Experiment 1 Isolation and Identification of Caffeine

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.

A pipet delivers 10.9 mLmL , 10.1 mLmL , and  10.9 mLmL  in consecutive trials. Find the mean volume of the samples.  =  Answer = 10.6 mL Part B What is the average deviation from the mean for the above samples?

What should the concentration be for the acid?  Calculate the percent error.

Convert the amount of spiperone in each sample to the concentration in the 1 ml total volume of assay tube. I have calculated amount of 3H spiperone in pmol in each dilution in second picture. To converted concentration in 1 ml total volume of each assay tube do I need to consider dilution factor？

I need help to calculate this data please thanks a lot

Trial 1 Trial 2 Trial 3 Vinegar Volume (mL) 5.00 5.00 5.00 Final buret reading of NaOH(mL) 34.96 32.38 33.12 Initial buret reading of NaOH(mL) 4.85 2.30 2.98 Volume of NaOH dispensed (mL) 30.11 30.08 30.14   Compare the experimental process of your three trials above. Was one trial more accurate than the others? Why? (What are you basing this decision on?) Suppose the concentration of the NaOH solution was 0.5 M instead of 0.1 M. Would this titration have required more, less, or the same amount of NaOH solution for a complete reaction? Suppose you used 0.5 M NaOH to titrate your vinegar sample instead of 0.1 M. What effect does the concentration of base added have on the reliability of the results of your titration?

2

How do you find the standard deviation with these calculations?

Concentration of TZ stock solution (μMμM) 42.06

Sources of error: Method 1  Equipment:About ten grams of NaHCo3. 10 ml distilled waterSmall beaker Electronic balanceGlass dome10 ml graduated cylinderGlass rod Safety instructions :Wear safety goggles Wear a smockBe deilcate with materials  Method:Measure out 10 ml of distilled water using the graduated cylinder. Transfer the water to the small beaker.Weigh out the total amount of sodium chloride available for the experiment.Weigh out 0.5 g NaHCo3. Add NaHCo3 to beaker containing water. Stir solution with glass rod until dissolved.Repeat step 3 until it becomes more difficult to dissolve the NaHCo3. Note the number of times 0.5 g NaHCo3 is added.Continue adding one grain of NaHCo3 at a time until it is no longer possible to dissolve it.Once saturation is reached, NaHCo3 crystals form at the bottom of the beaker.Measure the mass of NaHCo3 not added to determine the total amount of NaHCo3 that has exceeded the solubility limit.

can you show how the highlighted answers are acheived?

answer with all work

Trial 1 Trial 2   Initial Buret Reading 0.05 mL 0.02 mL   Final Buret Reading 25.25 mL 23.22 mL   Volume of base used       Molarity of base used 0.1045 M 0.1045 M   Volume of vinegar used 5.00 mL 5.00 mL

• Stock solution: 1000 mg/L Target sample concentrations: 50-400 mg/L • Create a 5-point standard dilution to cover the test • If each test only needs 10 mL, make plans to make the dilution so you have 20 mL of each concentration. ·

Prelab1 Please help with 1-3

1- Small bottles (500 water or soft drink bottles). 2- Balloons 3- about 500 mL of vinegar 4- About 50 g of baking soda (baking powder can be used) 5- small spoon Safety None of the chemicals used in this experiment are hazardous. Procedure 1. Use three dry empty water bottles (any size, lager size 0.500 L is better). Add around 100 mL (4 tablespoons). Make sure you label the bottle. 2. Place one teaspoon (or 5.00 g if you have kitchen scales) of sodium bicarbonate into first balloon, two teaspoon in the second and three teaspoon in the third. 3. Carefully attach one balloon to the top of each bottle or glass without letting any of the sodium bicarbonate tip out yet. 4. Tip the solid powder into the vinegar, making sure all of the solid powder is transferred down into the glass. 5. Record your observations in the corresponding sections in this document based on your experiments, then answer all questions. You will also need to take some photos and include them in this document. Please…

Monitored therapeutic drugs must have both a trough and a peak blood level drawn and tested.   Question 2 options:   True   False

I need help finding the %Composition for %cychohexane and %toluene. The formula (area of peak/total area) * 100%

Using figures 3 and 4 in the lab manual, rank each compound according to their polarity. For the least polar molecule, draw the structure and label any important functional groups on the molecule.