II. Materials A. Reagents 0.1 M potassium ferricyanide‚ K3Fe(CN)6 ferrous sulphate‚ FeSO4 sodium hydroxide‚ NaOH sodium chloride‚ NaCl hydrochloric acid‚ HCl potassium hydroxide‚ KOH potassium nitrate‚ KNO3 nitric acid‚ HNO3 trisodium phosphate‚ Na3PO4 sodium thiocyanate‚ NaSCN sulfuric acid‚ H2SO4 distilled water‚ dH2O B. Apparatus test tubes iron ring 250-mL beaker iron stand bunsen burner C. Others iron nails copper strip sand paper zinc strip pliers 2 III. Procedure A. Reactions
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4.1 & 4.2: General properties of aqueous solutions and Precipitation Reactions: 1. (Brown 4.11) When asked what causes electrolyte solutions to conduct electricity‚ a student responds that it is due to the movement of electrons through the solution. Is the student correct? If not‚ what is the correct response? 2. (Brown 4.15) Specify what ions are present in solution upon dissolving each of the following in water: a. ZnCl2 c. (NH4)2SO4 b. HNO3 d. Ca(OH)2 3. (Brown 4.16 ) Specify
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EXPERIMENT 4 TITLE Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction‚ or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft & Constable‚ 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution‚ it considered as precipitate. Commonly‚ the solid will fall out of the
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are there in 4‚595‚000‚000‚000‚000‚000 molecules of SF6? 58. 59. 3. Calculate the number of moles in 5.45x1025 atoms of Zn 1. What is the mass of 7.50 moles of sulfur dioxide (SO2)? 2. How many moles are there in 250.0 grams of sodium phosphate (Na3PO4)? 3. How many grams of potassium sulfate (K2SO4) are there in 25.3 moles? 4. Calculate the number of grams in 3.25-mol of AgNO3 60. 5. What is the volume of 0.38 moles of any gas at STP? 61. 6. Calculate the number of moles in 32.2-L of NH3 7
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tetranitride (d) SF2 sulfur difluoride (e) H2S dihydrogen monosulfide (f) P4O10 tetraphosphorus decaoxide 27. Name each of the following compounds. (a) Ca(NO3)2 calcium nitrate (b) KOH potassium hydroxide (c) MgCO3 magnesium carbonate (d) Na3PO4 sodium phosphate (e) LiNO3 lithium nitrate (f) Mg(C2H3O2)2 magnesium acetate 28. Write formulas for each of the following compounds. (a) iron(II) oxide FeO (b) tin(II) sulfide SnS (c) copper(I) chloride CuCl (d) mercury(II) iodide HgI2 (e)
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LAB REPORT 5 – ACID/BASE CHEMISTRY No credit will be given for this lab report if the Data section is not completely filled out and if the required photographs are not received. At least one photograph must show the student’s face. NOTE: This experiment is rather lengthy. Plan accordingly. OBJECTIVES 1. Define strong electrolyte‚ weak electrolyte‚ nonelectrolyte‚ acid‚ base‚ salt‚ strong acid‚ weak acid‚ strong base‚ weak base‚ and neutralization reaction. 2. Compare and contrast the chemical
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Experiment 5 Determination of Empirical Formulas of Hydrate and Oxide Compounds Room #216 Locker# 1137 Date of Experiment: May 11‚ 2014 Date of Submission: May 16‚ 2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass
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Ionic Reactions Results B - Do your results agree with your expectations from the solubility rules/table? Our results seemed to largely agree with the established solubility rules/table; however‚ a few reactions with the commonality of being mixed with Co(NO3)2 (cobalt nitrate) [reference Row A‚ Columns 2‚ 3‚ and 4] seemed to have such a pale pink tone that it was difficult to decide whether that could have been a precipitate or the lighting in the area where the experiment took place. Ultimately
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Data Table: Record your observations in the following table Na3PO4 NaI Na2SO4 NaCl NaHCO3 Na2CO3 NaOH Co(NO3)2 Precipitated a blue color NR NR NR Turned a milky purple color Precipitated a light purple color Precipitated a light blue color Cu(NO3)2 Precipitated a light blue color Precipitated a dark amber color NR NR Precipitated a light blue color Precipitated a light green color Precipitated a light blue color Fe(NO3)3 Precipitated a light milky yellow color Turned a dark black
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Questions: B. Yes C. Carbonates‚ Phosphates‚ sulfides‚ oxides or hydroxides form precipitates. Alkali metal hydroxides are the exceptions. D. Most salts. E. Group one and two cations F. A1. Cobalt nitrate with Sodium phosphate. CO(NO3)2+6 H2O+Na3PO4+12 H2O Na3+PO2Co(NO3)2+18 H2OD5. Ba(N03)2 - NaHC03 A7. Cobalt nitrate with sodium hydroxide Co(N03)2 - 6 H20 – NaOH B6. Copper nitrate with sodium carbonate Cu(N03)2 - 3 H20 - Na2C03 C1. Iron nitrate with sodium phosphate Fe(N03)3 - 9
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