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- An active ingredient has a relative molecular mass of 498. What mass of this active ingredient is required to make up 345 cm3 of a solution with a concentration of 0.03 mol dm−3? Give your answer in grams and approximate to 2dp:A spectrophotometric method for the quantitative analysis of Pb2+ in blood has a normal calibration curve for which Sstd=(0.296 ppb−1)×Cstd+0.003. What is the concentration of Pb2+ in a sample of blood if Ssamp is 0.397?What is the molar extinction coefficient at 625 nm for this copper (II) acetate solution? How was it determined? Standard Solution Concentration (M) Absorbance 1 0.025 0.049 2 0.050 0.153 3 0.100 0.242 4 0.200 0.499 5 0.250 0.694
- The acid-base indicator HIn undergoes the following reaction in dilute aqueous solution: HIncolor1H++Incolor2 The following absorbance data were obtained for a 5.00 I0-4 M solution of HIn in 0.1 M NaOH and 0.1 M HC1. Measurements were made at wavelengths of 485 nm and 625 nm with 1.00-cm cells. 0.1 M NaOH A485 = 0.075 A625 = 0.904 0.1 M HC1 A485 = 0.487 A625 = 0.181 In the NaOH solution, essentially all of the indicator is present as In-; in the acidic solution, it is essentially all in the form of HIn. (a) Calculate molar absorptivities for In- and HIn at 485 and 625 nm. (b) Calculate the acid dissociation constant for the indicator ¡fa pH 5.00 buffer containing a small amount of the indicator exhibits an absorbance of 0.567 at 485 nm and 0.395 at 625 nm (1.00-cm cells). (c) What is the pH of a solution containing a small amount of the indicator that exhibits an absorbance of0.492 at 485 nm and 0.245 at 635 nm (1.00-cm cells)? (d) A 25.00-mL aliquot of a solution of purified weak organic acid HX required exactly 24.20 mL of a standard solution of a strong base to reach a phenolphthalein end point. When exactly 12.10 mL of the base was added to a second 25.00-mL aliquot of the acid, which contained a small amount of the Indicator under consideration, the absorbance was found to be 0.333 at 485 nm and 0.655 at 625 nm (1.00-cmcells). Calculate the pH of the solution and Ka for the weak acid. (e) What would be the absorbance of a solution at 485 and 625 nm (1.50-cm cells) that was 2.00 10-4 M in the indicator and was buffered to a pH of 6.000?Construct the expression for Ksp for solid BiI₃ in aqueous solution. BiI₃(s) ⇌ Bi³⁺(aq) + 3 I⁻(aq)The Ksp of Al(OH)3 (MM: 78) is 1.90 xx 10^(-33). a) What is the molar solubility of Al(OH)3?
- The Ksp of Al(OH)3 (MM: 78) is 1.90 xx 10^(-33). a) What is the solubility of Al(OH)3 in g/L?A compound X is to be determined by UV/visible spectrophotometry. A calibration curve is constructed from standard solutions of X with the following results: - 0.50 ppm, A = 0.24;- 1.5 ppm, A = 0.36;- 2.5 ppm, A = 0.44;- 3.5 ppm, A = 0.59; and- 4.5 ppm, A = 0.70. Find the following:A. Slope and intercept of the calibration curveB. The mean concentration of the solution of unknown X concentration if the absorbance of 3 replicates are A = 0.29, A = 0.30 and A = 0.32.C. The standard deviation in the concentration of XSolid Na2S is slowly added to a solution of 1.0 x 10-3 M Cr3+ (with no change in volume). At what [S2-] will Cr2S3 start to ppt? For Cr2S3, Ksp = 1.0 x 10-20
- A second spectrophotometric method for the quantitative analysis of Pb2+ in blood yields an Ssamp of 0.712 for a 5.00 mL sample of blood. After spiking the blood sample with 5.00 μL of a 1560 ppb Pb2+ external standard, an Sspike of 1.546 is measured. What is the concentration of Pb2+ in the original sample of blood?The calibration curve y=0.0218x - 0.0001 for Fe2+ in buffer at 450 nm in a 0.5 cm cuvette. Is Beer's Law obeyed? Explain. and What is the molar extinction coefficient for the Fe2+ complex at 450 nm?Concentration=2.5 X 10^3 μM OD400nm=0.859 1cm cuvette is used what is the extinction coefficient (μM^-1 cm^-1)
