Andrew Li 101258492 Fe short report, TA-Maram Bakiro, 11-03-22 (1)

1. How would you find the solution for this dilution and absorbance problem? What would the set-up for solving this look like? (A = 0.0252C(ppm) - 0.0162)

How do I complete this problem?

How do I find Concentration? flask Calculate solution Concentration (M) Volume stock of 0.40 M CuSO4 (ml) Volume of flask (ml) Absorbance at 635 nm(a.u.) 1   2.0 10 .185 2   4.0 10 .362 3   6.0 10 .510 4   8.0 10 .674 5   10.0 10 .843

Answer provided: 2.5% Al2(SO4)3 Please show your complete solution and write your answer clearly and readable. Thank you.

Find #4 and #7

I need help please!!

(Solution AII) Prepare 25.00 mL of ~0.05000 M copper (II) acetate solution from your ~ 0.1250 M solution. Pipet the required amount of solution (AI) into a 25.00 mL volumetric flask. Fill it to the mark with distilled water, stopper it and invert several times to mix the solution. Measure the absorbance of this solution at a wavelength of 610 nm, the wavelength where this compound absorbs light most strongly. (e = 5.97 dm3/mol cm) Calculate molarity of solution AII Volume of stock solution AI added via pipette

Suppose that you follow the procedure and find the absorbance of the final solution to be 0.475.  What is the concentration of Fe (mg/L) in the final solution?

calculate the [FESCN2+] using volumes of stock solutions. Presume that all of the SCN- ions react. Next, record the light absorbance values of each standard solution. Volume Volume Volume [FESCN2+] Absorbance Standard Fe(NO3)3 SCN- H2O sample (mL) (mL) (mL) 1 2.50 2.00 20.50 0.1811 2 2.50 1.50 21.00 0.3219 2.50 1.00 21.50 0.4981 4 2.50 0.50 22.00 0.6328 Stock [Fe(NO3)3] = 0.200 M, Stock [SCN-] = 0.0020 M. %3D

and l x + zakeAssignment/takeCovalentActivity.do?locator-assignment-take X A copy of your chemistry textbook is found to have a mass of 2.52 x 10³ grams. Using unit analysis, show what the mass of the copy of your chemistry textbook is in milligrams. Use one of the following to set up the conversion factor. 1 kg 1000 g 1000 mL-1 L 100 cm=1 m 1000 mg=1 g 1 mL=1 cm³ 1000 mm=1m 3 2.52 x 10³ g x 80 F3 E D Submit Answer C $ 4 888 F4 R F (number) (unit) [Review Topics] [References] Use the References to access important values if needed for this question. (number) (unit) % 5 V Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support 29 F5 T G A 6 B MacBook Air F6 mg Y H & 7 N 44 F7 U J * 00 8 DII F8 I M K ( 9 DD F9 O . { Previous [ 11 4G Next> Save and Exit 4)) F12 } * O 1 delete MIT ¡ ? Silift

1. Data & Results 4.0 mglmL Concentration of stock solution (include units): Table 1-Beer's Law Plot Data V Volume of standard solution dispensed (mL) M, Diluted concentration (include units) Sample Absorbance A 2.00 mL 0.084 4.00 mL 0.173 l6.00 mL 0.259 8.00 mL 0.340 E 10.00 mL 0.418 Equation of trendline from Beer's Law plot: whats the diluted concentration and equation of trendline from the beers law plot once created?

Part Il: Determination of Standard Solutions mL of 0.200 mL H20 added M Cuso, diluted Tube # M Cuso4-5 H20 added Absorbance about 3 0.200 1.346 3. 4.00 1.00 0.945 4 3.00 2.00 0.715 2.00 3.00 0.469 6. 1.00 4.00 0.281 show calculation for Tube #3 diluted concentration:

AP Questions // Questions 10 - 11) A student creates four solutions with varying concentration of FeSCN2 and gathers the following data at 298 K using a spectrophotometer calibrated to 460 nm: [FESCN] Absorbance 1.1 x 10-4 M 0.076 1.6 x 10-4 M 0.112 2.2 x 10-4 M 0.167 2.5 x 10-4 M 0.199 On the axis below, create a Beer's Law calibration plot for [FESCN2*]. Draw a best-fit line through your data points.

Please answer the question correctly is all I want and explain why its thats answer for the final and please answer as quickly as possible, thanks! 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 absorbance of a 80 mmol/L solution of the metal at 400 nm?

Please help me find the concentration of each standard solution in the v-flask, and prepare a curve.     The solution was diluted with ddH2O.

Absorbance Beer-Lambert's Law (Spectrophotometry) #2 To spectrophotometrically determine the mass percent of cobalt in an ore containing cobalt and some inert materials, solutions with known [Co"] are prepared and the absorbance of each of the solutions is measured at the wavelength of optimum absorbance. The data are used to create a calibration plot, shown below. 0.80 0.70- 8 0.60- 0.50- 0.40- 0.30 0.20- 0.10- ++- 0.015 Concentration (M) A 0.6 g sample of the ore is completely dissolved in concentrated HNO3(aq). The mixture is diluted with 2+ water to a final volume of 50.00 mL. Assume that all the cobalt in the ore sample is converted to Co'(aq). a. What is the (Co] in the solution if the absorbance of a sample of the solution is 0.74? b. Calculate the number of moles of CoT(ag) in the 50.00 mL solution. 2+ C. Calculate the mass percent of Co in the 0.630 g sample of the ore.

Table 2: Absorbance Values of Standards and Unknowns. Sample Blank Standard Solution 1 Standard Solution 2 Standard Solution 3 Standard Solution 4 Standard Solution 5 Water Sample 1 Water Sample 2 Phosphate Concentration (in ppm) Y17 0 ppm 0.02 ppm 0.04 ppm 0.08 ppm 0.16 ppm 0.32 ppm Freeman Lake 0.001 0.325 0.292 0.413 0.315 0.039 0.054 0.049 Absorbance at 2= 690 nm Calculations: 1. Construct a phosphate standard curve in Excel by plotting concentration (in ppm) on your x-axis and Absorbance (unitless) on your y-axis for your known solutions. Label the axes on the graph and provide the curve with a title. Use a linear trendline to generate a best fit line to your data. Label the graph with the equation and the R" value. Insert your labeled graph in the space below. X

A student is given an antacid tablet that weighed 5.6832g. The tablet was crushed and 4.3628g of the antacid was added to 200 mL of stimulated stomach acid. This was allowed to react and then filtered. It was found that 25 mL of this partially neutralized stomach acid required 8.50 mL of NAOH solution to titrations it to a methyl red endpoint. It took 21.54 mL of this NAOH solution to neutralize 25 mL of the original stomach acid.  a)How much of the stomach acid had been neutralized in the 25 mL sample which was titrations? (Show work) B) how much stomach acid was neutralized by the 4.3628 g sample used? (Show work)  C)How much stomach acid would have been neutralized by the original 5.6832 g tablet? (Show work)

Solid residue weighing 7.158 g from an aluminum refining process was dissolved in acid to give Al3+ in solution. The solution was treated with 8-hydroxyquinoline to precipitate (8-hydroxyquinoline)3Al (FM 462.462 g/mol), which was ignited to give Al2O3 (FM 101.961 g/mol) weighing 1.178 g.  Find the weight percent of Al (FM 26.982 g/mol) in the original mixture.

Limestone consists mainly of the mineral calcite, CaCO3 (FM 100.09 g/mol). The carbonate content of 0.6070 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO₂: CaCO3 + 2 H+ Ca²+ + H₂O + CO₂t The excess acid required 33.15 mL of 0.1317 M NaOH for complete titration to a phenolphthalein end point. H+ + OH H₂O Find the weight percent of calcite, CaCO3 (FM 100.09 g/mol), in limestone.

The following absorbance values for four solutions with known MnO4 concentrations were measured using a spectrophotometer: Solution 1 2 3 4 [MnO4] 0.700 x 104 M 1.00 x 104 M 2.00 x 104 M 3.50 x 104 M Absorbance 0.175 0.250 0.500 0.875 A. Using Microsoft Excel, plot a graph of Absorbance vs. Concentration of MnO4. Write the trendline linear equation from the plotted graph. B. Determine the slope of the graph and include its units. C. Determine the concentration of an unknown MnO4 sample whose absorbance is 0.780.

A sample of a sports drink containing the dye was assayed using the prescribed method and found to have an absorbance of 0.398AU. Using the equation of the best fit line, determine the concentration of the dye in the drink. trendline equation: y=0.029x - 0.026

Caffeine (C8H10O2N4 • H2O) has an absorbance of 0.510 at 272 nm and 1 cm optical path in1 mg / 100 mL concentration solutions. A 2.5 g sample of soluble coffee is diluted withwater to 500 mL. Take 250 mL, add 25.0 mL of 0.1 N H2SO4 and dilute it to 500 mL. Theabsorbance at 272 nm resulting in 0.415. A) Calculate the grams of caffeine per kg of soluble coffee in the sample. Themolar mass of caffeine is 212 g / mol.

Do not give handwriting solution.

The nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO2 (46 g/mol) and the molarity of NaNO2 (69 g/mol) in the original sample

The thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg2+ via the reaction. Calculate the percent (NH2)2CS (76.12 g/mol) in the sample. 4 (NH2)2CS + Hg2+ →  [(NH2)2CS]4Hg2+