Determination of Phosphorus Content of Fertilizer: Skill Building Lab © 2011‚ Sharmaine S. Cady East Stroudsburg University Gravimetric Analysis Skills to build: Using vacuum filtration Using a digital balance Using mass stoichiometry Doing a gravimetric analysis Fertilizer Scientists estimate that the earth ’s soil contains less than twenty percent of the necessary organic nutrients needed to meet our current food production. Carbon‚ hydrogen‚ and oxygen used to synthesize
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following cases? a) S2b) H2SO4 c) S2O32d) CS2 e) S8 7. To prepare 100 g of 19.7% by weight solution of NaOH‚ how many grams each of NaOH and H2O are needed? 8. Balance the following equations: a) Fe2(SO4)3 + BaCl2 b) Ba(OH)2 + HCl c) BaSO4 + CuCl2 d) Zn + H2SO4 9. Balance the following skeleton reactions and identify the oxidizing and reducing agents (ion-electron method). MnO4 (aq) + H2O2(aq) Mn2+(aq) + O2(g)
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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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course will help the students to develop the ability to handle information and solve problem related to chemical reactions. COURSE OUTCOMES Upon completion of the course‚ students will be able: 1. To understand and solve the problems related to stoichiometry‚ relative masses‚ empirical and molecular formula as well as mole concept. 2. To illustrate and explain the structure of atoms based on Lewis and molecular orbital structure as well as generate electronic configurations for element. 3. To describe
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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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Stoichiometry is a large and influential factor in chemistry. Stoichiometry is the relationship between the relative quantities of substances taking part in a reaction or forming a compound‚ typically a ratio of whole integers. It deals with the quantitative factors and relationships of the reactants and products. The laws of definite proportions and the law of conservation of mass are both idle laws while dealing with stoichiometry. The law of definite proportions
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(b-cyclodextrin‚ b-CD) cavity protons as well as roxatidine acetate hydrochloride aromatic ring protons revealed the formation of a RAH–b-CD inclusion complex. Detailed FTIR and NMR spectroscopic (1H NMR‚ COSY‚ NOESY‚ ROESY) studies have been done. The stoichiometry of the complex was determined to be 1:1‚ and the overall binding constant was also determined by Scott’s method. The NOESY spectrum confirmed the selective penetration of the aromatic ring of RAH into the b-CD cavity in comparison to that of the
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#1) Fe(s) + Cu+2So4(aq) →Cu(s) +FeSo4(aq) -Single Replacement #2) Pb+2(No3)2(aq) +K+1I-1(aq) →Pb+2I-1+K+1NO3-1(aq) -Double Replacement #3) CuCl2∙2H2O→Cu+2Cl2-1+H2O -Decomposition #4) Mg(s)+2H+1 2Cl-1(aq)→Mg+2Cl-12(aq)+H2(g) -Single Replacement #5) 3H2O2(aq)→3H2O(l)+O2(g)
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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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Isotopes and average atomic mass Isotope: element variations with different atomic mass but same atomic number Isotopic Abundance: the relative amount in which each isotope of an element Calculating: given 2 isotopes of an element [B: 10.01u] [B: 11.01u] 1) Given average atomic mass: 10.81u If given percentages‚ you can find average atomic mass by adding each portion 2) Set variables for unknown values Let x represent % abundance for 10/5 B Let 1-x represent % abundance for 11/5 B Calculate:
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