VI. Flame TestWatch the following video: https://www.youtube.com/watch?v=kkBFG1mTSBkRecord the color of the flame observed for each substance tested in the video.Solution Color ObservedSrCl₂NaClKCISolutionLICICuCl2CaCl₂Color Observed1. Explain why colored flames are observed when elements are heated?

Answered: Image /qna-images/answer/86f117d8-9b7a-4943-b4d4-c7f3f92e1c3b.jpg

● Watch the following video: https://www.youtube.com/watch?v=kkBFG1mTSBk Record the color of the flame observed for each substance tested in the video. Solution SrCl₂ NaCl KCI Color Observed Solution LICI CuCl2 CaCl₂ Color Observed 1. Explain why colored flames are observed when elements are heated?

● Watch the following video: https://www.youtube.com/watch?v=kkBFG1mTSBk Record the color of the flame observed for each substance tested in the video. Solution SrCl₂ NaCl KCI Color Observed Solution LICI CuCl2 CaCl₂ Color Observed 1. Explain why colored flames are observed when elements are heated?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Gold can be determined in solutions containing high concentrations of diverse ions by ICP-AES. Aliquots of 50.0 mL of the sample solution were transferred to each of four 100.0 mL volumetric flasks. A solution was prepared containing 10.0 mg/L Au in 20% H2SO4 and quantities of this solution were added to the sample solutions to give 0, 2.5, 5, and 10 mg/L added Au in each of the flasks. The solutions were made up to a total volume of 100.0 mL, mixed, and analysed by ICP-AES. The resulting data are presented in the following table. Added Au, mg/L Emission Intensity Count 12,568 19,324 26,622 40,021 0.0 2.5 5.0 10.0 Calculate the concentration of gold in the original sample.
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A water sample was analyzed for Fe content using the iron- phenanthroline method. The following data were obtained from the analysis: Reagent Blank Absorbance Absorbance (au) Reagent Blank Absorbance 0.003 Concentration of Stock Solution: 10 ppm Volume of Stock Solution (mL) Total Volume of Standard Solution Concentration of Standard Solution (ppm) Absorbance (au) (mL) 0.50 10.00 0.012 1.00 10.00 0.132 2.00 10.00 0.267 3.00 10.00 0.349 4.00 10.00 0.428 5.00 10.00 0.560 Volume of Unknown Solution Total Volume of Unknown Solution Trial Absorbance (au) (mL) (mL) 1 5.00 10.00 0.289 2 5.00 10.00 0.296 3 5.00 10.00 0.281 Determine the value of the slope (m), y-intercept (b), and the coefficient of determination (r²) A m = 0.1128; b = -4.0 x 10-5; r2 = 0.9880 B m = 0.1128; b = -4.0 x 10-5; r² = 0.9762 C) m = 0.1128; b = -3.0 x 10-³; r² = 0.9880 D m = 0.1128; b = -3.0 x 10-³; r² = 0.9762
Absorbance Beer-Lambert's Law (Spectrophotometry) #2 To spectrophotometrically determine the mass percent of cobalt in an ore containing cobalt and some inert materials, solutions with known [Co"] are prepared and the absorbance of each of the solutions is measured at the wavelength of optimum absorbance. The data are used to create a calibration plot, shown below. 0.80 0.70- 8 0.60- 0.50- 0.40- 0.30 0.20- 0.10- ++- 0.015 Concentration (M) A 0.6 g sample of the ore is completely dissolved in concentrated HNO3(aq). The mixture is diluted with 2+ water to a final volume of 50.00 mL. Assume that all the cobalt in the ore sample is converted to Co'(aq). a. What is the (Co] in the solution if the absorbance of a sample of the solution is 0.74? b. Calculate the number of moles of CoT(ag) in the 50.00 mL solution. 2+ C. Calculate the mass percent of Co in the 0.630 g sample of the ore.
What is the balanced equation for the combustion of C8H7NO2SBrCl in aC,H,N,S elemental analyzer?
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1. A sample of freshly precipitated silver chloride weighs 704.7 mg. Before the solution can be filtered and washed, 10.0 mg of AgCl is photodecomposed. After the precipitate is filtered and washed, another 10.0 mg of AgCl is photodecomposed. Calculate the weight of the precipitate.
What is the mass percent of Fe for each trial ? Mass of (NH4)2Ce(NO3)6 (in 100.00 mL) = 4.5038 g Mass of unknown (in 250.00 mL) = 10.000 g Trial # Volume of unknown solution (mL) Titration Volume (mL of Ce4+) Mass Percent(% Fe) 1 25.00 mL 7.20 mL 2 25.00 mL 7.40 mL 3 25.00 mL 7.60 mL 4 25.00 mL 7.50 mL
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2. In one gravimetric analysis, the aluminum in a 1.2g sample of impure NHAI(SO4)2 was precipitate as hydrous ALO3.XH2O. The precipitate was filtered and ignited at 1000 °C to give anhydrous Al2O3 which weighed 0.1798g. Calculate the % Al inthe sample. 3. A sample of 0.4500g impure potassium chloride was dissolved in water treated with excess silver nitrate solution. 0.8402 g of silver chloride was precipitated. What is the percentage of potassium chloride in the sample?
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