what is partition coefficients and their application to medicine or the environment. please provide some background on the topic.

In order to analyze for Mg and Ca, a 24-hour urine sample was diluted to 2.000 L. After the solution was buffered to pH 10, a 10.00 mL aliquot was titrated with 44.96 mL of 0.003474 M EDTA. The calcium in a second 10.00 mL aliquot was isolated as CaC2O4, redissolved in acid, and titrated with 17.35 mL of the EDTA solution. (Note: Normal levels for magnesium are 15 to 300 mg per day and for calcium are 50 to 400 mg per day.)

How many mg of Ca were in the original sample?

How many mg of Mg were in the original sample?

1) 20.00 mL of a 0.3000 M lactic acid solution is titrated with 0.1500 M NaOH.

a. What is the pH of the initial solution (before any base is added)?

b. What is the pH of the solution after 20.00 mL of the base solution has been added?

c. What is the pH of the solution after 40.00 mL of the base solution has been added?

How much heat (in kJ) is given off when 41.0g of water at 50.0°C is changed to 41.0g of ice at -5.00°C?

The specific heat of water is 4.184 J/g·°C
The specific heat of ice is 2.087 J/g·°C
The heat of fusion of water is 6.02 kJ/mol
1 mol of water is 18.0g

Describe the powder X-ray diffraction experiment. List the basic components in your diagram and discuss the features/roles of each component. Include Bragg’s Law as well as coherent and incoherent scattering. What types of information can be obtained using this technique? Pros and cons with respect to single crystal XRD?

what are the merits of normal absorbance to concentration calibration curve and log of absorbance versus log of concentration curve. Also state the comparison of the results obtained by those methods. which results are better.

The relative donor effect of simple ligands can be determined by measuring the carbonyl stretching frequencies of their metal carbonyl coordination complexes. Imagine you have prepared a series of L2-Ir(CO)Cl complexes and measured the carbonyl stretches. Assign the stretches (2102, 2054, 2032, 2014, 1995 cm -1 ) to the complexes containing the following ligands (assume that all ligands are purely σ-donors): NPh3, PPh3, pyridine, 4-fluoropyridine, 4-bromopyridine. Explain your reasoning!

A) Calculate the pH of a buffer that is 0.225M HC₂H₃O₂ and 0.162M KC₂H₃O. The Ka for HC₂H₃O₂ is 1.8x10^-5

B) A 1.00L buffer solution is 0.250M in HF and 0.250M in NaF. Calculate the pH of the solution after the addition of 0.100 moles of solid NaOh. Assume no volume chane uon the addition of base. Ka for HF= 3.5x10^-4

^C) A 100.0ml sample of 0.20M HF is titrated with 0.10M KOH. Determine the pH of the solution after the addition of 100.0mL of KOH. The Ka of HF is 3.5x10^-4

Using some of the materials listed below, come up with a reasonable synthesis for the preparation of Cp2TiMe2.

TiCl4, Cp-H, KH, PhBr, Mg, dicyclopentadiene, Li, hexane, THF, MeI, table salt, urea, dihydrogen monoxide, CO, CO2, SO2, KI, UI4, VCl5

6) If a mixture of compounds with a wide range of polarities has to be separated, two different eluents have to be used to isolate the chemicals. In this case, the eluent of lower polarity should be used first. Please explain why?

what are the merits of normal absorbance to concentration calibration curve and log of absorbance versus log of concentration curve. Also state the comparison of the results obtained by those methods. which results are better.

You have 77.0 mL of a 0.500 M stock solution that must be diluted to 0.100 M.

Assuming the volumes are additive, how much water should you add?

I'm trying to study for my General Chemistry II Exam, but I want to make sure that I don't miss anything important! If you could provide your input on the following concepts, that would be greatly appreciated! Thank you so much!(:

Chapter 16 - Chemical Kinetics

I. Reaction Rates

            A. Definition of reaction rate

            B. Mathematical expression for Reaction rate

            C. Instantaneous rate

            D. Initial rate

            E. Rate constant

            F. Rate law

            G. Integrated rate law

II. Determining Reaction Order

            A. Method of initial rates

III. Types of Reactions

            A. Second-order reaction

                        1. second-order integrated rate law

                        2. What must be plotted to verify that a reaction is second order?

                        3. What does the slope equal?

            B. First-order reaction

                        1. First-order integrated rate law

                        2. What must be plotted to verify that a reaction is first order?

                        3. What does the slope equal?

                        4. Half-life

            C. Zeroth-order reaction

                        1. zeroth-order integrated rate law

                        2. What must be plotted to verify that a reaction is zeroth-order?

                        3. What does the slope equal?

            D. Overall order of reaction

IV. Temperature dependence of reacton rates

            A. Realtionship between k and E_a

                        1. Arrhenius behavior

                        2. Arrhenius parameters

            B. Collision Theory

V. Catalysis