In lab, your spectrophotometer has a maximum detection limit of 1.1 M. The solution you want to measure has a concentration of 3 M, so you measure out 33 mL and dilute it to 259.2 mL. What is the final concentration of your solution?
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In lab, your spectrophotometer has a maximum detection limit of 1.1 M. The solution you want to measure has a concentration of 3 M, so you measure out 33 mL and dilute it to 259.2 mL. What is the final concentration of your solution?
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- The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μLμL of the sample and injecting it into a cuvette already containing 2.00 mLmL of water (total volume is 2.00 mLmL + 100.0 μLμL). The absorbance value of the diluted solution corresponded to a concentration of 7.71×10−6 M M . What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units.The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL�L of the sample and injecting it into a cuvette already containing 2.00 mLmL of water (total volume is 2.00 mLmL + 100.0 μL�L). The absorbance value of the diluted solution corresponded to a concentration of 6.22×10−6 M � . What was the concentration of the original solution?Please answer this question as fast as you can please and tahnk you. I will afterwards write an wonderful review on solving the question. Thank you. You determined experimentally the density of a solution in triplicate. Considering the results what is the standard deviation of your results? Answer your question with the correct number of significant figures. The answer should be in units of g/mL Trial 1: 0.9991 g/mL Trial 2: 0.9984 g/mL Trial 3: 0.9996 g/mL
- After creating her standard curve for absorption versus the concentration (M) of FD&C Red 40 and processing her data, Sally found that her drinking strength Kool-Aid sample had a concentration of 4.692 x 10–5 M. If 0.132 grams of Kool-Aid powder was used to prepare an 8-fl oz cup of her assigned flavor, what is the percent by mass of FD&C Red 40 in her Kool-aid powder? Report your answer as a percentage with two places after the decimal. Do not include the percentage sign in your answer. Pay attention to units. You are trying to find the mass percentage of red dye, so you need to know each variable in the equation in Appendix B. Note that the percent by mass equation should be multiplied by 100. There may be some useful conversion factors in the experimental procedure.f the tolerance of a 50 mL Burette is \pm 0.05 mL, which of the following would not be acceptable readings to record? 9.3 mL 43.02 ml. 22.3 mL 0.65 mL 52.45 mL 30.07 mL 15.30 mL 36.55The color change of a chemical requires an overtitration of 0.04 mL. Calculate the percent relative error if the total volume of the titrant is 50 mL.
- Find the true mass of 28.0 wt% ammonia (density = 0.90 g/mL) when the apparent mass is 20.000 g.Student A got the following densities of water; 1.09g/mL, 1.14g/mL, and 1.15g/mL with an average of 1.127 g/mL and a standard deviation of 0.026 g/mL. Student B determined the density of water to be 1.04 ± 0.05 g/mL. Determine the acceptable range of mass when you are asked to obtain 3.000g of NaCl.1. What is a spectrophotometer used for in a cobalt chloride solution analysis?
- During a titration experiment, 50.00 mL of a certain solution needs to be transferred to an Erlenmeyer flask. To measure the volume, a student used a calibrated 10-mL pipette five times. If the pipette delivers an actual volume of 9.98 mL with an uncertainty of ±0.02 mL, what will be the uncertainty in the final volume?pls complete the 2nd table given the data1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)Julie has been asked to measure the concentration of a sample solution using a spectrophotometer. After a first attempt, she realizes that, to make the measurement, she must first dilute the sample solution. Julie transfers 2.3 mL2.3 mL of the sample to a 250 mL250 mL volumetric flask and fills the rest of the flask with water to the 250 mL250 mL line. She then uses the spectrophotometer to measure the concentration of the dilute solution as 5.5×10−5 M.5.5×10−5 M. What is the concentration of the starting sample solution? sample solution concentration: M