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Submit Part C Dilution as a procedure in analysis We sometimes purposely dilute solutions if the analyte concentrations are too high to permit an accurate measurement. For example, a spectrophotometer can measure the amount of light that passes through a sample solution for wavelengths in the visible (and sometimes ultraviolet) range. Based on the dissolved solute's properties, we can quantify that solute's concentration. If the solute's concentration is too high, a relatively small amount of incident light having the wavelength that corresponds to the solute's absorption behavior will reach the detector, which results in an inaccurate measurement (consider the result if you blocked the light with an opaque disc). If the solution is diluted, less light is absorbed, and the detector in the spectrophotometer can generate more reliable data. When talking about small quantities, it is important to understand the relationship between common prefixes. Here are some relationships that may help when working through Part C. 1L = 1,000,000 μL 1000 μL openvellum.ecollege.com HA original concentration of Fe²+ = Value Submit 1000 mL OR 0.001 L 1 mL OR 1x 10 L= 0.001 mL The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 8.14x10-6 M. What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units. ▸ View Available Hint(s) Units = ? 1 μL Ⓒ a P Pearson Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |

Submit Part C Dilution as a procedure in analysis We sometimes purposely dilute solutions if the analyte concentrations are too high to permit an accurate measurement. For example, a spectrophotometer can measure the amount of light that passes through a sample solution for wavelengths in the visible (and sometimes ultraviolet) range. Based on the dissolved solute's properties, we can quantify that solute's concentration. If the solute's concentration is too high, a relatively small amount of incident light having the wavelength that corresponds to the solute's absorption behavior will reach the detector, which results in an inaccurate measurement (consider the result if you blocked the light with an opaque disc). If the solution is diluted, less light is absorbed, and the detector in the spectrophotometer can generate more reliable data. When talking about small quantities, it is important to understand the relationship between common prefixes. Here are some relationships that may help when working through Part C. 1L = 1,000,000 μL 1000 μL openvellum.ecollege.com HA original concentration of Fe²+ = Value Submit 1000 mL OR 0.001 L 1 mL OR 1x 10 L= 0.001 mL The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 8.14x10-6 M. What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units. ▸ View Available Hint(s) Units = ? 1 μL Ⓒ a P Pearson Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |

Chemistry
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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3 Submit E Dilution as a procedure in analysis We sometimes purposely dilute solutions if the analyte concentrations are too high to permit an accurate measurement. For example, a spectrophotometer can measure the amount of light that passes through a sample solution for wavelengths in the visible (and sometimes ultraviolet) range. Based on the dissolved solute's properties, we can quantify that solute's concentration. If the solute's concentration is too high, a relatively small amount of incident light having the wavelength that corresponds to the solute's absorption behavior will reach the detector, which results in an inaccurate measurement (consider the result if you blocked the light with an opaque disc). If the solution is diluted, less light is absorbed, and the detector in the spectrophotometer can generate more reliable data. When talking about small quantities, it is important to understand the relationship between common prefixes. Here are some relationships that may help when working through Part C. 1L = 1000 mL 1000 mL = 1,000,000 μL OR Part C original concentration of Fe²+ = Value Submit 80 F3 $ The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 8.14x10-6 M. What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units. View Available Hint(s) 4 R F4 D F % 0⁰4 μÅ 6 5 F5 openvellum.ecollege.com T G ^ 0.001 L = 1 mL OR 1x 106 L = 0.001 mL Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | 6 F6 C www. ? Units MacBook Air Y H & 7 P Pearson F7 U = * = 8 J 1000 μL FB 1 μL 1 ( 9 K DD FO O ) 0 L J F10 1 P (1 F11 + F12 11 +
Transcribed Image Text:3 Submit E Dilution as a procedure in analysis We sometimes purposely dilute solutions if the analyte concentrations are too high to permit an accurate measurement. For example, a spectrophotometer can measure the amount of light that passes through a sample solution for wavelengths in the visible (and sometimes ultraviolet) range. Based on the dissolved solute's properties, we can quantify that solute's concentration. If the solute's concentration is too high, a relatively small amount of incident light having the wavelength that corresponds to the solute's absorption behavior will reach the detector, which results in an inaccurate measurement (consider the result if you blocked the light with an opaque disc). If the solution is diluted, less light is absorbed, and the detector in the spectrophotometer can generate more reliable data. When talking about small quantities, it is important to understand the relationship between common prefixes. Here are some relationships that may help when working through Part C. 1L = 1000 mL 1000 mL = 1,000,000 μL OR Part C original concentration of Fe²+ = Value Submit 80 F3 $ The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 8.14x10-6 M. What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units. View Available Hint(s) 4 R F4 D F % 0⁰4 μÅ 6 5 F5 openvellum.ecollege.com T G ^ 0.001 L = 1 mL OR 1x 106 L = 0.001 mL Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | 6 F6 C www. ? Units MacBook Air Y H & 7 P Pearson F7 U = * = 8 J 1000 μL FB 1 μL 1 ( 9 K DD FO O ) 0 L J F10 1 P (1 F11 + F12 11 +
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