Use Tanabe-Sugano diagrams to predict the number of transitions for the following species:
a) Mn(H2O)6 ^2+
b) Cu(H2O)6 ^2+
c) Fe(CN)6 ^3-

1. Calculate [OH−] for a solution formed by adding 5.00 mL of 0.120 M KOH to 20.0 mL of 7.1×10⁻² M Ca(OH)2.

2. Calculate pH for a solution formed by adding 5.00 mL of 0.120 M KOH to 20.0 mL of 7.1×10⁻² M Ca(OH)2.

3. Pyridine is a weak base that is used in the manufacture of pesticides and plastic resins. It is also a component of cigarette smoke. Pyridine ionizes in water as follows:

C5H5N+H2O⇌C5H5NH++OH−

The pKb of pyridine is 8.75. What is the pH of a 0.430 Msolution of pyridine?

4. Benzoic acid is a weak acid that has antimicrobial properties. Its sodium salt, sodium benzoate, is a preservative found in foods, medications, and personal hygiene products. Benzoic acid dissociates in water:

C6H5COOH⇌C6H5COO−+H+

The pKa of this reaction is 4.2. In a 0.79 M solution of benzoic acid, what percentage of the molecules are ionized?

The common-ion effect and solubility The solubility of a slightly soluble compound can be greatly affected by the addition of a soluble compound with a common ion, that is, with one of the ions in the added soluble compound being identical to one of the ions of the slightly soluble compound. The general result of the addition of the common ion is to greatly reduce the solubility of the slightly soluble compound. In other words, the addition of the common ion results in a shift in the equilibrium of the slightly soluble compound. Part B - Calculate the molar solubility in NaOH Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.110 M NaOH?

1. Interpret the infrared and NMR spectra of benzocaine.

2.What is the structure of the precipitate that forms after the sulfuric acid has been added?

3. When 10% sodium carbonate solution is added, a gas evolves. What is the gas? Give a balanced equation for this reaction.

4. Explain why benzocaine precipitates during the neutralization.

5. Refer to the structure of procaine in the table in the essay “Local Anesthetics.” Using p-aminobenzoic acid, give equations showing how procaine and procaine monohydrochloride could be prepared. Which of the two possible amino functional groups in procaine will be protonated first? Defend your choice. (Hint: Consider resonance.)

For each of the following oxidation – reduction reactions, identify which element is being oxidized and which is being reduced? a. Ca (s) + 2H2O (l)  Ca(OH)2 (s, aq) + H2 (g) b. H2 (g) + F2 (g)  2HF (g) c. 4Fe (s) + 3O2 (g)  2Fe2O3 (s) d. 2Fe (s) + 3Cl2 (g)  2FeCl3 (s)

Describe how you could separate and purify compound A from a mixture of two neutral compounds (A and B) when A comprises 95% of the total and B the other 5% of the total. Assume that A and B have similar polarities.

What is the pH of 250.0mL solution that is 0.0955 M HCH3CO2 (Ka=1.8x10-5) and 0.125 M NaCH3CO2?

a. Now, 20.0 mL of 0.455 M HCl (aq) is added to the original buffer.

i. Write the neutralization reaction (use the actual species in the reaction).

ii. Find the moles of all species. iii. Build a stoichiometry table with the reaction and the data (or anything that shows what happens in the reaction).

iv. What is the pH of the solution? Was your prediction correct?

v. Do you still have a buffer? Why?

Ascorbate and copper ions have the following electrochemical potentials:

Dehydroascorbate+2H⁺+2e⁻→Ascorbate ε^∘′=+0.08V

Cu²⁺+e⁻→Cu⁺ ε^∘′=+0.159V

10 mL of a 0.02 M solution of ascorbate in a buffered solution at pH7 at 25∘C is mixed with 10 mL of 0.02 M of Cu²⁺. Figure out the equilibrium concentration of dehydroascorbate, ascorbate, Cu²⁺, and Cu⁺.

1. In a bomb calorimeter, reactions are carried out

a. at 1 atm pressure and 25

What is the percentage of Fe2O3 in a sample of limonite ore if the iron from a 0.5000-g sample is reduced and titrated with 35.15 ml of a potassium dichromate solution of which 15.00 mL is equivalent in oxidizing power to 25.00 mL of a potassium permanganate solution which has an iron value of 0.004750 g?

Question 3

1) What is the H+ concentration for an aqueous solution with pOH = 4.09 at 25 ∘C? Express your answer to two significant figures and include the appropriate units.

2)

Arrange the following aqueous solutions, all at 25 ∘C, in order of decreasing acidity.

Rank from most acidic to most basic. To rank items as equivalent, overlap them.

Ph=5.45 POH=8.55 .0018MKOH .0023 M HCL

3)

At a certain temperature, the pH of a neutral solution is 7.33. What is the value of Kw at that temperature?

Express your answer numerically using two significant figures.

How are lithium ion batteries different from regular batteries?

How does this allow for a rechargeable battery?

Assuming standard conditions, answer the following questions.
(If hydrogen is one of the reagents, assume acidic solution.)

a) Is Fe²⁺(aq) capable of oxidizing Cr metal?
b) Is H₂(g) capable of reducing Ni²⁺(aq)?
c) Is Cr³⁺(aq) capable of oxidizing Fe²⁺(aq) to Fe³⁺(aq)?
d) Is H₂(g) capable of reducing Ag⁺(aq)?
e) Is Fe²⁺(aq) capable of reducing VO₂⁺(aq)?
f) Is Sn²⁺(aq) capable of oxidizing Fe²⁺(aq)?

I got yes, no, no, yes, no, no but it's wrong.
Guidance & help for this question would be greatly appreciated.
Thanks!

Calculate the pH at 25°C of a 0.94 M solution of lidocaine HCL (C14H21NONH2Cl). Note that lidocaine is a weak base with a PKB of 7.94. Round answer to 1 decimal place.

a) A student A weighed .50 Ca(OH)2 for his saturated solution and student B weighed 0.23 g, Both students dissolved it in 60 ml of water and both had solid left in their solution before filtrating. After filtrating to a clear solution, which student had the most concentrated solution? What would the effect on the volume of HCl titrant used and the calculated Ksp of the reaction if one of the students had a couldy solution after filtering and proceeded to titrate it compared to a clear solution?

(b) A saturated solution of CA(OH)2 is prepared and filtered. If 9.32 mL of 0.045 M HCl is used to titrate a 10 ml sample of the solution to end point:
- how many moles of Ca^2+, OH- were in the original 10 mL sample
- what are the concentrations of Ca^2+ and OH- in the saturated solution?
- what is the molar solubility for Ca(OH)2 under these conditions?
- Calculate Ksp for Ca(OH)2 under these conditions

(c) If change in entropy of the universe can tell us whether a process will be spontaneous, why do we need delta G (Gibb's free energy)