A.) what is the normality of Na2C2O4 solution if you use 1.14g of Na2C2O4 to prepare 100.00 mL of solution?

B.) what is the normality of the stock KMnO4 solution if it took 31.20 mL of the KMnO4 solution to titrate a 20.00 mL sample of the oxalate solution prepared in part a?

The pKa of the α-carboxyl group of phenylalanine is 1.83, and the pKa of its α-amino group is 9.13. Calculate the average net charge on phenylalanine if it is in a solution that has a pH of 8.20. If the charge is positive, do not enter a + sign.

Determine the Kanfor a .035 M weak (monoprotic) acid with a ph of 3.5. Show work too please?

how to make a mole fraction of 0.25, 0.50, 0.75 ethyl acetate and cyclohexane having a total volume of 5 or 10 ml

Be sure to answer all parts.

Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH₃CH₂)₃N

(

K_b = 5.2

×

10⁻⁴

)

,

with 0.1000 M HCl solution after the following additions of titrant.

(a) 10.00 mL:

pH =

(b) 20.50 mL:

pH =

(c) 25.00 mL:

pH =

What is the concentration of a NH₃ solution having a pH of 11.15?

Methanol and ethanol are both oxidized by alcohol dehydrogenase (ADH). Methanol is poisonous because it is oxidized by ADH to form the highly toxic compound formaldehyde. The adult body has 40 L of water, throughout which these alcohols are rapidly and uniformly distributed. The densities of both alcohols are 0.79 g/mL. The Km of ADH for ethanol is 1.0x10-­‐3 M, and for methanol the Km is 1.0x10-­‐2 M. The molecular mass of methanol is 32 g/mol and that of ethanol is 46 g/mol. If an individual consumed 100 mL of methanol (a leathal amount), how much 100-­‐proof whiskey (50% ethanol by volume) must this person consume in order to reduce the activity of ADH toward methanol to 5%? Assume the Ki for ethanol = Km.

Given:

Ka1= 7.5*10^-3

Ka2=6.2*10^-8

Ka3=4.2*10^-13

What is the pH of a solution of 0.550 M K2HPO4, potassium hydrogen phosphate?

What is the pH of a solution of 0.400 M KH2PO4, potassium dihydrogen phosphate?

calculate the formula mass of each compound given below. keep at least one decimal place in atomic masses from the periodic table. a) hydrogen peroxide, H2O2. b) sulfuric acid, H2SO4.

Calculate the change in entropy when 108 ml of hot (97 oC) water added to 36 ml cold (5 oC) water in a closed Styrofoam cup given that C_p (H₂O, l) = 75.5 J/(mol * K)

200. g of liquid phase octane (C8H18) are burned in air at a temperature of 100. degrees Celsius and a pressure of 1.00 atm, forming vapor phase water and carbon dioxide.

a) Write the balanced chemical reaction equation for this process.

b) What is the magnitude of the difference between ΔE and ΔH for one mole of octane going through this process? (Hint: use the value of R that makes life easiest.)

c) The reaction is in contact with a reservoir of water that is also at 100 degrees Celsius. If that reservoir absorbs all of the heat released by the reaction (of the 200. g of octane), how many moles of the water will evaporate? Each mole of C8H18 releases 5074.482 kJ of heat when it goes through this process.

Part a I got no problem, but I can't seem to figure out parts b and c. Thanks for the help!!

.

Hi, I am doing an experiment that is called NaBH4 reduction of acetophenone. I am having trouble understand the techinque/wording when using a sep funnel. These are some of the procedures below:

1. Pour the mixture into a separatory funnel and add 20 mL of ice water. Rinse the beaker with additional ice water (5 mL) and add the rinsing to the separatory funnel. Rinise the beaker with ether (2 X 15 mL), adding the ether to the separatory funnel.

2. shake mixture, vent, and then remove the ether layer and set aside. Most of the product should be in the ether layer

3. extract the aqueous layer with ether (2 x 25 mL) to remove the remainder of the product. Combine all ether layers in a common beaker

(The multiply sign means the number of times you do it)---however can someone explain to me more clearly of that the steps tell you to do?

Consider the reaction between oxalate ion and permanganate ion in acidic solution: ???4 − (??) + ?2?4 2−(??) → ??2+(??) + ??2 (?)

a. Balance the reaction in acidic solution

b. Determine the standard cell potential of the representative voltaic cell

c. Determine the standard free energy change of this reaction

d. Determine the cell potential if the pH = 4 and all other solute concentrations were standard.

Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol):

(a) 1 Cl2(g) + 1 Ca(s) --> 2 Cl-(aq) + 1 Ca2+(aq) E = ___V

b) 2 Cu2+(aq) + 1 Fe(s) --> 2 Cu+(aq) + 1 Fe2+(aq) E = ___V

(c) 1 Hg22+(aq) + 2 Cu(s) --> 2 Hg(l) + 2 Cu+(aq) E =___ V

(d) 1 Cd2+(aq) + 1 Sn(s) --> 1 Cd(s) + 1 Sn2+(aq) E = ___V