Table 2.1. Unknown Mixture Identification Code: Filter paper weight 0.906g Glassware and Component Mass Evaporating Dish (g). 42.7739 Evaporating Dish + Sample (g) 43.3243 Sample (g) 0.551 Beaker A (g) 67.9943 Beaker A + NaCI (g) 68.416g NaCl (g) 0.4929 Evaporating Dish (g) 42.773g Evaporating Dish + Sio, (g) 43.002g SiO, (g) 0.229 9 Evaporating Dish + Filter Paper (g) 43.6799 Evaporating Dish + Filter Paper + CaCO, (g) 43.8749 CaCO, (g) 0.195g Table 2.2. Unknown Mixture Identification Code: Glassware and Component Mass Mass Sample (g) Mass NaCl (g) % NaCl in Mixture Mass SiO, (g) % Sio, in Mixture Mass CaCO, (g) % CACO, in Mixture NaCl, SiO, CaCo, recovered (g) Total % Recovery

Table 2.1. Unknown Mixture Identification Code: Filter paper weight 0.906g Glassware and Component Mass Evaporating Dish (g). 42.7739 Evaporating Dish + Sample (g) 43.3243 Sample (g) 0.551 Beaker A (g) 67.9943 Beaker A + NaCI (g) 68.416g NaCl (g) 0.4929 Evaporating Dish (g) 42.773g Evaporating Dish + Sio, (g) 43.002g SiO, (g) 0.229 9 Evaporating Dish + Filter Paper (g) 43.6799 Evaporating Dish + Filter Paper + CaCO, (g) 43.8749 CaCO, (g) 0.195g Table 2.2. Unknown Mixture Identification Code: Glassware and Component Mass Mass Sample (g) Mass NaCl (g) % NaCl in Mixture Mass SiO, (g) % Sio, in Mixture Mass CaCO, (g) % CACO, in Mixture NaCl, SiO, CaCo, recovered (g) Total % Recovery

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter1: Basic Concepts Of Chemistry

Section: Chapter Questions

Problem 43GQ: Hexane (C6H14, density = 0.766 g/cm3), perfluoro-hexane (C6F14, density = 1.669 g/cm3), and water...

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using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution? 5.027 g 2. Calculate the mass of solid CuSO4 dissolved in the solution? 0.033 g 3. Calculate the number of moles of solid CuSO4 dissolved in the solution? 2.07 x 10-4 mol4. Calculate the mass of water evaporated from the solution? 0.0414 M5. Calculate the density of solution, (g solution/mL solution)?6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution)?7. Calculate the molality of solution (moles CuSO4/kg solvent)?8. Calculate the molarity of solution (moles CuSO4/L solution)?9. Given that the true molarity is 0.0400 M, calculate the percent error…
using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution2. Calculate the mass of solid CuSO4 dissolved in the solution.3. Calculate the number of moles of solid CuSO4 dissolved in the solution.4. Calculate the mass of water evaporated from the solution.5. Calculate the density of solution, (g solution/mL solution).6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution).7. Calculate the molality of solution (moles CuSO4/kg solvent).8. Calculate the molarity of solution (moles CuSO4/L solution).9. Given that the true molarity is 0.0400 M, calculate the percent error of your result.
Sample Physical Appearance 0.1 M Na2CO3 0.1 M CaCl2 Na2CO3 + CaCl2 mixture Part II filtrate + CaCl2
Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
Substance Melting Points in ℃ Benzoic acid 122.3 ℃ Succinimide 125-127 Urea 133 ℃ Cinnamic acid (trans). 133 ℃ Thiourea 182 ℃ Hippuric acid. 187 ℃ For Questions 1-3 assume that you were given 5.00 g of an unknown A for this lab, one of the six compounds whose melting points you looked up for prelab. 1. You recrystallized A and obtained 2.23 g pure product. What was your percent recovery? That is, what percent of the original mass did you get back? Show your work. 2. Assume you took the melting point of the pure product and it was 123oC. Considering…
What volume of iron (7.87 g/cm3) would be required to balance a 1.25 cm3 sample of lead (density 11.4 g/cm3) on a two-pan laboratory balance?
A method to determine an antibiotic was developed and validated in a pharmaceutical company. The method allows analysis of 100 mg tablets containing 7.5 mg of the antibiotic. According to the validation data, the confidence limits are 7.50 mg± 0.04mg. How many samples will need to be analyzed for an analyst to ensure that the content of the antibiotic in a macerated sample of that drug is 7.50 mg ± 0.03 mg with 95% reliability when analyzing 100 mg of the macerated sample?
A forensic chemist prepares a standard of caffeine in chloroform for use in a quantitative assay. The caffeine is purchased from a reputable supply company and arrives with a certificate stating that it is 99.5% pure or better (written 99.5% + or + 99.5%). The analyst needs to make a stock solution at a concentration near 1 mg/mL. To do so, she obtains a Class A 50.00 mL volumetric flask (± 0.05 mL) and uses an analytical balance to accurately weight out 49.6 mg. The balance uncertainty is listed as ± 0.0003 g near the 50 mg range. The analyst quantitatively transfers the powder to the flask and carefully dilutes the solution to volume. Report the concentration of the solution in mg/mL and the propagated uncertainty associated with it. Use the NUSAP form to report your answer with the proper number of significant figures in the final result. You get to pick which “assessment” is presented.
A 3-component mixture of compounds A, B, and C (5.000 g) was separated by filtration, extraction, and evaporation to yield 0.462 g of A, 2.358 g of B, and 1.612 g of C. What is the % composition of compound C (relative to the sum of all recovered masses)? Report your answer to two decimal places without the % symbol.
i have hard time geting it stright even after I do the experiment can u help me with the one pls Material ChemicalsSealed NO2 tubes, KSCN solution (0.002 M), acidified Fe(NO3)3 solution (0.2 M), KSCN crystals, Fe(NO3)3 crystals, KOH (concentrated (8 M)), distilled waterApparatus:Bunsen burner, ring stand, wire gauze, matches, thermometer, dropper, test tubes, glass stirring rod, beaker tongs Procedure Part A: Fill a 600 mL beaker to the 3/4 mark with water. Bring to a boil using a Bunsen burner. In another 600 mL beaker, fill to the 1/2 mark with water; add ice in order to lower the temperature to about 0°C. Note the room temperature. Observe the NO2 thoroughly at room temperature. Place the sealed NO2 tube in the cold bath. Note your observations. Remove the test tube from the cold bath. Let the test tube stand until it reaches room temperature. Note your observations. Place the test tube in the hot bath. Note your observations. Remove the test tube from the hot bath. Let the test…
Given the following data forMass of test tube, beaker and cyclohexane = 100.17 gMass of test tube and beaker = 84.07 gFreezing point of cyclohexane = 6.59 oCMass of weighing paper + naphthalene =1.080 gMass of weighing paper = 0.928 gFreezing point solution = 5.11oCKf = 20.8oC/mDetermine the followinga. mass of cyclohexane in g (2 decimal places); _____b. mass of naphthalene in g (4 decimal places); _____c. freezing point depression (2 decimal places); _____d. molality of solution (3 significant figures); _____e. moles of naphthalene (3 significant figures); _____f. molar mass of naphthalene, experimentally (3 significant figures); _____g. % error if theoretical molar mass of naphthalene is 128.17 g/ mole, USE ABSOLUTE VALUE (3 significant figure); ____
A sample sodium is being dried. After 1 hour drying, the mass of the sample was 0.337g. After an additional 30 minutes of drying, the mass of the sample is 0.333g. What is the percent change between the first and second meaasurement? if to be considered "dry", two consecutive measurements must have a percent change <_ +- 1%; is the sample dry?