Write balanced molecular and net ionic equations for the reaction of (identify phases):

1. sulfuric acid with iron (assume iron(II) compound formation)

2. hydrobromic acid with magnesium

3. acetic acid,HC2H3O2, with zinc

I don't understand how to do these, we didn't cover oxidation in class and the chapter section is really brief and not a big help.

A 12.0 L solution contains 4.15 M Ba(NO3)2. Adding a sufficient amount of Na3PO4 to the solution will precipitate Ba3PO4. Will a precipitate form if 15.00 mg Na3PO4 is added to a given Ba(NO3)2 solution? Determine the minimum concentration of Na3PO4 needed to precipitate Ba(PO4)2 from the given Ba(NO3)2 solution.

What is a completeness of preciptation and why is it important?

Which compound will have the larger Rf value on a SiO2 TLC plate using 10% ethyl acetate/hexane as eluent: 3-decanone or 3-decanol, toluene or benzoic acid, cyclooctane or cyclooctanone? Why?

A student reacts 37g of salicylic acid with 60 mL of acetic anhydride producing 26.7g of acetyl salicylic acid. What is the percent yield of the reaction

You are the lead engineer at a bioremediation field site that is contaminated with 330 mg/L PCE, which has a molecular formula of C2Cl4. The other available electron acceptors are: oxygen at 8 mg/L, nitrate (NO3-) at 600 mg/L, Fe(OH)3 at 600 mmol/L, and sulfate (SO42-) at 250 mg/L. When these are reduced they become: water, NH4+, Fe2+, and S2-, respectively. PCE must be reduced completely to ethene (C2H4) or the local community group will protest. However, all of the other electron acceptors must be completely reduced for this to happen (i.e. everything needs to be completely reduced.) You are going to use ethanol (C2H6O) as the electron donor for all of these reactions, and it is oxidized to bicarbonate (HCO3-). What is the minimum concentration of ethanol you need to get the job done in mg/L ethanol?

1. From the Kb values for arsenate in the following equations, calculate the three Ka values of arsenic acid. (Assume that Kw is 1.01???10?14.)

a) Kb1 = 3.19???10?3

b) Kb3 = 1.76???10?12

2. A solution contains 0.0490 M Ca²⁺ and 0.0316 M Ag⁺ (The K_sp of CaSO₄ is 2.4???10^?5, and theK_sp of Ag₂SO₄ is 1.5???10^?5.)

a) What will be the concentration of Ca²⁺ when Ag₂SO₄ begins to precipitate?

I would greatly appreciate assistance with the both of these problems.

Part A) Determine the [OH−] of a solution that is 0.150 M in CO32−. Express your answer using two significant figures.

Part B) Determine the pH of a solution that is 0.150 M in CO32−. Express your answer to two decimal places.

Part C) Determine the pOH of a solution that is 0.150 M in CO32−. Express your answer to two decimal places.

1. Whereas the excitation scan showed two features (bands, or peaks), the emission scan only showed one band. Why is this?

1. What are the advantages and disadvantages to the method of internal standards?

2. If someone made a mistake while preparing the unknown by adding too much solvent and going over the mark on the volumetric flask, how would the results be affected?

3. What is the purpose of the temperature ramp in the GC program? Based on your chromatogram, was the use of a ramp successful? Why/why not?

4. The internal standard method accounted for variation in injection volume. However, in some instances it would be useful to know how much variability there was in injection volume. How could you estimate the variability in the manually injected volume?

A.Neglecting activity coefficients, calculate the pH of an aqueous solution of 5.0 x 10-7 M KOH.

B. What fraction of the total [H+ ] is derived from the autoionization of water?

Propose a detailed, step-by-step procedure for making 100-mL buffer solutions from the following: 0.100 M NaCH3CO2 and 0.100 M HCH3CO2 0.100 M HCH3CO2 and 0.100 M NaOH