Hi, I had a quick question about hydrophobic and hydrophillic regions on a molecule.

I am confused on how to know if a molecule, which has both hydrophillic and hydrophobic regions, will be soluble in water or not? Can someone please explain in clear and simple words, thank you so much!

For example, in the molecule vitamin A, theres OH group which is hydrophillic but the rest of the molecule is hydrophobic, so how would I know if the whole molecule would be soluble in water or not?

Calculate the amount of energy in kilojoules needed to change 153 g of water ice at –10 ∘C to steam at 125 ∘C. The following constants may be useful: Cm (ice)=36.57 J mol−1 ∘C−1 Cm (water)=75.40 J mol−1 ∘C−1 Cm (steam)=36.04 J mol−1 ∘C−1 ΔfusH=+6.01 kJ mol−1 ΔvapH=+40.67 kJ mol−1

For the determination of the Fe in a Mohr's salt sample, do you expect to obtain more accurate results, with the data obtain after the direct titration using the indicator or with the data obtained with the potentiometric titration? Briefly justify your answer

What are the significance of bandstructure (E-k) plots? Which information we can get from E-k plots (obtained from DFT analyses) for materials? Please explain in details with some relevant diagrams or plots.

Please explain how to solve and show all work! I'm extremely lost.

Part 1:

A 180,000 gal. swimming pool requires treatment with 8.85 L of 7.00% "by mass" chlorinating solution to give chlorine level of 1.00 ppm (1.00 g chlorine per 10^3 kg of pool water). Based on these data, calculate d (in g/ml) for the chlorinating solution nothing that it is close to 1 g/mL. * "% by mass" means "mass of solute/100g solution". thus, this chlorinating solution contains 7.00 g chlorine/100 g chlorinating solution.

Part 2:

Take pool water as pure and, for the poo, calculate the H2O/Cl2 molecular ration after treatment with the 8.85 L of the chlorinating soln.

Part 3:

If density, d (pool water) = 1.00 g/mL, and d (chlorinating solution) = 1.10 g/mL, calculate volume, V, of chlorinating solution to add to the 180,000 gal pool water to up d of resulting pool wter to 1.01 g/mL.

25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of 0.200 M solution of NaOH in a constant pressure calorimeter. The temperature increases from 23.00 °C to 24.37 °C. Assume that the specific heat of the solution is the same as that of pure water (4.18 J/(g•°C)) and that the density is the same as pure water (1.00 g/mL). Calculate ΔH per mole of reaction for the below chemical reaction.

HBr (aq) + NaOH (aq) → H₂O (l) + NaBr (aq)           

2.(3) Translate the following statement into a balanced chemical equation.

Three moles of calcium chloride react with two moles of sodium phosphate to produce solid calcium phosphate and six moles of sodium chloride.

3.(3) 50.0 mL of 1.0 M Ag(NO3) is added to 5.55 g of CaCl2 (MM=111.0 g). What is the concentration of nitrate ion in the final solution in moles/liter?

3a.(3) How many grams of silver chloride can be produced in this reaction?

at 25c the standard enthalpy of formation of HF(aq) is -320.1 kj/mol. of OH(aq) it is -229.6Kj/mol. of F (aq) it is -329.2 Kj/mol.of H2O(l) it is -285.9Kj/mol.

a. calculate the standard enthalpy of neutralization of HF.
HF (aq) + OH- (aq) -->F-(aq) +H2O (l)

b.using the value of -56.2kj as the standard enthalpy change for the reaction
H+(aq)+ OH(aq)->H2O(l)

c. calculate the standard enthalpy of change for the reaction
HF->H+F

Ro-vib spectroscopy observe what type of molecule? What is his energy range? Measured molecule properties.

If a small amount of the benzoic acid measured fails to dissolve in the lauric acid, what impact would this have on the molecular weight calculated? Would it be too high or too low? Explain your answer

The boiling point of ethanol CH₃CH₂OH is 78.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is estrogen (estradiol).  

How many grams of estrogen, C₁₈H₂₄O₂ (272.4 g/mol), must be dissolved in 265.0 grams of ethanol to raise the boiling point by 0.500 °C ? Refer to the table for the necessary boiling or freezing point constant.

g estrogen.

Why is molecular bonding an important consideration inn the manufacture of plastics?

Determine whether each of the following statements about the thermodynamic functions are True or False as they apply to chemical reactions.

1.The heat of reaction at constant volume is never equal to the heat of reaction at constant pressure.

2.All spontaneous chemical reactions have negative entropy changes.

3.The entropy change does not effect spontaneity.

4.Enthalpy and temperature are multiplied in the Gibbs free energy.

5.Spontaneity is increased by negative enthalpy changes.

Will combining Thr and Phe into the dipeptide Thr-Phe will release a molecule of water?

Please show work, thank you!

Relative strengths of acids:

Can an Organic Chemistry I and II MASTER explain to me some rules of thumb in regards to the relative strengths of acids.

1) List the functional groups (alcohols, carboxylic acids, phenols, anhydrides, amides, etc.) in order of DECREASING ACIDITY.

2) In regards to substituents on aromatic rings, which substituents would act as stronger bases, why, and in what relative position (ortho, meta, or para); and if the number of substituents affects basicity?

The list will be most helpful, so please list as many functional groups as possible. Thank you in advance.