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Chapter 18: Q9 P (page 456)

18-9 Why does a compound whose visible absorption maximum is at 480 nm (blue-green) appear to be red?

Short Answer

Expert verified

The Transmitted light will be complement of the color of absorption at 480 nm.

Step by step solution

01

Definition

Spectrophotometry isa standard and inexpensive technique to measure light absorption or the amount of chemicals in a solution. It uses a light beam which passes through the sample, and each compound in the solution absorbs or transmits light over a certain wavelength

Absorption: The process in which incident radiated energy is retained without reflection or Transmission on passing through the medium.

02

Absorption

A Compound whose visible absorption maximum at 480 nm (blue-green) because the transmitted light (red) will be complement to the color taht is absorbed(blue-green).

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Most popular questions from this chapter

The absorbance of a 2.31×10-5M solution of a compound is 0.822 at a wavelength of 266nm in a 1.00-cm cell. Calculate the molar absorptivity at 266nm.

Vapor at a pressure of 30.3μtbar from the solid compound pyrazine had a transmittance of 24.4% at a wavelength of 266nm in

a 3.00 - cm cell at 298K

Pyrazine

(a) Convert transmittance to absorbance.

(b) Convert pressure to concentration (mol/L) with the ideal gas law (Problem 1-18).

(c) Find the molar absorptivity of gaseous pyrazine at 266nm.

Standard addition. Selenium from 0.108 g of Brazil nuts was converted into the fluorescent product in Reaction 18-15, and extracted into 10.0 mL of cyclohexane. Then 2.00 mL of the cyclohexane solution were placed in a cuvet for fluorescence measurement. Standard additions of fluorescent product containingSe/mL are given in the table. Construct a standard addition graph to find the concentration of Se in the 2.00-mL unknown solution. Find the wt%of Se in the nuts and its uncertainty and 95% confidence interval

Preparing standards for a calibration curve.

(a) How much ferrous ammonium sulfate(FeNH42SO42⋅6H2OFM392.15)should be dissolved in a 500mL volumetric flask withto obtain a stock solution with1000μgFe/mL?

(b) When making stock solution (a), you weighed out 3.627 g of reagent. What is the Fe concentration in?

(c) How would you prepare 250mL of standard containing containing ~1,2,3,4,5,6,7,8and10in0.1MH2SO4infrom stock solution (b) using only 5- and 10-mL Class A pipets, only 250mL volumetric flasks, and only two consecutive dilutions of the stock solution? For example, to prepare a solution with ~4μgFe/mL,, you could first dilute 15mL(=10+5mL) of stock solution up to 250 mL mLto get~(1525)(1000μgFFe/mL)=∼60μgFe/mL Then dilute 15mL of the new solution up to 250 mL again to get~(15250)(60μgFe/mL)=∼3.6μgFe/mL

Preparing standards for a calibration curve.

(a) How much ferrous ethylene diammonium sulfate(FeH3NCH2CH2NH3SO42⋅4H2O,FM382.15)should be dissolved in a 500mL volumetric flask with1MH2SO4to obtain a stock solution with~500μgFe/mL2?

(b) When making stock solution (a), you actually weighed out 1.627 g of reagent. What is the Fe concentration in role="math" localid="1668357579931" 500μgFe/mL2?

(c) How would you prepare 500 mL of standard containing 1,2,3,4, and5μgFe/mL2in0.1MH2SO4infrom stock solution (b) using any Class A pipets from Table 2-4 with only 500 -mL volumetric flasks?

(d) To reduce the generation of chemical waste, describe how you could prepare 50 mL of standard containing, andinfrom stock solution (b) by serial dilution using any Class A pipets from Table 2-3 with only 50mL volumetric flasks?
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