Lab 5 REPORT FORM_F22_V2

given the following results " create a “standard curve” (a graph) that shows the concentration on the x-axis and the absorbance on the y-axis" and "a solution of copper(II) sulphate with an unknown concentration was found to have an absorbance of 0.09. Use your standard curve to determine its concentration" ample Number Concentration of Copper(II) Sulphate (mM) Measured Absorbance 1 0   0 2 50   0.12 3 100 0.24   4 150   0.35 5 200   0.47 Unknown   40 0.09

Table II Cuvette # Concentration Absorbance 0.50 M 1 1.049 2 0.40 M 0.926 3 0.20 M 0.740 0.298 4 0.10 M 5 0.05 M 0.202 Unknown # 9 0.427 Unknown # 10 7 0.646 Blank (DI water) 0 1. If Beer's Law is valid, the value of "E" should be constant. Use A = E*C*L or E= A/(E*L) and the data from Table II to calculate values of E for the five solutions below The value of L is normally 1 cm so E = A/C in this experiment. Table III Solution # Calculated Values of E 1 2 3 4 5

Using the data below, please create a calibration graph and determine the concentration of the unknown sample. Standard #1 Standard #2 Standard #3 Unknown sample Concentration 1.5 x 10 M 2.0 x 103 M 2.5 x 10 M ? Absorbance 0.61 0.80 0.98 0.72 a) 1.6 x 10 M b) 1.8 x 10° M c) 2.1 x 103M d) 2.2 x 10 M

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The first photo is the data, second photo is the question! thank you!

PART ONE: Preparation of FECNS* Solution Prepare the two solutions in table 1 by accurately measuring the required volumes of distilled water and CNS into two labeled test tubes. The absorbance of the solutions must be measured soon after adding the Fe" solution from a buret. TABLE 1 Fe 5 ml 5S mL Solution Distilled Water CNS 2 mL Total Volume 3 ml 2 ml 10 ml 3 mL 10 ml In this part of the experiment you are to explore what the above quote means. As a PRELIMINARY Exercise, formulate a hypothesis as to what would happen under each of the following circumstances: 1. 1ml of 0.0020 M CNS' solution is added to the unused portion of solution 1 in the test tube 2. One drop of 0.20 M CNS solution is added to the unused portion of solution 2 in the test tube.

1. Given the following values, use the absorbance formula to find the     hemoglobin concentration of the unknown.   As =0.600 Au =0.300 Cs =20g/dl   2. Convert 12.8 g Hb into percent Hb   3. Compute the grams Hb of 88% Hb.

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If A=absorbance, B=molar absorptivity, C=length of light path, D=concentration, and you plot a graph of absorbance (y-axis) vs concentration (x-axis), what does the slope of the Beer's Law (A=BCD) curve signify? Choose one:  a. absorbance b. molar absorptivity c. length of light path d. concentration

10 Use contrastive analysis to think about how the following conversion might be done. Then write the steps required for the following conversion to take place -Br

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.

+3 +2 Na MgO Li +1 Ca N -1 SF Al Br -2 H -3 Reset Help

4. You prepare several dilutions of an unknown compound. You measure the absorbance of each solution at 340 nm using a 1 cm cuvette (your results are listed in the table below). What is the extinction coefficient (in (M•cm)') of the compound? (Hint: assume that each of the individual values contains some degree of experimental error.) Concentration(uM) Absorbance at 340 nm 10.0 0.011 20.0 0.023 40.0 0.066 80.0 0.119 160.0 0.189

Given this data, if a CV solution has an absorbance of 1.125, what is [CV]? [CV] / M              A  1.0 × 10–6 M      0.250 3.0 × 10–6 M      0.750     Question 12 options:   4.5 × 10–6 M   5.0 × 10–6 M   5.5 × 10–6 M

Based on the data in the table, summarize what was shown here, what did they do here? And was this lab successful or not?     Substance  Physical Appearance Odor Density (g/mL) Reacts with NaHCO3 1.      Benzaldehyde  Clear liquid or almost pale yellow It smelled like almonds  1.00 No, significant reaction 2.      MTBE Colorless  Fruity smell to it 1.236 -1.247  No chemical reaction occurred 3.      Urea White solid  A very strong order of ammonia  0.791 No reaction occurred   4.       Acetone Colorless Pungent odor like nail polish remover 1.335 No, did not react with sodium bicarbonate 5.      Glycerol Colorless N/O 1.044 No, it did not cause a reaction 6.      Citric Acid colorless then turns white with sodium bicarbonate added N/O 1.044 Yes, caused fizzy/bubbles to it.

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QUESTION 13 Analysis of an Iron Complex In part C of this experiment, the iron content of the iron complex is determined by first converting it to a tris(bipyridine)iron(II) complex ion, and measuring its absorbance with a spectrophotometer. Which of the following correctly describes the relationship between the absorbance of a solution and its concentration? Preparation & Analysis of Iron Complex.pdf O A. The relationship between absorbance of light by a solution and its concentration should be exponential so that when concentration increases, absorbance increases exponentially. O B. The relationship between absorbance of light by a solution and its concentration should be inverse so that when concentration increases, absorbance decreases. OC. The relationship between absorbance of light by a solution and its concentration should be linear so that when concentration increases, absorbance increases. OD. The relationship between absorbance of light by a solution and its concentration…

(Single Standard addition) Vitamin C was measured by an electrochemical method in a 50.0 mL sample of lemon juice. A detector signal of 2.02 μA was observed. A standard  addition of 1.00 mL of 29.4 mM Vitamin C increased the signal to 3.79 μA.    Find the concentration of Vitamin C in the juice.

I need answers for # 2-9 on this worksheet

You begin preparation of the calibration curve to measure absorbance vs concentration of FeSCN²+. To do so, you add 1.58 mL of 0.200 M Fe(NO3)3 to a cuvette and then directly add 316 µL of 0.001 M KSCN. What is the resulting concentration of FeSCN2+, assuming complete conversion of SCN´¯ to FeSCN²+´ Enter your answer in units of mM to four digits after the decimal.

how do i find the absolute and relative uncertainty of my data?

Calculate the concentration in ppm of Cd in a 2.00 mL sample which has been shown to contain 16.4 μg Cd. Assume the sample has a density of 1.00 g/mL. Show your work for full credits (just explain step by step and put the answer at the end)

1. A student performed this experiment and obtained the following concentration values: 0.02813 M, 0.02802, and 0.02788 M a. what is the mean concentration? b. what is the standard deviation of these results? 3. how would the following errors affect the concentration of Cl- obtained in question 2b? give your reasoning in each case. a. the student read the molarity of AgNo3 as 0.02104M instead of 0.02014M b. the student was past the endpoint of titration when he took the final buret reading.

For the following questions (Q1-Q5), consider the compound tartrazine (Yellow 5 food dye) that has a chemical formula of C16H9N4Na3O9S2. Ana weighs out 0.1328 g of tartrazine powder on the balance for her experiment and makes a stock solution by dissolving her powder in 500.0 mL of solution.     Concentration (µM or µmol/L) Absorbance 0.00 0.001 9.94 0.252 19.9 0.506 29.8 0.738 39.8 1.018   slope (m): 0.02534 1/(µM) y-intercept (b): -0.0009147   Q4. Calculate the molar extinction coefficient (molar absorptivity) of tartrazine in units of 1/(M·cm). Assume a cuvette path length of 1.00 cm.

For the following questions (Q1-Q5), consider the compound tartrazine (Yellow 5 food dye) that has a chemical formula of C16H9N4Na3O9S2. Ana weighs out 0.1328 g of tartrazine powder on the balance for her experiment and makes a stock solution by dissolving her powder in 500.0 mL of solution.     Concentration (µM or µmol/L) Absorbance 0.00 0.001 9.94 0.252 19.9 0.506 29.8 0.738 39.8 1.018   slope (m): 0.02534 1/(µM) y-intercept (b): -0.0009147   Q5. If Ana determines the absorbance of an unknown tartrazine sample to be 0.662, what is the concentration of the sample in µM?

To run a spectrophotometry experiment, begin by warming up the spectrophotometer and preparing the samples. Be sure to select the correct absorbance (X), then run a measurement on the sample solution. Follow up by running measurements on sample solutions. Once data is collected, turn off the instrument, clean the area, and discard the samples. Partially correct (2 of 4 correct)

Table 2   Absorbance vs CoCl2 concentration   Test Tube Number Cobalt Chloride Concentration    (mol/mL) Absorbance at 510 nm       1 0.000 0.000 2 0.009 0.024 3 0.018 0.055 4 0.027 0.085 5 6 0.036 0.045 0.112 0.138   7   (Unknown)   0.088   explain the results of this experiment and find the unknown concentration

The concentration of green dye in green apple Gatorade was determined in a manner identical to experiment 3.The slope of the Beer lambast law plot (calibration curve) for this dye (FD & C Green 3 or fast green) was determined to be 53.7 L/g cm (assume the intercept of the beer lambast law plot is zero)what is the concentration,in units of g/L,of the green dye in the sample of Green Apple Gatorade with an absorbance of 0.369?In three significant figures

Supply the missing information in the table. (Given in Blue). Answers in scientific notation should be in this sample format >>> 1.0 x 10-14

please highlight the correct answer