1. Calculate the percent of SiO, in the mixture by using the equation: %= part * 100 whole 2. Calculate the percent of NaCl in the in the mixture. (continued on back!) Fundamental Chemistry I 44 3. Calculate the percent recovery for the experiment.
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- 2) As an example of precision and accuracy of data, suppose the % carbon in a single compound has been measured thrce separate times by 2 different students. The theoretical % carbon is 21.34%. Student 1: trial 1:26.11%, trial 2: 26.24% trial 3: 25.92 %, Avg - 26.09 Student 2: trial 1: 20.35%. trial 2: 22.64 % trial 3: 19.79 %. Avg = 20.93 a) Which student had the more precise data and how can you tell? b) Which student had the more accurate data and how can you tell? 3a) Calculate the % error of Student 1 data in problem 2 above. Show all work below. WATCH SIG FIGSPage 2 2. A 0.9527 g sample containing only KCI and CaCl2 yielded 3.9802 g of dried Hg2Cl2. Calculate the percent of each halogen compound in the sample. KCI = K* + CIr; CaCl2 = Ca2+ + 2C-; 2CI- + 2Hg* = Hg2Cl2 CI 35.453; K 39.0983; Ca 40.078; Hg 200.59Table 1: Standardization Data Trial 1 Trial 2 O145504 Mass of KHP 04536 Initial burette reading 0.05ML 12.3 ML Final burette reading 12.8 a6.omL Volume of base used ר.12 13.2 mL Data Analysis: KH Cg Hg Da (MOIAR MASS 2041ag) 1. Calculate the molarity of base for each trial. You must use dimensional analysis – show all unit conversions (hint: start with grams of KHP used). Review the balanced equation for KHP and NaOH you wrote in Expt 11 part 1. (204.29 TRIAI 1: 0.4550g. Average: Trial 2: Trial 1: with 1875 mL of your base (use the average
- Standardization of EDTA Solution Weight of pure CaCO3: 0.2517 g % Purity of CaCO3: 98.0% Total volume of standard CaCO3 solution: 250.00 mL Trial 1 2 3 Volume of standard CaCO3 solution (ml) 25.00 25.00 25.00 Final Volume Reading EDTA (ml) 24.30 47.95 24.72 Initial Volume Reading EDTA (ml) 0.00 24.30 0.20 Volume of titrant, EDTA (ml) Molarity of EDTA (M)A student weighed 2.0 g crude sample (impure) and found 0.3 g glass and recovered 0.7 g of the sample after purification. Determine the percentage of the pure compound (recovery)? Select one: O a. 40% Ob. 55% OC. 65% O d. 35% Snot too much of a compound on tha TIC nlato wIould make2 TOSHIBA 144 A & %24 4 8 A 9. T Y Y FIG ý Hi J J - K B NIM Saur X Macmilla X 2/ Course X 50 ~ T Sections X Submit Answer evo/index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707786042&snapshot! References lancing Molecular Equations: This is group attempt 2 of 10 HOMEW X Use the References to access Important values if needed for this question. When the following molecular equation is balanced using the smallest possible Integer coefficients, the values of these coefficients are: Na (s) + H₂0 (1). NaOH (aq) + H₂ (8) ≡く □ □ A MindTap ㅁ Autosaved at 5:51 PM MacBook Air Gatoms to When the following molecular equation is balanced using the smallest possible Integer coefficients, the values of these coeffi Br₂(g) + Cl₂(g) →BrCl(g) X Dom
- 28 Report Sheet Separation of the Components of a Mixture D. Determination of Percent Recovery Mass of original sample 10.588 Mass of determined (NH Cl+ NaCl+ SiO2) 1-88 8 Differences in these weights g matter recovered Percent recovery of matter %3D = %00 % g original sample Account for your errors. Combor QUESTIONS 1. Could the separation in this experiment have been done in a different order? For example, if the mixture was first extracted with water and then both the extract and the insoluble residue were heated to dryness, could you determine the amounts of NaCl, NH,Cl, and SiO, originally present? Why or why not? Consult a handbook to answer these questions. 2. How could you separate barium sulfate, BaSO4, from NaCl? 3. How could you separate magnesium chloride, MgCl2, from silver chloride, AgCl? 4. How could you separate tellurium dioxide, TeO2, from SiO,? 5. How could you separate lauric acid from a-naphthol? (See Table 3.1.)Sample Physical Appearance 0.1 M Na2CO3 0.1 M CaCl2 Na2CO3 + CaCl2 mixture Part II filtrate + CaCl2only tiype solutio
- 119 X My Course X Macmillan: X Course Mo X What is the FORMULA for the limiting reagent? Submit Answer Sections 5 X .com/static/nb/ui/evo/index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707786042&snapshoti... Use the References to access important valdes ir needed for this question. 900 For the following reaction, 9.43 grams of carbon (graphite) are allowed to react with 28.5 grams of oxygen gas. carbon (graphite) (s) + oxygen (g) carbon dioxide (g) What is the maximum amount of carbon dioxide that can be formed? What amount of the excess reagent remains after the reaction is complete? HOMEWOR X MacBook Air MindTap - C X GI grams gramsASSAY Calibration solutions Calibration solutions of naproxen in the range 5 – 25 μg/mL were prepared. Sample preparation 20 tablets weighing 12.3819 g were crushed to a fine powder. A portion of the powder (145.4 mg) was shaken with approximately 150 mL of acetic acid (0.05 M) for 5 min and then made up to volume in a 250 mL volumetric flask (stock solution). Approximately 50 mL of the stock solution was filtered and a 25 mL aliquot was diluted to 100 mL in a volumetric flask. 10 mL of the resulting solution was further diluted to 100 mL with acetic acid (0.05 M). Analysis The standards and sample solutions were analyzed by HPLC under the following conditions: Column: octadecylsilyl (ODS), 4.6 mmx150 mm, mobile phase: acetonitrile : 0.05 M acetic acid (85:15), flow rate: 1 ml/min, UV detection at 243 nm. Results: A calibration curve of concentration versus peak area was constructed for the standard solutions and gave the straight-line equation: y = 3555.6x + 85, r = 0.9999 The area…(10) You have 4 powdered samples, A, B, C, & D. One sample contains fullerenes, C16 to C70. Another is nano diamond. Another one is a mixture of C60 and carbon nanotubes. The 4th is a mixture of graphite & graphene. Indicate the analytical methods you would use to identify and distinguish the samples from each other.