Commercial club soda is produced by pressurizing water with 10 atmo- spheres of CO2. Find the value of KH for CO2 on the net or in the library, and calculate how much CO2 is in a 12 fl. oz. glass of club soda. When the CO2 reverts to the gas phase (as it eventually will in your digestive system), figure out how much volume it occupies at physiological conditions (37o C and 1 atm). Then contemplate burping.

The density of liquid methanol, CH3OH (FM=34.05), is 0.791g/mL at 77 degrees F. What is this same temperature in K, and how many methanol molecules will occupy a cubic container, 1mm on each side?

A protein solution was placed in an analytic centrifuge and spun until equilibrium was reached. The measurement was then repeated. But it was realized, too late, that prior
to the second run, the protein had been denatured. The average size of a denatured protein is larger than that of a native, compact protein. (a) Do you expect the distribution of molecules to be the same, at equilibrium, for the two different runs? Explain. (b) The time that it takes to reach equilibrium depends on the sedimentation constant of the molecules. Which run will reach equilibrium faster, the one with the native protein, or the one with the denatured protein? Explain how you imagine the sedimentation process of the two molecules.

What would happen to the pH as Ksp values increase? And Why?

Two 24.0mL samples, one 0.200 MKOH and the other 0.200 M CH3NH2, were titrated with 0.100 MHI. Answer each of the following questions regarding these two titrations.

What is the volume of added acid at the equivalence point for KOH?

What is the volume of added acid at the equivalence point for CH3NH2?

Predict whether the pH at the equivalence point for each titration will be acidic, basic, or neutral.

Predict which titration curve will have the lowest initial pH.

Thanks!

A student mixed 5.00 mL of 0.0120 M Pb(NO3)2 with 5.00 mL of 0.0300 M KI and observed a yellow precipitate.

a. What is the molecular formula of the precipitate? PbI2

b. How many moles of Pb2+ are present initially? ___

c. How many moles of I- are present initially? ___ The concentration of I- at equilibrium is experimentally determined to be 8.0*10^-3 M.

d. How many moles of I- are present in the solution (10mL)? ___

e. How many moles of I- precipitated? ___

f. How many moles of Pb2+ remain in solution? ___

g. What is the concentration of Pb2+ in the equilibrium solution? ____ M (Equilibrium solution is still 10mL)

h. Determine Ksp of PbI2 from this data. ____

Write the electronic configurations for Mn, Mn²⁺, Mn⁴⁺, Mn⁶⁺, and Mn⁷⁺

Calculate the concentration and the pH in a .10 M solution of sodium acetate, Na(CH3CO2). Equilibrium constant of acetic is 1.8*10^-5.

When methyl alcohol is treated with NaH, the product is CH3O -Na+ (and H2) and not Na+ -CH2OH (and H2). Explain why this is so.

Predict the spontaneity of a reaction (and the temperature dependence of the spontaneity) for each possible combination of signs for ?rH and?rS (for the system).

-?rH negative, ?rS positive

-?rH positive, ?rS negative

-?rH negative, ?rS negative

-?rH positive, ?rS positive

Here are some questions and their answers. I would appreciate it if someone could explain to me step by step how to get the answer?

1) A student pipets 25 mL of propanoic acid from a stock container labeled 0.18 M propanoic acid. The student then dilutes the 25 mL to 100 mL with distilled water. He labels the bottle of 100 mL of propanoic acid with what concentration? The answer for this is 0.045M propanoic acid, but can someone show step by step how to get to this answer?

2) Which of the following three salts would be acidic if dissolved in water: I. KCN II. NH4Br III. C2H5NH3Cl
answer: II and III only (how and why???)

3) What is the OH− concentration in Drano, a common drain cleaner that has a pH of 12.3 at 25oC? Answer: 0.02 M

4) What is the hydronium ion concentration (x) in a 1.23M solution of hypochlorous acid (HOCl) at 25oC. Answer: sqrt 1.23 ∗ 3.5x10^-8

5) The two acid dissociation constants for sulfurous acid, H2SO3, are 1.3× 10–2 and 6.3× 10–8 at 25oC. The base constant, Kb, for HSO3– is:7.7 × 10^–13

A beaker with 1.70×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.70 mL of a 0.430 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.

Using atomic absorption, 0.0105 grams of copper sulfate pentahydrate were dissolved in a 100 mL volumetric flask and diluted to mark to make a 100 ug/mL solution. An unknown was made by placing an unknown amount of the above stock solution in a 100 mL volumetric flask and diluting to mark. The unknown gave an absorbance of 5.809 mg/L. How many mL of stock was used to make this unknown? The answer should be between 1 and 10 mL

Using standard reduction potential, predict and explain which of the following is the strongest reducing agent: Mg, I^-, Fe²⁺

If possible, please provide a detailed solution to accompany your answer.

A yellow compound is placed on a column and the column is eluted with hexanes. After a large volume of solvent has been collected but the yellow band is still at the top of the column. What should be done to recover the yellow compound? How could this experiment have been done better?