B) I 2 \red to yellow 02: To calculate the molecular weight of a volatile liquid, the liquid was vaporized in an Erlenmeyer flask which had a total volume of 152 mL. In the procedure, the flask containing an excess amount of the volatile liquid was covered with aluminum foil with a tiny pinhole, and then the flask and the liquid was laced in a boiling water bath at 100 °C. The atmospheric pressure was measured 754 torr with a barometer the room. As the liquid in the flask vaporized, the excess vapor escaped through the pinhole until no visible liquid remained in the flask. The flask was then removed from the water bath and allowed to cool. The mass of the flask, foil, and vapor was 94.53 g. The initial mass of the dry, empty flask and foil was 94.12 g. From this information, calculate the molecular weight of the volatile liquid in grams per mole. E) None of them D) 36 A) 48 B) 56 C) 83 blanch is hudroxide

B) I 2 \red to yellow 02: To calculate the molecular weight of a volatile liquid, the liquid was vaporized in an Erlenmeyer flask which had a total volume of 152 mL. In the procedure, the flask containing an excess amount of the volatile liquid was covered with aluminum foil with a tiny pinhole, and then the flask and the liquid was laced in a boiling water bath at 100 °C. The atmospheric pressure was measured 754 torr with a barometer the room. As the liquid in the flask vaporized, the excess vapor escaped through the pinhole until no visible liquid remained in the flask. The flask was then removed from the water bath and allowed to cool. The mass of the flask, foil, and vapor was 94.53 g. The initial mass of the dry, empty flask and foil was 94.12 g. From this information, calculate the molecular weight of the volatile liquid in grams per mole. E) None of them D) 36 A) 48 B) 56 C) 83 blanch is hudroxide

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 6P

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A chemist receive different mixtures for analysis with the statement that it contain NaOH, NaHCO3 , Na2CO3 or compatible mixtures of these substances together with the inert material. From the data given, identify the respective materials and calculate the percentage of each component. 1.000g samples and 0.2500 N HCl were used in all cases. Sample 1 With phenolphthalein as the indicator, 24.32 ml of HCl was used. A duplicate sample required 48.64 ml HCl using methyl orange as the indicator. Sample 2. With phenolphthalein as the indicator it uses 28.2 ml of HCl to make it colorless and added with methyl orange indicator and uses 11.3 ml of HCl to reach the end point.
The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.
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In this experiment you were given the concentration of NaOH(aq). That concentration was determined in part A.1. by using a solid acid, potassium hydrogen phthalate. Suppose the potassium hydrogen phthalate used for the standardization of the sodium hydroxide solution is not completely dry. This technique error will result in the reported concentration of NaOH(aq) to be ____________. a. unaffected b. too high c. too low
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
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SCE students measured the concentration of HCl in a solution by titrating with different indicators to find the end point.Indicator Mean HCl concentration (M)(± standard deviation)Number of measurementsBromothymol blue 0.09565 ± 0.00225 28Methyl red 0.08686 ± 0.00098 18Bromocresol green 0.08641 ± 0.00113 29Is the difference between indicators 1 and 2 significant at the 95% confidence level? Answer the same question for indicators 2 and 3
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?
Given the following data and the λmax determined in the previous questions, determine:1) the molar absorptivity of copper at λmax of cobalt 2) the molar absorptivity of copper at λmax of copper 3) the molar absorptivity of cobalt at λmax of cobalt 4) the molar absorptivity of copper at λmax of cobalt 5) the concentration of cobalt in mM 6) the concentration of copper in mM Copper concentration, mM λmax cobalt λmax copper 20.00 0.177 0.238 40.00 0.382 0.487 60.00 0.518 0.731 80.00 0.765 1.134 100.00 0.902 1.391 Cobalt concentration, mM λmax cobalt λmax copper 20.00 0.186 0.163 40.00 0.412 0.354 60.00 0.637 0.477 80.00 0.754 0.694 100.00 0.961 0.831 unknown, Abs at λmax cobalt 0.893 unknown, Abs at λmax copper 0.997
Solution of Pb(NO3)2 and NaCl are combined, resulting in concentrations of 0.0050 M Pb(NO3)2 and 0.00250 M NaCl immediately upon mixing. select the correct description of the final solution, given that the Ksp of PbCl2 is 1.7x10^-5. A) NaNO3 Precipitates B) All solutes reamin soluable C) Pb(NO3)2 precipitates D) PbCl2 precipiates E) All Solutes precipitate.
Table 1: Temp vs. solubility data of ammonium chloride. Test tube g NH4Cl/10 mL H2O Crystallization temp. (ºC) 1 1.0 g/10 mL H2O 10 oC 2 1.8 g/10 mL H2O 20 oC 3 2.9 g/10 mL H2O 40 oC 4 3.8 g/10 mL H2O 65 oC 5 4.4 g/10 mL H2O 95 oC Use the table to plot a solubility curve for ammonium chloride on the graph provided below. For the best fit line, use a smooth curve. "Mass of Solute per 100 mL of H2O," should be written on the y-axis (use increments of 2g for every box). "Temperature (°C)" should be written on the x-axis (use increments of 10 °C for every 2 boxes).