How many unpaired electrons are in the following transition metal ions in an octahedral crystal field? Part 1(1 pt) High-spin Fe3+ unpaired electron(s) Part 2(1 pt) Cu+ unpaired electron(s) Part 3(1 pt) V3+ unpaired electron(s) Part 4(1 pt) low-spin Mn3+ unpaired electron(s)

Match the following aqueous solutions with the appropriate letter from the column on the right. Assume complete dissociation of electrolytes.

Rank the following molecules or ions in order of decreasing bond length using their bond order to predict relative lengths.

- oxygen difluoride (bond order = 1)

- O2 (bond order = 2)

- carbon monoxide (bond order = 3)

13.) Redox chemistry isn’t only for chemists, it’s important in biology as well. Below are two different redox forms of Vitamin C. Oxygen lone pairs are omitted for clarity. a) Identify the oxidation states of the carbons that change oxidation state for both molecules. How many electrons are transferred when these forms interconvert? b) From a redox perspective (ignore acid/base aspects), would H2 or O2 be more likely to change Ascorbic Acid into Dehydroascorbic Acid? Briefly explain your choice.

A-CH3SH reacts with CO according to the following unbalanced chemical equation:

CH3SH + CO → CH3CO(SCH3) + H2S

Calculate the mass in grams of the excess reagent remaining after the complete reaction of 2.17 g of CH3SH with 1.45 g of CO. ( )

B- a compound containing only C, H and O was subjected to combustion analysis. A sample of 4.270×10¹ g produced 9.200×10¹ g of CO₂ and 3.766×10¹ g of H₂O. Determine the empirical formula of the compound and enter the appropriate subscript after each element.

C( ) H( ) O( )

If the molar mass of the compound is 204.266 g/mol, determine the molecular formula of the compound and enter the appropriate subscript after each element.
C( ) H( ) O( )

You have available the buffer ADA: disodium salt a) using the buffer, explain, in some detail including numerical calculations, how to prepare 500ml of a buffer with a pH=6.50 and a total concentration of 50.0mM for the acid and conjugate base. b) What volume of either the NaOH or HCl solutions would you need to add to change the pHof 100mL of the buffer to pH 6.00

Explain, briefly one of the phenomena below and describe how it relates to quantization of energy. (a) the photoelectric effect OR (b) line (emission) spectra

Will a precipitate occur when 12.0 mL of 0.00035M silver chlorate and 15.0mL of 0.00150M sodium carbonate are mixed?

Fe²⁺ is present at very low concentrations in seawater. The primary source of this iron is Fe(OH)₂. The pH of seawater is between 7.4 and 8.3. For this problem assume that the pH of seawater is 8.0.

a) Write a chemical equation that describes the solubility of Fe(OH)_2.

b) Knowing that ΔGº for this reaction is 90.7 kJ/mol, calculate the K_sp of Fe(OH)₂.

c) What is the solubility of Fe(OH)₂ in pure water?

d) What is the solubility of Fe(OH)₂ in seawater?

I need to know how to do these questions not just the answers, thank you!

1. Use the Henderson-Hasselbalch equation to determine the ratio of base/acid in a formic acid-formate buffer with a pH of 3.00

2. Assume that the human blood buffer includes, at any one point, 0.00080 M carbonic acid and 0.0080 M hydrogen carbonate. What is the pH of 7.00 liter of blood under these conditions?

3. Metabolic acidosis results in the addition of excess acid to blood. How many moles of strong acid must be added to the blood in question 2 to bring the hydrogen carbonate/ carbonic acid ratio to the hazardous level of 5:1 and what would the pH be?

The constant pressure molar heat capacities of linear gaseous molecules are approximately (7/2)R and those of non-linear gaseous molecules are approximately 4R. Estimate the change in the standard reaction entropy of the reaction forming liquid water from oxygen and hydrogen gas when the temperature is increased by 10K at constant pressure.

The chemical reactions:
CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) The copper on the surface quickly reacts with oxygen according to the following reaction: 2Cu(s) + O2(g) → 2CuO(s)

Experimental Procedure Dissolve
completely about 0.5 to 0.7 g of copper (II) sulphate pentahydrate in about 10 to 20 mL of deionized water. Calculate the amount of zinc powder that must be added to a copper sulfate solution so that the sulfate completely reacts. This calculated mass of zinc, plus an extra 0.01 g, is added to the copper sulfate. Stir. When the reaction appears to be complete (what signifies this?), add enough sulfuric acid to create a colourless solution. What is the purpose of this step? Suction filter the final product. Wash with about 5 mL of ethanol. Maintain suction for about 10 minutes. Determine the mass of the final product to 2 significant figures. Reagents 0. 6 g Copper (II) sulfate pentahydrate (CuSO4(s)) (FW = 249.68) Zinc powder (FW = 65.41) Sulfuric acid (1.5 M H2SO4(aq)) Ethanol

Data Mass of CuSO4 = 0.61g Mass of Zn = 0.17g Mass of empty watch glass = 48.72g Mass of watch glass and Cu = 48.91g

Questions:

1. Please show the calculation for the amount of Zn added to the reaction mixture and for the percentage of Cu recovered from the original copper sulfate sample (theoretical yield).

2. What is the purpose of adding enough sulfuric acid to create a colorless solution?

1. What are the critical differences among spectroscopy, spectrometry and spectrophotometry?
2. What kinds of parameters are critical for the physical properties of electromagnetic wave radiation?
3. What is the dual property of the light (electromagnetic wave)?

In the laboratory you dissolve 15.0 g of iron(III) nitrate in a volumetric flask and add water to a total volume of 250 mL.  

What is the molarity of the solution?   M.

What is the concentration of the iron(III) cation?   M.

What is the concentration of the nitrate anion?   M.