A standard curve for a compound was created with a series of standards, and is shown below. If an unknown produced an absorbance of 0.279, what was the concentration of the compound? Absorbance 0.6 0.5 0.4 0.3 0.2 0.1 Standard Curve for Comound A 0 -0.1 0 10 20 30 Conc. A (ppm) 40 y = 0.0104x -0.0044 R² = 0.9947 50 60

em1.png Part 3: Q9 Average absorbance Flask 8 Flask 9 Flask 10 1:1 Ratio so, Flask 11 Part 3: Q Flask 8 Flask 9 Flask 10 Flask 11 Part 3: Q10 Flask 8 Flask 9 Flask 10 Flask 11 Part 3 0.146 0.166 [Fe] -0.002mol/L 0.215 0.294 [FESCN³mol/L) 4.59% 10 5.18*10* 6.64*10* 9.08*10* [FXmol/L) 5.00 *10* 5.00*10* Y=3362x-0.0083 R² = 0.9993 5.00*10* 5.00*10* (Amounts of flask 8 (9 - 11's values are in the spreadsheet) 71% volume 5.00mL Molarity of Fe(NO3))3 = 0.2M Volume of Fe(NO3))3 = 5.00mL Moles of Fe³= Molarity x volume(L) Moles of Fe¹ = 0.2M X 0.005L = 1x10-³mole x [SCN][mol/ 4x10 5×10-4 7x10 1×10 1 Concentration of Fe³ = mole of Fe³ Volume mole of Fe³1x10³ mole G.O05L 8, Average absorbance for solution 8 (same for 9 - 11) Average absorbance for flask 8 = sum of all absorbances / number of readings (0.145 +0.147 +0.148) 3 Using equation of calibration curve's line(slope) of best fit, the average absorbances of the unknown concentrations to determine [FeSCN-Jat equilibrium in solution 8:…

How do I find the theoretical molarity?

Chemistry

Suppose that a solution has an absorbance of 0.250 at a wavelength of 450 nm.  If the concentration of the solution is 22 μM, what is the value of the molar absorptivity?  The data were taken with a standard 1-cm cuvette. molar absorptivity in (L cm^−1 mol^-1):

A standard containing 20 mg/mL of compound P is placed in a 1 cm cuvette. The absorbance of the standard is 1.20 at 600 nm.  A sample containing Compound P has an absorbance of 0.50.  What is the concentration of this sample?

A medical lab technician creates a standard solutions of percent hemoglobin in whole blood. The technician measures the absorbance of each solution at 520 nm and creates a standard curve of the absorbance versus percent hemoglobin in whole blood and finds the linear equation below, with an R2 of 0.9985. y = 0.0523 x + 0.072 A patient sample has an absorbance of 0.162. Using the standard curve data, calculate the percent hemoglobin in the patient sample

How would I do 2? the concentration iron is 1.85mg/vitamin tablet, and the absorbance at 508nm is 0.37

A colored ion solution has a concentration of 0.200 M with a measured absorbance A = 0.880. Another ion solution made of the same chemicals has an absorbance A = 0.172. What is the concentration of this unknown sample solution?

Can you help me on questions 2 AND 3