Mass of aspirin used is .090 g the absorbance for the final solution was .304 nm Slope is 1708 and y-intercept is -0.03397 what is the molarity of the final unknown solution and the molarity of the original solution made from aspirin in the 250.0 ml flask
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Mass of aspirin used is .090 g
the absorbance for the final solution was .304 nm
Slope is 1708 and y-intercept is -0.03397
what is the molarity of the final unknown solution and the molarity of the original solution made from aspirin in the 250.0 ml flask
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- 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?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.What is the concentration of hydrochloric acid? Find the concentration using the information given below. Equipment used in the lab: 50 mL burette X M H2SO4 solution (aq) • Two 50 mL beakers 0.10 M NaOH (aq) Procedure: 25 mL volumetric pipette • Bromothymol blue indicator • Pipette pump • 250 mL Erlenmeyer flask Observations from the Titration Lab. Trial 1 Trial 2 Trial 3 Final burette reading 14.6 mL 27.85 mL 40 mL Initial burette reading 0 mL 14.5 mL 27.85 mL Volume of H2SO4 (aq) added 25 mL 14.6mL 13.35 mL 12.15 mL
- In carrying out the first standardization in this experiment, a student used 0.5169 g of potassium hydrogen phthalate (KHP) and 24.17 mL of a NaOH solution are needed to reach the equivalence point. What is the concentration (in mol/L) of the student's NaOH solution? Include only the numerical answer (no units). be careful with significant digitYou want to determine the concentration of NaCl in a water. In preliminary analysis, it appears to be saline water with a NaCl content of approximately 4%. Should you dilute the sample if your titrant has a concentration of 0.1 M and you want to spend 25 mL of sample?Please show all the calculations. I have these information available: 32.00 mL of 1 butanol and 20.00 mL glacial acetic acid were in the 100 mL distilling flask. Initial Aliquot:1 mL and add around 20 mL of water.Volume of NaoH required for titration: 67.3 mL After Aliquot:1 mL and add around 20 mL of water.Volume of NaOH required for titration: 23.4 mL Concentration of NaOH: 0.0972 M
- I need help with filling out the accompanying chart. Here is the data provided: Part A: The standardized HCl solution being used is 0.198 M. Trial 1: Using a volumetric pipette, you pipet exactly 20.00mL of the standardized HCl solution into a 250-mL Erlenmeyer flask. You then add 2-3 drops of phenolphthalein. Trial 2: Using a volumetric pipette, you pipet exactly 10.00mL of the standardized HCl solution into a 250-mL Erlenmeyer flask. You then add 2-3 drops of phenolphthalein. Trial 3: Using a volumetric pipette, you pipet exactly 10.00mL of the standardized HCl solution into a 250-mL Erlenmeyer flask. You then add 2-3 drops of phenolphthalein. Trial B: Determining the molarity (M) of acetic acid in vinegar. Trial 1: Using a volumetric pipette, you pipet exactly 5.00mL of the vinegar solution into a 250-mL Erlenmeyer flask. You then add 2-3 drops of phenolphthalein. Trial 2: Using a volumetric pipette, you pipet exactly 5.00mL of the vinegar solution into a 250-mL Erlenmeyer flask.…Suppose a group of students put 2.92 grams of an unknown solid acid into a 250-mL volumetric flask and filled it up to the mark with deionized water. After this they pipetted out 15.75 mL of a 1.78 M NaOH(aq) solution into another 250-mL volumetric flask and filled it up to the mark with deionized water. The students were given a pH meter that was already calibrated by their teaching assistant (T.A.) and they got the following result shown in the table below. Calculate the Molarity of the unknown solid acid. Hint: You can approximate the endpoint of the titration by taking the average volume between two consecutive titrant volume reading and you can assume that it is a 1:1 stoichiometry ratio between the acid and OH-(aq). VNaOH (mL) pH VNaOH (mL) pH 0 1.97 15 3.43 1 2.05 16 3.57 2 2.12 17 3.65 3 2.20 18 3.77 4 2.29 19 3.88 5 2.38 20 4.01 6 2.47 21 4.23 7 2.58 22 4.65 8 2.69 23…Pre Lab Questions: (Each answer is to be written as a complete sentence) What is the reason for washing the precipitate with water in Step 9? Define precipitate. Define filtrate. In Step 2, what is the purpose for rinsing the stirring rod? read the Procedure to answer the questions Using a balance, mass between 1.50 – 2.00 grams of sodium carbonate in a pre-massed 150mL beaker. Add 20 mL of distilled water and stir thoroughly to make sure all the crystals are dissolved. Rinse the stirring rod with a little distilled water after stirring. Using a balance, mass between 1.50 – 2.00 grams of calcium chloride dihydrate in a pre-massed 50 mL beaker. Repeat Step 2 for the solution in the 50 mL beaker. Pour the calcium chloride solution into the 150mL beaker containing the sodium carbonate solution and stir. Mass a piece of filter paper. Fold the filter paper and place it into the funnel. Wet it with a little distilled water to ensure that it is stuck to the sides of the funnel. Slowly…
- 50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution. Information of stock solution - molar mass- 534.3g/mole 0.587g in MilliQSTARTING AMOUNT X = 0.1 A student dissolves 24.3 g Na2S₂O3 in enough water to make a 0.302 solution. How many mL solution did the student make? ADD FACTOR x( ) 0.302 24.3 509 1 DELETE 6.022 x 10²3 0.509 L solution g Na₂S₂O3 A 158.1 ANSWER 1000 0.001 1.965 0.01 M RESET 5 3.311 100 M Na2S₂O3 kg Na₂S₂O3 mol Na2S₂O3 mL solution 10Should be 3 answers in total. Will thumbs up! Next the student conducts two different runs: In RUN 1, 10.0 mL of 5.00 M NAOH is combined with 10.0 mL of 0.010 M CO and 80.0 mL of wate In RUN 2, 20.0 mL of 5.00 M NAOH is combined with 10.0 mL of 0.010 M CO and 70.0 mL of wate The following plots were obtained for each of the runs: [crystal orange] vs time (RUN 1) In[crystal orange] vs time (RUN 1) 0.0012 0.001 -2 y--0.4463x- 7.3334 y =-0.0002x + 0.0007 R- 0.6565 R = 0.893 0.0008 4 0.0006 -6 0.0004 -8 0.0002 0.0002 -12 time (hr) time (hr) 1/[crystal orange] vs time (RUN 1) 1/[crystal orange] vs time (RUN 2) 12000 25000 10000 20000 8000 15000 6000 y = 2000x + 1000 R =1 10000 y 4000x + 1000 R =1 4000 2000 5000 time (hr) time (hr) Figure 4. Kinetic traces for the reaction between crystal orange and sodium hydroxide. What is the order with respect to CO? | Select ] What is the order with respect to NaOH? | Select ] What is the value of the averaged rate constant for the reaction above? Give…