b) Methoxide ion, CH3O , and amide ion, NH2 , are very strong bases commonly used in organic solvents. However, both bases are

1) What volume of 17.4 M acetic acid should be used to produce 0.100 L of 3.00 M acetic acid solution?

2) Given the following thermochemical equation, how much total energy is released when 1.50 kg of CH₄ is combusted?:
CH₄ (g) + 2O₂ (g) -----> CO₂(g) + 2H₂O (l)

Thank you!!

Starting with the 0.1250M Cu(NH3)+2 as the stock (concentration) calculate the following concentrations of the dilute solutions showing work:

15mL stock diluted to 20mL

10.0mL of stock solution diluted to 20.0mL

5.0mL of the stock solution diluted to 20.0mL

Demonstrate by a “microstate analysis” that four electrons in a degenerate set of three p‐orbitals gives rise to the same electronic state

113 “terms” as two electrons do (i.e. ¹D, ¹S and ³P)

2.5 grams of a metallic sample containing an unknown amount of zinc is dissolved in 500 ml of acidic water, releasing the zinc into the water as Zn²⁺ ions. A 10.00 ml aliquot of this solution is extracted with 10 ml of CCl₄ containing an excess of 8-hydroxy quinoline. The CCl₄ and aqueous phases separate and 8-hydroxy quinoline forms a fluorescent complex with Zn²⁺ ions that partitions entirely into the CCl₄ phase. The CCl₄ phase is separated and then diluted to 25 ml. This solution gives a fluorescence intensity of 155 (arbitrary units). A similar procedure is done with 10.00 ml of the unknown zinc solution plus 8.00 ml of an aqueous 2.50 ppm Zn²⁺ solution, and the final fluorescence intensity is 247. Calculate the Zn²⁺ concentration in the original 500 ml solution and the amount of zinc in the original solid.

A sample of an unknown gas with a mass of 4.67 goccupies a volume of 1.88 L at a pressure of 785 mmHg and a temperature of 20.0 ∘C. Molar mass=57.9 g/mol. If the unknown gas is composed of 3.86 g of carbon and the rest is hydrogen, what is its molecular formula?

Choose the answer which lists ionic compounds RbBr, SrCl2, SrBr2, and RbCl in order of increasing lattice energy (smallest lattice energy listed first). Be sure to show how you found the lattice energy for each element

A reaction is found to ahve a forward activation energy of 150 kj and an exothermic enthalpy of reacton (delta H = -250kJ). FInd teh activaiton energy for the reverse reaction.

What am I doing wrong in this titration problem?

Calculate the ph at the equivalence point for the following titration 0.20M HCl versus 0.20M methylamine (CH3NH2). The Ka of methylammonium is 2.3x10^-11.

First I have to divide .20M methylamine by 2 (Why?) to get .10M

Then, I set up the equilibrium:

(2.3 x 10^-11) = x^2 / .10M

Since the ka is SO small, I just multiplied .10 with (2.3 x 10^-11) to get 2.3x10^-12, which is wrong.

Why is this wrong? Since the Ka is small, the approxiamation method should work and I won't need to do the quadratic. Instead, I am told that the x value is 1.5x10^-6 from the quadratic.

Find the pH of a solution prepared from 1.0 L of a 0.20 M solution of Ba(OH)₂ and excess Zn(OH)₂(s). The Ksp of Zn(OH)₂ is 3×10⁻¹⁵ and the Kf of Zn(OH)₄²⁻ is 2×10¹⁵.

1. An aqueous solution of sodium hydroxide is standardized by titration with a 0.108 M solution of perchloric acid.

If 17.0 mL of base are required to neutralize 29.4 mL of the acid, what is the molarity of the sodium hydroxide solution?

______ M sodium hydroxide

2. An aqueous solution of potassium hydroxide is standardized by titration with a 0.130 M solution of nitric acid.

If 23.3 mL of base are required to neutralize 15.8 mL of the acid, what is the molarity of the potassium hydroxide solution?

________M potassium hydroxide

3. An aqueous solution of hydrobromic acid is standardized by titration with a 0.140 M solution of barium hydroxide.

If 27.7 mL of base are required to neutralize 26.9 mL of the acid, what is the molarity of the hydrobromic acid solution?

_______M hydrobromic acid

Refer to the reaction 2Mg + O2---> 2MgO

starting amounts 1.25mg 2Mg, and 25g of O2. What are the changes that occur in this reaction as its happening? Complete an ice table using the starting amounts and referring to the reaction above.

*I have no idea how to do these, in the words of Micheal Scott, "Why don't you explain this to me like I'm 5 years old."*

In the laboratory, a general chemistry student measured the pH of a 0.530 M aqueous solution of codeine, C18H21O3N to be 10.820. Use the information she obtained to determine the Kb for this base.

Which choice is expected to form (a) the strongest and (b) the weakest ionic bond (choices listed as strongest/weakest)?

Options:

Na+ & Cl-, Cs+ & Cl-, Cs+ & Br-, Ca2+ & Cl-,

Ca2+ & O2-, Sr2+ & O2-, Sr2+ & Cl-, Sr2+ & Br-