorate (KClO3)– Beaker Temperature of water (°C) Amount of KClO3 at saturation (g) A 5.2 20 B 28.7 10 C 43.9 15 D 68.2 28 (3 points) 5
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Chemistry 1211 Prof. Dan Schwartz Exam #2 Thursday‚ 3/13/2003 7:00 – 8:30 P.M. There is a single correct choice for each question. Answer all questions on the Scantron sheet by filling in the proper bubble with a #2 pencil. If you change an answer‚ erase the undesired mark thoroughly. Be sure to fill in the boxes for your student number‚ name and lab section; then correctly fill in the corresponding bubbles beneath them. A periodic table and other useful information are attached to the back
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of carbon dioxide will be produced? 3) Given the equation: HCl + Na2SO4 ( NaCl + H2SO4 If you start with 20 grams of hydrochloric acid‚ how many grams of sulfuric acid will be produced? 4) Given the following equation: LiOH + KCl ( LiCl + KOH a. I began this reaction with 20 grams of lithium hydroxide. What is my theoretical yield of lithium chloride? b. I actually produced 6 grams of lithium chloride. What is my percent yield? 5) Given the following
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The experiment’s objectives were to synthesize alum‚ test for various ions in alum‚ and form crystals in aqueous alum solution. The alum was synthesized from aluminum foil and run through a filtration system to isolate the alum. 2 Al(s) + 2 KOH + 22 H2O + 4 H2SO4 → 2 KAl(SO4)2●12H2O(s) + 3 H2(g) Its composition was analyzed using two precipitation tests and two flame tests. Three methods for growing crystals were then set up for observation next lab. Theoretical yield and percent yield: The theoretical
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experiential learning model (which simply means learning through experience)‚ Gibbs’ model is sometimes referred to as an iterative model (which simply means learning through repetition). 1 Peter Lia: Learning Support Tutor: Disability Advisory Service: KCL The version of Gibbs’ model given to students may be slightly adapted‚ such as the one that appears in Bulman and Schultz (2013) Reflective Practice in Nursing p232. It looks like this: Description what happened? Final evaluation What were your
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5.) a.) b.) Ethyne (C₂H₂) has the shortest C-to-C bond because there is a triple bond between the two C’s. The shorter the bond‚ the smaller the distance between the two bonded atoms‚ a single bond has the largest distance between two bonded atoms. c.) i.) trigonal planar ii.) pyramidal d.) This is not true because the bonds described are intramolecular forces‚ C-H‚ C-O‚ O-H‚ which are not affected by boiling. When boiling occurs‚ added energy overpowers intermolecular forces‚ not
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fine powder and heated to drive off any atmospheric moisture‚ the resulting powder is an excellent catalyst for chemical reactions. Balancing Chemical Equations Balance the equations below: 1) ____ N2 + ____ H2 ____ NH3 2) ____ KClO3 ____ KCl + ____ O2 3) ____ NaCl + ____ F2 ____ NaF + ____ Cl2 4) ____ H2 + ____ O2 ____ H2O 5) ____ Pb(OH)2 + ____ HCl ____ H2O + ____ PbCl2 6) ____ AlBr3 + ____ K2SO4 ____ KBr + ____ Al2(SO4)3 7) ____ CH4 + ____ O2 ____ CO2 + ____ H2O 8) ____
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