For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

a) For 230.0 mL of a buffer solution that is 0.205 M in HCHO2 and 0.275 M in KCHO2, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

b) For 230.0 mL of a buffer solution that is 0.320 M in CH3CH2NH2 and 0.290 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

1.Which C = O aliphatic group absorbs more to the right of the IR spectrum? Show an example and explain the reason.

2. What functional groups show characteristic absorptions in the region of traces of the IR spectrum? Provide one molecule for each case

3.What is the expression for the Planck equation as a function of the wave number? Apply it to calculate the energy when  is equal to 3.0 μ. Emphasize the units

A rough analysis of cell contents suggests their cytoplasm contains 5% by weight of solutes: 1% is proteins of average molecular weight 45,000; 1% is soluble lipids of molecular weight 400; 1% is sugars of molecular weight 170; and 2% is salts like KCl. What is the osmotic pressure inside these cells relative to pure water at 37C? Assume the density of the cytoplasm is approximately 1g/cm^3 and has the properties of water.

Determine the molar solubility of AgI (Ksp = 8.50e-17) in 2.577 M S2O32- if the complex ion [Ag(S2O3)2]3- forms with a Kf = 2.90e13. Answers 0.09193/ 0.11637/ 0.04516/ or 0.14730

A 71.0 mL sample of 0.0400 M HIO4 is titrated with 0.0800 M RbOH solution. Calculate the pH after the following volumes of base have been added.

(a) 10.3 mL

pH =

(b) 34.4 mL

pH =

(c) 35.5 mL

pH =

(d) 36.2 mL

pH =

(e) 63.9 mL

pH =

Consider the titration of 30.0 mL of 0.0700 M (CH3)2NH (a weak base; Kb = 0.000540) with 0.100 M HClO4. Calculate the pH after the following volumes of titrant have been added:

(a) 0.0 mL

pH =

(b) 5.3 mL

pH =

(c) 10.5 mL

pH =

(d) 15.8 mL

pH =

(e) 21.0 mL

pH =

(f) 33.6 mL

pH =

For one of your trials during the equilibrium experiment at room temperature as described in the lab manual. You determine the following for Tube #1 while performing the experiment as described in the lab manual. For the standard solution in tube # 5 the absorbance value is 0.789 and the [FeSCN2+]eq of the standard is 0.0002000M. The following resuts apply to tube #1:

[Fe3+]o - 0.00100308 M

[SCN-]o - 0.00040005 M

absorbance tube 1 - 0.1657 au

Determine Kc.

Concentration of acetic acid: 1.041M and concentration of sodium acetate is 1.071M.

The buffer is created by mixing 100mL of acetic acid with 100mL of sodium acetate soluiton.

a) What is the pH of 75mL of the buffer solution after the addition of 1mL of 3M NaOH?

b) What is the pH of 75mL of the buffer solution after the addition of 5mL of 3M NaOH?

c) What is the pH of 75mL of the buffer solution after the addition of 15mL of 3M NaOH?

d) Calculate the volume of 3M HCl needed to change the pH of 75mL of the buffer solution by one pH unit (buffer capacity).

PLEASE SHOW ALL WORK. I DID SOME MISTAKES SOMEWHERE AND WOULD LIKE TO SEE FULL SOLUTIONS TO COMPARE.

Thank you very much.

To clean the impeller blades of a stainless steel tank, plant technicians pour 210.0 L of a 240.0 g HNO3/L solution in a 820.0-L tank to soak. When the tank needed to be emptied, the tank was first filled with water entering at a rate of 1.90 L/s. (Figure 1). At t = tF, the tank is completely full of solution. At this point water continued to enter the tank at the same rate, but solution was also drained from the bottom of the tank at 1.90 L/s (Figure 2). Make the assumption that the fluid density does not change and answer the following questions. 1.) What is the value of tF, the time it takes to fill the tank? 2.) What is CF, the concentration of HNO3 in the tank at tF? 3.)At what point after starting to add water to the tank is the concentration of HNO3 0.0500 of the original concentration?

1.

A.write a chemical equation which goes with the statement:

i) K_b= 4.3 X 10^-10 for aniline (C6H5NH2)

ii)K_b = 2.1 X 10^-4 for carbonate ion

B. K_b =1.3 X 10^-3 for C5H11N and k_b= 6.3 x 10^-5 for N(CH3)3

i) Which base is the stronger base in water

ii) For the same solute concentration, which base has the larger equilibrium OH- concentrations?How did you decide?

C. Reaction of amide ion (NH2^-), ethoxide ion (OCH2CH3-), methoxide ion (OCH3-), hydride ion (H-), or oxide ion (O^2-) with water gives hydroxide ion as one product , for each ion, the reaction goes to completion.

i) For each of these ions write a net ionic equation for the reaction of the ions with water.

ii) is a salt supplying one of these ions a strong base or a weak acid?Explain.

When doing the kinetic trials, Peyton mistakenly omitted the starch solution from the kinetic trials. How will this

omission change the appearance of the resultant solution (from the mixing solutions A and B) from that of a cor-

rectly completed experiment? Explain your reasoning.

Develop a recipe for 1.00 L of pH 4.50 buffer using only 17.4 M HC2H3O2 and 3.00 M NaC2H3O2 (and deionized water). Be sure that it canaccommodate additioin af at least 0.50 mol of strong acid or base with delta pH less than or equal to 1.

Thin Layer Chromatography

1. After running the first plate, the spot was not observed. Provide two possible reasons (not including operator error) as to why?

2. What other technique could be used to determine if a reaction was complete? Explain to a peer, how you would do this in lab.

3. Why might TLC not be the best technique to determine the identity of a compound?

1. The Ka of a monoprotic weak acid is 6.11 × 10-3. What is the percent ionization of a 0.151 M solution of this acid? use quadratic equation to solve

2. A certain weak base has a Kb of 7.60 × 10-7. What concentration of this base will produce a pH of 10.23?

please show all your steps

thank you!