You graph the calibration curve of a solution of an unknown metal (we will call it M+) at 400 nm. The graph is shown below. What is the concentration the solution with an absorbance of 0.500 at 400 nm? Absorbance 1.4 1.2 1 0.8 0.6 0.4 0.2 0 Absorbance vs. Concentration at 400 nm for solution of M+ 50 100 200 Concentration (mmol/L) 150 250 300 350 400 450

You graph the calibration curve of a solution of an unknown metal (we will call it M+) at 400 nm. The graph is shown below. What is the concentration the solution with an absorbance of 0.500 at 400 nm? Absorbance 1.4 1.2 1 0.8 0.6 0.4 0.2 0 Absorbance vs. Concentration at 400 nm for solution of M+ 50 100 200 Concentration (mmol/L) 150 250 300 350 400 450

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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

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

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.8: Stoichiometry Of Reactions In Aqueous Solution-titrations

Problem 2RC

See similar textbooks

Similar questions

.Q1. To determine the concentrations (mol/L) of Co(NO3)2 (A) and Cr(NO3)3(B) in an unknown sample, the following representative absorbance data wereobtained.A (mol/L) B (mol/L) 510nm 575nm5×10−1 0 0.714 0.0970 6×10−2 0.298 0.757Unknown Unknown 0.671 0.330Measurements were made in 1.0 cm glass cells.i. Calculate the four molar absorptivities: ∈A(510), ∈A(575), ∈B(510) and ∈B(575).ii. Calculate the molarities of the two salts A and B in the unknown.
A solution has a %T value of 48.2% at 600 nm. What is the absorbance of this solution at this wavelength?
Find the concentration of benzene in hexane if the absorbance is 0.188 in a 1.000-cm cell.
Based on the calibration curve, what is the molar concentration for a solution with a measured absorbance of 0.383?
A solution of a specific vitamin has a åmax of 245 nm and a concentration of 4.15 x 10-M. The absorbance of the solution at 245 nm is A = 0.145. What is the molar absorptivity of the vitamin at 245 nm ? A sample path length is 1.00 cm. molar absorptivity: L mol-'cm-!
2. ] You make 150.0 mL of a copper(II) sulfate solution but forget to cover it before leaving for the day. The next class, you measure the volume and find that you only have 132.0 mL remaining. You didn’t record the initial concentration, but you measure the absorbance of the remaining solution at 620 nm and find that it is 0.386. You also construct the following calibration curve for CuSO4: Standard solution Abs620 0.50 M 0.424 0.40 M 0.336 0.30 M 0.247 0.20 M 0.159 (refer to image) a. What is the value for k (in Beer’s Law)? Provide a calculation or graph to support your answer. b. What is the concentration of the (remaining) solution? c. What was the concentration of the original solution from the first class? d. If you removed 7.5 mL from the 132.0 mL solution in the process of measuring the absorbance, how much water should you add to obtain the original concentration that you solved for in part (c)?
A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 7.9 × 10–3 M. The absorbance of this solution is measured, and the equilibrium FeSCN2+(aq) concentration is found to be 1.8 × 10–3 M. Fe3+ + SCN- <=> FeSCN2+ Determine the equilibrium constant for the above reaction
The drug Tolbutamine (molar mass = 270) has a molar absorptivity of 703 at 262 nm.One tablet is dissolved in water and diluted to a volume of 2L. If the resulting solution(taken in a cell of 1 cm) exhibits an absorbance equal to 0.687 at 262 nm, how manygrams Tolbutamine are contained in the tablet?
5. A 2.50x10-5 M solution of a specific dye has an absorbance value of 1.300 when measured at 525 nm in a cell with a path length of 2.00 cm. Calculate the molar absorptivity of this dye at this wavelength.
In an analytical laboratory a chemical compound namely Paracetamol (151.163 g/mol) is determined in a sample. A sample weighing 0.0295 g was dissolved in a solvent and diluted the solution to 1 L. The solution has λ max at 243 nm (ε=2.6×104 cm-1 mol-1 L). The solution exhibits an absorbance of 0.638 in a 2 cm cell. Calculate the percentage paracetamol in the sample.
Blue Blue dye stock solution Absorbance at 630 nm Calibration curve Part 1: 0.1944 M 0.00697 y = 0.0682x A purple solution is prepared by mixing 5.00 mL of the blue dye solution with 6.75 mL of red dye solution. The calibration curve for each color is provided. Part 2 out of 3 (a) Determine the theoretical molar concentration of each dye in the mixture. [Blueltheoretical = 8.27 x 10-2 [Red] theoretical = 1.16 [Bluelexperimental [Redlexperimental " *10-1 M M x 10 (b) Using the absorbance and calibration curve for each dye, calculate the experimental molar concentration of each dye in the mixture. x 10 Red Red dye stock solution Absorbance at 500 nm Calibration curve 0.2015 M 0.00193 y = 0.0170x M M
6. Blue Blue dye stock solution 0.293 M Absorbance at 630 nm 0.00265 Calibration curve y = 0.0833x A solution is prepared by diluting 2.79 mL of the blue dye stock solution to 25.00 mL. The measured absorbance for the prepared solution is listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical x 10 |M (b) What is the experimental molar concentration? [Blue]experimental x 10 M (c) What is the percent error? Percent error (blue) = %