The equation of the line for an Abs vs. [FESCN^2+] plot was determined to be y=4462.2x - 0.00329. The absorbance for an unknown concentration was 0.512. What is the concentration of FESCN^2+ in the sample? O A. 1.15 X 10^-4 O B. 1.15 X 10^-6 O C. 1.23 X 10^-4 D. 1.5 X 10^-5
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- answer the following 3. What is the path length in centimeters when the molar absorptivity for a given absorbing species is 1.32 x 103L mol-1cm-1, the concentration is 0.000923 M, and the absorbance is 0.490? 4. Value for Kw at 0.0°C is 1.14 x 10-15. Calculate the pH for a neutral solution at this temperature.The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.4150.415 . The slope-intercept form of the equation of the line is ?=4558.4?+0.0147y=4558.4x+0.0147 . The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe3+Fe3+ concentration of the unknown solution?The un-ionized form of the weak acid HA does not absorb in the visible region. When it ionizes, its conjugate base (A-) absorbs light strongly at 510 nm. The following data were obtained by measuring the absorbance at 510 nm of solutions with a concen- tration of 1.0 x 104 M HA in different pH buffers. pH Absorbance 2.0 0.00 3.0 0.00 4.0 0.00 5.0 0.025 6.0 0.180 7.0 0.480 8.0 0.570 9.0 0.595 10.0 0.595 11.0 0.595 12.0 0.595 What is the approximate pK of HA?
- The equation of the line for an Abs vs. [FeSCN^2+] plot was determined to be y=4462.2x - 0.00329. The absorbance for an unknown concentration was 0.512. What is the concentration of FeSCN^2+ in the sample? A. 1.15 X 10^-4 B. 1.15 X 10^-6 O C. 1.23 X 10^-4 O D. 1.5 X 10^-5 At equilibrium, [Fe^3+] = 3.1X 10^-4 M and [SCN^-] = 8.6 X 10^-4 M. Using your answers from the previous question on equilibrium, what is the value of K? O A. 3.19 X 10^-4 О В. 431 O C. 43.1 O D. 3845- A 5.0 mL solution containing 3.36 pm Fe(Ill) ions is diluted to 50.0 mL by first treating with an excess of an appropriate amount of KSCN solution. The molar absorptivity of the FeSCN^2+ complex formed at 580 nm is given 7.0x10^3 L/cm.mol. Which of the following values is the absorbance of this solution as measured with a 2.0 cm cell? Fe:56 A. 0.168 B. 0042 C. 0,084 D. 0.126A student measures k for a certain blue dye to be 600.4 M-¹ at 560 nm. What is the molarity of the dye in a solution with an absorbance of 0.204 at this wavelength? Ens nousior #inslo: Monia sin 8 foi 00.01 Par det id elsem. sow & netimuloa 51 (5) sonos silf et trawIm 00 001 et gauzulib im
- The max of aspirin (molar mass 180g/mol) in neutral solution is 225 nm and & is 650 mol-¹Lcm ¹. An absorbance of 1.80 was measured for a solution of aspirin, with a 1 cm path length. Calculate the concentration of the aspirin solution.4. Calculate the expected absorbance of solution of a 5.50x10-6 M solution of Blue # measured at 629 nm in a 1.50cm cell. The molar absorptivity for Blue #1 is 1.30x105 M-1.cm-1 at 629 nm.Estimate the Ka of a weak acid from the data given below. One gram quantities of the acid were dissolved in equal quantities of the various buffer solutions and all solutions were measured under the same conditions. The anion of the acid is the only species that absorbs at the wavelength used. pH: Abs: 4 0.0 5 0.0 6 0.06 7 0.39 8 0.95 9 1.13 10 11 1.18 1.18
- 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/L8:A 75mL sample of water is titrated with 0.100M EDTA. exactly 16.9mL of EDTA are required to reach the EBT endpoint. calculate the total hardness in ppm CACO3 a) 2.253 ppm O 0.030 x 10^3 ppm. c) 0.02534 ppm O d) 2.253 x 10^3 ppmFe+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?