I need yo know this answer by midnight tonight. thanks.

you will need to construct your own data sheet for this experiment.

DATA ANALYSIS steps 1-2:
The colorimeter wsa used to measure teh absorbance of each of a series of [FeSal]+ solutions. A standard curve was constructed by plotting the absorbance vs. the concentration (M). The slope and y-intercept were found to be 1510 M^-1 and 0.001, respectively.
PROCEDURE:
An aspirin sample was prepared, following the procedure given in the experiment: hydrolyzing the 0.139 g of it with 5 mL of a 1 M NaOH (reaction 1), diluting this mixture to 50.0 mL (forming solution A), and taking a 1.00 mL aliquot of this solution an diluting it to 50.00 mL with 0.02 M Fe(III) (forming solution B - reaction 2). The absorbance of solution B was measured to be 0.366.
DATA ANALYSIS step 3:
(a) Use the measured absorbance and the standard curve's slope and y-intercept to calculate the concentration of [FeSal]+ in solution B.

(b) How many moles of [FeSal]+ were in the 50.00 mL of solution B?

(c) How many moles of sodium salicylate were in the 1.00 mL aliquot of solution A used to prepare soution B?
Hint: look at the stoichimetry of reaction (2) in the experiment to see how the moles of sodium salicylate realte to the moles of [FeSal]+.

(d) Given the number of moles of sodium salicylate in 1.00 mL of solution A (calculated above), how many moles are in the 50.00 mL of solution A?
Hint: This is not a dilution or Beer's Law problem. It is a simple multipication.

(e) Based upon the number of moles of sodium salicylate calculated in part (d), how many moles of acetlsalicylic, C9H8O4, were in the aspirin sample?
Hint: look at the stoichiometr of reaction (1) in the expt.

(f) Use the mass of the aspirin sample (given in the PROCEDURE section above) and the answer to part (e), coverted to grams to calculate the mass percent of acetlsalicyclic acid, C9H8O4, in the aspin sample.

2. A one liter of solution phosphate buffer is made so that it is 1.00M in NaH2PO4 and 1.50M in Na2HPO4. If the pka of NaH2PO4 is 7.21 assuming the volume negligible change upon addition of acid or base calculate?

a. the Ph of buffer?

b. the resulting pH after addition of 0.25 mol of NaOH?

c. the amount of NaOH that would have to original buffer to bring pH upto 8.0

1) During the work-up procedure of our second reaction (“Hydrogenation of a Chalcone”), the following steps are performed:

a) Add 15 mL of brine and 10 mL of ethyl acetate to the mixture. Shake vigorously, then separate the ethyl acetate layer from the aqueous phase. Store the ethyl acetate layer in a dry, clean Erlenmeyer flask.

b) Extract the aqueous phase again with an additional 5 mL of ethyl acetate.

c) Combine the two ethyl acetate solutions and wash this ethyl acetate layer with 5

mL of brine. Drain the aqueous phase and pour the ethyl acetate solution into a

clean 25-mL Erlenmeyer flask.

d) Dry the organic phase with anhydrous magnesium sulfate for 5 min.”

Why are we performing each of the four steps mentioned above? (What is the purpose?) Please explain.

Give the values of the quantum numbers ( n, l, ml, ms) associated with the following orbitals: 2p spin up, 3s spin up, 5d spin up.

A certain chemistry instructor felt that there were some "dry-labbers" in the chemistry course. ["Dry-labbers" think they know the answer to a lab experiment, and give their expected answer without doing the experiment--which isn't fair to the others in the lab!] So, all students in the lab were asked to determine the boiling point of pure water contained in a flask labeled "pure water." The "pure water" was actually a very concentrated calcium dichloride solution. Three students were caught not actually doing the experiment and given F's for their experiment. Explain how the chemistry instructor was able to catch the dishonest "dry-labbers."

According to the textbook: “lectin and glycan arrays provide a platform to screen large number of samples for specific binding interactions using fluorescently labeled molecules. Two basic types of arrays have been developed for screening purposes: (1) protein arrays containing covalently attached lectin proteins or antibodies for the detection of labeled glycoproteins in experimental samples; and (2) glycan arrays containing covalently attached glycoproteins with intact glycan groups (or chemically synthesized glycan groups) for the detection of labeled lectin proteins or antibodies in experimental samples. Pick one type of array. Explain one advantage and one disadvantage to this type of glycan analysis. Find a method that has been developed to overcome the disadvantage that you listed and briefly explain how it works.

determine the miller indice of the plane comprised of the following coordinates: (1/2,0,1/2) (0,0,1) (1,1,1)

A reaction was run and found to have a half life that got shorter as the initial concentration of the reactant ([A]) was increased. When the reaction was run at two different temperatures, the following data sets were generated.

Use the data given to determine the value of k (the rate constant) at each temperature, and then determine the Energy of Activation for this reaction.

k at 530 K = ??? 1/Msec

k at 940 K = ??? 1/Msec

Ea = ??? kJ/mol

Professor Modyn owns a device called a pneumatic accumulator. This device maintains constant pressure of 217.00 psia as air enters by using a piston. Initially the device is filled with air at 76.74 °F and the volume is 0.317 ft3 (State 1). Air at 191.2 °F and 217.00 psia is fed into the accumulator until the volume triples and the temperature increases to 181.2 °F (State 2). Assume air is an ideal gas with a CP = 3.5R and MW = 29. No air leaves the system.

a) Find the amount of air added. (lbmol)

b) Calculate the work interaction term. (ft*lbf)

c) Calculate the heat interaction term. (ft*lbf)

A mixture is prepared that has 0.5276 g of solute in 9.9022g of cyclohexane. The freezing point temperature change is found to be 5.4 degree C. The percent composition of the solute is: 93.7% C, and 6.30% H.

a. find the empirical formula of the solute.

b. find the empirical mass of the solute.

c. find the molar mass of the solute.

d. find the molecular formula of the solute.

column chromatography

Why do you begin with a nonpolar solvent and continually increase polarity instead of the other way around?

. Are the factors controlling the movement of the compounds the same for TLC as they are for column chromatography? Briefly, why or why not?

. what would you change to make for a more efficient separation.

Problems by Topic - The Common Ion Effect and Buffers

Solve an equilibrium problem (using an ICE table) to calculate the pH of each of the following.

(1) a solution that is 0.17 M in HCHO2 and 0.11 M in NaCHO2

(2) a solution that is 0.12 M in NH3 and 0.16 M in NH4Cl

2nd set of problems

Part A

Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.110 M in HClO and 0.155 M in KClO.

Part B

Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.180 M in C2H5NH2 and 0.155 M in C2H5NH3Br.

Part C

Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 10.5 g of HC2H3O2 and 13.5 g of NaC2H3O2 in 150.0 mL of solution.

Why my percentage yield is much less than 100%?

what couze that ?

Determine the percent ionic charcter of the following bonds, based on the electronegativity differences: Show your work.

a. NaCl

b. FeCl2

c. CuCl

d. AlCl3

e. CCl4