The table below describes a procedure in preparing standard solutions of a protein sample with different concentrations. (A) Determine the concentrations of each tube if the starting concentration of the protein is 500 mg mL. (B) Determine the equation of the line if the concentration (x-axis) was plotted vs the absorbance (y-axis). (C) What is the concentration, in mg mL, of the diluted unknown protein sample if the absorbance at 595 nm is 0.333? Tube Volume of protein, Volume of water, Final concentration, Absorbance # mL mL (at 595 nm) mg mL-1 1 0.00 5.00 0.113 2 0.70 4.30 0.184 3 1.40 3.60 0.251 14 2.10 2.90 0.329 2.80 2.20 0.385 6 3.50 1.50 0.454 7 4.20 0.80 0.503 5.00 0.00 0.577 Suppose that the unknown protein (diluted) sample in 4.C was diluted from a protein stock solution. Determine the concentration of the original unknown protein stock solution if 2.00 mL of the protein solution was mixed with 8.00 mL of water to create the unknown protein (diluted) sample in 4.C.

The table below describes a procedure in preparing standard solutions of a protein sample with different concentrations. (A) Determine the concentrations of each tube if the starting concentration of the protein is 500 mg mL. (B) Determine the equation of the line if the concentration (x-axis) was plotted vs the absorbance (y-axis). (C) What is the concentration, in mg mL, of the diluted unknown protein sample if the absorbance at 595 nm is 0.333? Tube Volume of protein, Volume of water, Final concentration, Absorbance # mL mL (at 595 nm) mg mL-1 1 0.00 5.00 0.113 2 0.70 4.30 0.184 3 1.40 3.60 0.251 14 2.10 2.90 0.329 2.80 2.20 0.385 6 3.50 1.50 0.454 7 4.20 0.80 0.503 5.00 0.00 0.577 Suppose that the unknown protein (diluted) sample in 4.C was diluted from a protein stock solution. Determine the concentration of the original unknown protein stock solution if 2.00 mL of the protein solution was mixed with 8.00 mL of water to create the unknown protein (diluted) sample in 4.C.

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

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 2.81 mL of the blue dye stock solution to 25.00 mL. The measure absorbance for the prepared solution is listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical | × 10 |M (b) What is the experimental molar concentration? [Bluelexperimental x 10 M (c) What is the percent error? Percent error (blue) =
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) = %
5. (1) (ii) Ibuprofen (206.3 g/mol) absorbs at 255 nm and shows a molar absorptivity of 3010 L/mol.cm. A tablet of ibuprofen, 0.6654 g, was ground and 0.2203 g powder was dissolved in 20% methanol in a 100 mL volumetric flask (Solution A). Exactly 5.0 mL of Solution A was diluted in a 50.0 mL flask and the resulting solution showed an absorbance of 0.1228 AU in a 1.00 cm cell. (i) What is the concentration (mol/L) of ibuprofen in the 100 mL stock solution? (ii) Report the amount of ibuprofen in mg/Tablet. Ibuprofen H3C | HCCH; 1 H3C CH3 -CH-COOH
(b) A compound having molecular weight 151.163 g/mol is determined in a sample. A 0.0302 g sample was dissolved in an aqueous solvent and diluted the solution to 1 L. The solution has A max at 243 nm (ɛ=2.6×104 cm1 mol1 L). The solution exhibits an absorbance of 0.642 in a 2 cm cell. Calculate the percentage of the above compound in the sample.
What is the concentration of a tyrosine solution when the absorbance at 280 nm is 1.5 using a 1 cm cuvette and the molar extinction coefficient is 1405 L/mol·cm?
A student measures k for a certain blue dye to be 400.4 M-1 at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.118 at this wavelength?
A solution of Tryptophan has an absorbance at 280 nm of 0.54 in a 0.5 cm length cuvette. Given the absorbance coefficient of trp is 6.4 x 103 Lmol-1cm-1. What is the concentration of solution? The options are as follows A) 0.17 x10-3 mol/L B)2.56x10-3mol/L C)0.17x10+3mol/L D)2.56x10+3mol/L
Determine the net charge of the predominant form of Asp at (a) pH 1.0, (b) pH 3.0.
A solution of Tryptophan has an absorbance at 280 nm of 0.54 in a 0.5 cm length cuvette. Given the absorbance coefficient of trp is 6.4 x 103 Lmol-1cm-1. What is the concentration of solution? The answers are as follows A)0.17x10-3mol/L B)2.57x10-3mol/L C)0.17x10+3mol/L D)2.57x10+3mol/L
(A) You measured the absorbance of a solution of 0.2 mM NADH at 340 nm and the reading was 0.55. Calculate the extinction coefficient of NADH.
A 2.78 ✕ 10−4 M solution of a compound has an absorbance of 0.417 at 520 nm in a 1.00 cm cell. The solvent's absorbance under the same conditions is 0.020. (a) What is the molar absorptivity of the unknown compound? M -1cm-1(b) What is the concentration of the compound in a solution, if the absorbance of the solution in a 1.00 cm cell at 520 nm is 0.391? M
Fe+3 (aq) + SCN – (aq) FeSCN +2 (aq) She mixes 4.00 mL of 2.00 mM SCN– and 5.00 mL of 2.00 mM Fe+3 ions, then diluting with 1.00mL of water to give a total volume of 10.00mL. She measures the absorbance of the solution asbeing 0.210. If she has previously calculated the molar absorbtivity constant (ε) of the product tobe 2583 cm–1 M–1, what is her best estimate for the K value for this reaction?