The Separation of Three Organic Compounds by Acid, Base Reactions and Liquid, Liquid Extraction.

Okay, so we had solid benzoic acid, ethyl 4- aminobenzoate, and 9-fluorenone all dissolved in diethyl ether. We separated the basic component by adding 3M HCl, we separated the acidic component by adding 3M NaOH. I don't understand what happens here. To isolate the acidic solution, we added 6 M NaOH and used the vacuum to recover the solid. To isolate the basic solution we added 6M HCl. I did an experiment where a 1:1:1 mixture of Benzoic Acid solid (C6H5COOH), ethyl 4-aminobenzoate solid (C9H11NO2), and 9-fluorenone solid (C13H8O) was dissolved with methylene chloride. Then each component was extracted and tested. I need to come up with a proton transfer chemical reaction that represents what happened in each separation. First separation: HCl was added and two layers formed. aqueous layer was extracted and transfer to a clean container and methylene chlotide layer was left aside. NaOH was added dropwise to aqueouse layer extraction and vacuum filtration was used to extract/separate the basic component ethyl 4-aminobenzoate solid (C9H11NO2).

Results &Data:

1)Benzoic acid (Acid)

Table 1: Collected data from Benzoic acid

2) Benzoate (Base)

Table 2: Collected data from Benzoate.

3) 9-Fluorenone (Neutral)

Table 3: Collected data from 9-Fluorenone.

I need to find the theoretical and percent yield of each product, how many mg of each product is present. And also create 4 chemical reactions. Need help, Please help thankyou

Calculate the change in standard-state entropy for the following reaction that results in the formation of glucose:

6 CO2(g) +6 H2O(l) ⟶ 1 C6H12O6(s) + 6 O2(g)

(If applicable, coefficients of one have been included for clarity.)

Express your answer with the appropriate units. Use FOUR significant figures.

1. Complete Table 1 by calculating the volume of 2.0 mg/mL myoglobin, 6.0 M GuHCl, and 0.5 M phosphate buffer needed to make the 15 solutions needed for the experiment.

Describe the procedure you would follow to determine the concentration of Vitamin C in a sample if the volume of DCPIP required to reach the endpoint was more than the 25-mL flask could hold. Note the titration must still be carried out in the flask. Be sure to include any calculations you would need to perform.

Calculate Delta H rxn for the following reaction (watch the significant figures)

2 NOCl (g) --> N2(g) + 02(g) + Cl2(g)

Given the following set of reactions;

1/2 N2(g) + 1/2 02(g) ---> NO(g) Delta H= 90.3KJ
NO(g) + 1/2 Cl2(g) ---> NOCl(g) Delta H = - 38.6 KJ

Chromic acid (H₂CrO₄) is an acid that is used in ceramic glazes and colored glass. The pH of a 0.070 M solution of chromic acid is the same as the pH of a 0.054 M HNO₃ solution. Calculate K_a for chromic acid.

A hydrogen-oxygen fuel cell is used in the space program to generate clean energy. Describe, in detail, the principle and process of electrical energy generation from hydrogen-oxygen fuel cell. Also include in the discussion major advantages and limitations of such fuel cells.

The solutions at the two Pb electrodes of a concentration cell were prepared as follows:

Cell A: A mixture of 1.00 mL of 0.0500 M Pb(NO3)2 with 4.00 mL of 0.0500 M KX (the soluble potassium salt of an unspecified monovalent ion X-). Some PbX2(s) precipitates.

Cell B: 5.00 mL of 0.0500 M Pb(NO3)2.

The cell potential was measured to be 0.05100 V at 25 °C.

1.)By use of the Nernst equation, determine the concentration (M) of Pb2+ in the solution of Cell A.

2.)In Cell A, how many moles of X- have reacted with Pb2+?

3.)What is the concentration (M) of X- in the solution of cell A.

4.) Calculate Ksp of PbX2.

(a) Calculate the standard free-energy change (ΔG°) for the following oxidation-reduction reaction. Cu(s) + Br2(aq) → Cu2+(aq) + 2 Br−(aq)

(b) Calculate the equilibrium constant for this reaction at 298 K.

Describe the preparation of 40 L 0.02 M phosphate buffer, pH 6.9 starting from Solid KH₂PO₄ and K₂HPO₄

What is the minimum mass of ice at 0.0 C that must be added to 1 kg of water to cool the water from 28 C to 12 C? (heat of fusion = 333 J/g, Specific heat capacity of ice = 2.06 J/g K, water = 4.184J/g K)

Determine whether the entropy increases or decreases in the given situations.

a. A vapor that turned to solid
b. A vapor condenses to a liquid
c. A mole of vapor becomes solid
d. A liquid freezes
e. A solute dissolved in a solvent

A rigid stainless steel chamber contains 210 Torr of methane, CH4, and excess oxygen, O2, at 200.0

A 100.0 mL solution containing 0.976 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.296 M KOH. Calculate the pH of the solution after the addition of 56.00 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27

. pH =

At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the fully protonated, intermediate, and fully deprotonated forms, respectively.

[M2-] = ___ M

[HM-] = ___ M

[H2M] = ___ M

A 9.10-g sample of solid MnCl2·4H2O was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 atm and 100.0 °C?