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.

At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. Both the forward and the reverse reactions are occurring, but because they are occurring at the same rate, no change is observed in the appearance of the solution.

For this analysis, think about the affect that the addition or removal of reactant will have on the rate of the forward reaction relative to the rate of the reverse reaction at the instant that the reactant is added or removed. You also have to think about the addition or removal of product on the rate of the reverse reaction relative to the rate of the forward reaction.

a. When the concentration of reactant is increased for a system at equilibrium, what is the effect on the rate of the forward reaction? Does an increase in the rate of reactant have any effect on the rate of the reverse reaction? Explain your answer.

b. When the concentration of reactant is increased for a system at equilibrium, which reaction is immediately faster – the forward or the reverse reaction? Why?

c. As the reaction proceeds and the added reactant is used up, what happens to the rate of the forward reaction? At the point at equilibrium has been reached, what has happened to the rate of the forward reaction relative to the rate of the reverse reaction?

d. If reactant is removed from a system at equilibrium, what is the effect on the rate of the forward reaction? Does the rate of the reverse reaction change when reactant is removed?

e. When reactant is removed in a system at equilibrium, which reaction is faster – the forward reaction or the reverse reaction? Would that result in an accumulation of reactant or product in the flask?

f. Write a statement about why the addition of product causes the reaction to shift to reactants in terms of the relative rates of the forward and reverse reactions.

g. Write a statement from a kinetic perspective about why the removal of reactant causes the reaction to shift towards reactant.

What volume of a 0.1 M NaOH solution must be combined with 25 mL of 0.2 M HNO3 to reach a pH of 11.5?

Something that burns is said to be flammable. Do you think steel wool is flammable? is it readily flammable in air? in oxygen? what sort of differences to you observe?

In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH2)3CNH2, often abbreviated as Tris. At 25 ?C,                 Tris has a pKbof 5.91. The hydrochloride of Tris is (HOCH2)3CNH3Cl, which can be abbreviated as TrisHCl. Question 1.) What volume of 10.0 M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCl? ANSWER IS 6.67 Question 2.) The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100mol of hydrogen ions without changing the volume. What is the pH of the final solution? Answer IS 7.58 Question 3.) What additional volume of 10.0 M HCl would be needed to exhaust the remaining capacity of the buffer after the reaction described in Part B?