45.0 mL of an unknown FeCl3 solution is diluted to a total volume of 230.0 mL. The diluted FeCl3 solution measured an absorbance of 0.223. Calculate the molarity of the undiluted unknown FeCl3 solution if the molar extinction coefficient is 230.0 M-1⋅cm-1 and a path length of 1.00 cm. Group of answer choices 0.000190 M 0.00496 M 0.00593 M 10.0 M 0.00399 M
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- 45.0 mL of an unknown FeCl3 solution is diluted to a total volume of 230.0 mL. The diluted FeCl3 solution measured an absorbance of 0.223. Calculate the molarity of the undiluted unknown FeCl3 solution if the molar extinction coefficient is 230.0 M-1⋅cm-1 and a path length of 1.00 cm.An unknown sample of Cu2+gave an absorbance of 0.262. Then 1.00 mL of solution containing 100 ppm (ug/mL)Cu2+was mixed with 95.0 mL of the unknown and the mixture was diluted to 100 mL in a volumetric flask with deionized water. The absorbanceof the new solution was 0.500. a.Denoting the initial unknown concentrationas [Cu2+]i,write an expression for the final concentrationafter dilution [Cu2+] b.Find [Cu2+]in the unknown.A solution of a dye with an absorptivity coefficient (ε) of 3.75 x 102 M-1cm-1 had an absorbance of 0.039 measured in a cell whose width is 1.00 cm. What is the concentration of the dye in the solution? a. 1.46 x 10-3 M b. 1.04 x 100 M c. 1.04 x 10-4 M d. 1.46 x 101 M
- 1) Titrant 5 mg H2O/ mL Resolution 2.5 µg H2O/step Detection limit is 125 µg H2O for a 5 g sample (= 25 ppm) 2) Titrant 2 mg H2O/ mL Resolution 1 µg H2O/step Detection limit is 50 µg H2O for a 5 g sample (= 10 ppm) You have a 10 g sample which is expected to contain 200 µg H2O. True or false? 1. Titrant 5mg/mL is the preferred system over 2. Titrant 2mg/mL for this sample. True FalsePreparing a standard curve. 1. determine the absorbance max of [FeSCN]2+ it is 448.1 2. determine the concentration of FeSCN2+ in the stock solution. M1V1=M2V2 stock solution: ~0.200 M iron (iii) nitrate in 1M nitric acid intial volume: 0.3mL final volume: 10.3mL volume: 10mL ~0.002M potassium thiocyanate initial volume: 0.3mL final volume: 10.3mL volume: 10mL not sure if this is needed stock solutions: ~0.200M iron (iii) nitrate in 1M nitric acid: 0.207M ~0.002M iron (iii) nitrate in 1M nitric acid: 0.00209M ~0.002M potassium thiocyanate: 0.00193MQuinine in a 1.664 g antimalarial tablet was dissolved in sufficient 0.10 M HCl to give 500 mL of solution. A 15.00 mL aliquot was then diluted to 100.0 mL with the acid. The fluorescense intensity for the diluted sample at 347.5 nm provided a reading of 288 on an arbitrary scale. A standard 100 ppm quinine solution registered 180 when measured under conditions identical to those for the diluted sample. Calculate the mass in milligrams of quinine in the tablet.
- 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 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq): Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.A water sample is approximated to have a total hardness equal to 120.0ppm. How many milliliters of 0.01000N EDTA will be needed to titrate 250.00mL of the said water sample?(MM CaCO3=100.09g/mol). ** Need asap pls. Thanks.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?
- Absorbance measurements were taken on a series of Fe standards complexed with 1,10-phenanthroline. A plot of absorbance vs. concentration yielded a linear curve with the equation y=1.008e03x + 0.0395 (where y is the absorbance and x represents the Fe concentration in moles/L). Using this information calculate the Fe concentration (in ppm) in a 40.0-mL aliquot of ground water that produced an absorbance of 0.580.Ben ran through the experiment and found the best-fit line listed below for his standard calibration curve of absorbance vs concentration in M. y = 3214.0x + 0.0076 Ben then prepared a solution that had 5.00 mL 0.002 M iron(III) nitrate in 1 M nitric acid, 3.00 mL 0.002 M potassium thiocyanate, and 2.00 mL DI water. If the absorbance for the solution was 0.436, calculate the equilibrium concentration of iron(III) thiocyanate in the solution. Report your answer in mM with three places after the decimal.Following AAS analysis, a graph of absorbance versus ppm nickel standard gave a best-fit line y = 0.0428x + 0.0487 . Calculate the ppm nickel in the well water sample having an absorbance of 0.675. 0.13 15.91 0.08 14.60