Copy of 5AL Lab 5 Submission Template - F23v2

Plz look at the pic. Thanks.

Please let me know which 2 answers are correct, an explanation including evidence

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?

You have a stock solution of 150.0±0.3 mg SO²/mL that has been certified by the manufacturer. You decide to dilute the solution by a factor of 100 to get a final concentration of 1.500 mg/mL. To do this, you use a 1.000±0.006 mL transfer pipette to transfer your stock solution to a 100.000.08 mL volumetric flask that you then dilute to the mark. Please calculate the absolute and relative error for the final concentration.

Q3: In a chromatographic analysis, a solution was prepared with 0.0837 M Octane (A) and 0.0666 M nonane (B). Each one produced a peak area of AA = 423 and AB = 347.10.0 ml of 0.146 M nonane was added to 10 ml of an unknown sample, and the sample diluted to 25 ml. The peak areas obtained were AA = 553 and AB = 582. What is the concentration of Octane in the unknown sample?

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.

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.

28 Report Sheet Separation of the Components of a Mixture D. Determination of Percent Recovery Mass of original sample 10.588 Mass of determined (NH Cl+ NaCl+ SiO2) 1-88 8 Differences in these weights g matter recovered Percent recovery of matter %3D = %00 % g original sample Account for your errors. Combor QUESTIONS 1. Could the separation in this experiment have been done in a different order? For example, if the mixture was first extracted with water and then both the extract and the insoluble residue were heated to dryness, could you determine the amounts of NaCl, NH,Cl, and SiO, originally present? Why or why not? Consult a handbook to answer these questions. 2. How could you separate barium sulfate, BaSO4, from NaCl? 3. How could you separate magnesium chloride, MgCl2, from silver chloride, AgCl? 4. How could you separate tellurium dioxide, TeO2, from SiO,? 5. How could you separate lauric acid from a-naphthol? (See Table 3.1.)

2 What methods are used to sep X G In Part Il of experiment 5, a 1:1: X + u/ultra/courses/_393452_1/cl/outline * Question Completion Status: QUESTION 3 After you complete the second step, you will be left with a clear colorless liquid. What should be done to the liquid to finish the separation? O Heat the mixture to evaporate the liquid O Add a base to neutralize the solution. O Nothing - you are done since you have a pure, clear, colorless substance O Add the residue back to the solution and dry. QUESTION 4 In Part II of experiment 5, a 1:1:1 mixture of sand, salt, and salicylic acid must be separated. Order the following steps necessary to separate this mixture into three pure, dry solids. Filter the liquid leaving a filtrate with just salt dissolved and a residue of sand. v Add hot water to the residue obtained in two steps prior to this one. Filter the liquid leaving a filtrate with just salicylic acid dissolved and a residue of salt and sand. v Heat the filtrate obtained in two…

Please don't provide handwriting solution

Pre-lab 1. In your own words, what is accuracy and precision? Why are they important in the clinical lab?

Please help with the following, make sure your asner is correct with proper signs 100%, pls and thank you

Individually weigh each of the nine nickels used in part 2b. Then calculate the average,average deviation, and standard deviation of the nine samples. The mass of a U. S. nickel,when minted, is 5.000 g. What is the percent error between your average and the U. S. Mintvalue? Pay close attention to your significant figures when doing these calculations.   Sample Mass (g)                                                         Average Mass ____________ gNo.1 _5.029 ______                         Average Deviation ____________ g2 _5.010 ______                          Standard Deviation ____________ g3 _4.983 ______                            Percent Error ____________ %4 _5.036 ______5 _4.989 ______6 _5.026 ______7 _5.028 ______8 _4.980 ______9 _4.952 ______   im having issues with average deviation and standard deviation

1a. Throughout the experiment, what are some possible sources of error that could have led to someone recovering a significantly smaller amount of table salt (NaCI) than was originally present in the sample mixture. 16. What are some possible sources of error that could have led to someone to appear to have recovered a significantly larger amount of sand (SiO2) than was originally present in the sample mixture.

Determine the volume of a sample of copper in (m³) with a mass of 2.2 x 105 tons and a density of 8.96 g/cm. (1 ton = 2205 lbs, 1 lb = 16 ounces, 1 kg = 2.20 lbs,1 kg = 1000g. 100 cm = 1m) %3D %3! %3D

You begin preparation of the calibration curve to measure absorbance vs concentration of FeSCN2+. To do so, you add 2.422 mL of 0.200 M Fe(NO3)3 to a cuvette and then directly add 215 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.

Log Nt = Log N0 – t/D.   D is the time required for a log kill. Levels of bacterial cells in the water supply must be undetectable, which, in terms of the equation, is <1 per mL of drinking water. A single addition of chlorine yields a log kill every 5 minutes.  During a storm, levels in the incoming water reach 10,000/mL. You hold the incoming water in a treatment tank and give it a single hit with chlorine. If you add the chemical at 10 a.m., when will it be safe to open the valve and release that water for drinking?

Consider the following SAS data and formula. Volume of sample at $1%: 50.2 ml 51% = 55% 52% = 70% Volume of SAS = [(volume of sample at S1%) (S2% - S1%)] / 100 [(1-(S2% / 100)] Calculate the volume of SAS needed for this experiment given this information.

QUESTION 10 A student combined two colorless chemical compounds in a test tube. Immediately a yellow solution formed. When the student cooled the test tube the solution once again turned colorless. Was the reaction exothermic or endothermic? Explain, clearly and concisely, how you arrived at your answer. For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac), T T T Arial 3 (12pt) -T-= - E Path: p Words:0

Assuming all other values are accurate, what would happen to the experimental value of Rif the Mg was not completely consumed? R=PV/nT

To enter exponential values, use the format 1.0e-5. Solution 1.10 M Acetic acid (mL) 0.900 M Sodium acetate (mL) [H30*] (M) 1 8.00 2.00 2 7.00 3.00 3 6.00 4.00 4 5.00 5.00 4.00 6.00 6. 3.00 7.00 7 2.00 8.00 8 1.00 9.00 LO