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- When 0.2 millimoles of Y are dissolved in 250 ml of water, the resultant solution has an absorbance of 1.6. What is the molar extinction coefficient of Y?How many moles of Nal would be found in 250mL of a 4.5 M solution? Write your answer with three digits beyond the decimal point (IMPORTANT - zeroes count as a digit) The answer is molesIf your 16x concentrated stock solution contains 20g of NaCl per liter, how much Nacl would one liter of your working solution contain? Round your result to 2 decimal points. g of Nacl
- You wish to determine the %concentration of a stock solution of brilliant blue FCF (MW=792.8grams/mole; extinction coefficient,25=97000M1cm 1). You take 5ul of the stock and dilute up to 1ml. You take 10ul of this dilution an dilute it up to 500ul. Finally you take 1ul from this dilution and dilute it up to 1ml in a 1cm diameter cuvette. You obtain an As91=0.001 SHOW YOUR WORK. Do not forget units. 1. What is your total dilution factor? 2. What is the molar concentration of the dye in the original stock? 3. What is the % concentration of the dye in the original stock?Use excel to plot the following titration data. Once you have done your plot, make sure to label the axes correctly. Use your graph to determine the pKa for the weak acid. Attach your plot to the back of this worksheet. A 1.0M solution of weak acid was titrated with a base and the following data was collected. Equivalents of Base pH observed 3.4 3.9 4.2 4.5 4.9 5.2 me 0.05 0.15 0.25 0.40 0.60 0.75 0.85 0.95 BANGir 5.4 6.0Guanosine (C10H13N5O5) in solution has a maximum absorbance at a wavelength of 275 nm. The molar extinction co-efficient at this wavelength is 84M−1cm−1and the path length is 24.7 cm. Through the use of a spectrophotometer, it is found that the that A275= 1.48. What is the concentration of the guanosine solution in grams/litre? Molecular weights (g/mol): C-12, H-1, N-14, O-16 Select one: A. 0.201869 g/L B. 0.435188 g/L C. 0.059919 g/L D. 0.294046 g/L E. 0.000713 g/L
- A saline solution contains 1.00 g of NaCl (molar mass = 58.55 g/mol) in 75.8 mL of solution. Calculate the concentration of NaCl in this solution, in units of molarity. %3D Express the concentration in molarity to three significant figures. ? MThis is a question regarding spectrophotometry. Scenario: 0.1 mL of the unknown and 0.9 mL of distilled water are mixed in a cuvette and the absorbance is measured at 280 nm. Given the absorbance, molecular mass and the extinction coefficient of the unknown are 0.253, 16950 g and 13940 M-1cm-1 respectively, and the path length is 1 cm, how can I find the concentration of the unknown in mg/mL by Beer-Lambert Law (NOT molarity M)?How much index [18] embalming fluid would you need to mix with 15oz of an index [10] embalming fluid to create N 256 OZ. [4.5] embalming solution Answer Choices: 1. 55.67 oz 2. 67.55 oz 3.372.0 oz 4. 4.2 oz
- A beaker with 1.40x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.00 mL of a 0.490 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( - ) sign if the pH has decreased. View Available Hint(s) ΑΣφ ApH =Lab Data Verify your concentration calculation. Did you report your data to the correct number of significant figures? Stock solution Concentration iron(III) nitrate 0.40000 [Fe(NO3)a] (M) Color of iron(III) nitrate yellow Concentration potassium thiocyanate [KSCN] (M) 0.00300 Color of potassium thiocyanate colorless Volume iron(III) nitrate (mL) 10.00 Volume potassium thiocyanate (mL) 2.00 Volume DI water (mL) 8.00 Concentration iron(III) thiocyanate ion in stock solution [FESCN2"] (M) 0.000300 Color of stock solution red-orange Diluted solutions Solution 1 Solution 2 Solution 3 Volume stock solution (mL) 4.00 4.00 4.00 Volume DI water (mL) 1.00 2.00 3.00 Concentration iron(III) thiocyanate ion [FeSCN2*] (M)The calibration curve shown below was used to analyze an unknown protein solution. What is the concentration of the unknown solution, if the absorbance of the unknown is 0.505? Answer in ug/mL. 1.2 y%3D0.005x+0.061 R=0.992 0.8 0.6 0.4 0.2 50 100 150 200 250 Concentration ug/ml Absorbance