You wish to prepare 50.00 mL of 0.0600 M NH₃ from concentrated ammonia (15.28 M) by serial dilution using a 50 mL volumetric flasks, a 1.00 mL volumetric pipet, and a 10.00 mL graduated pipet.

For the first dilution in the series, 1 mL of concentrated ammonia is added to a 50.00 volumetric flask and then filled to the line. The solution is mixed thoroughly, poured into a beaker, and then used to make the second solution in the series. What volume of the first solution should be used to make the second solution, 50.00 mL of 0.0600 M NH₃ solution

1.) Explain the following observations in terms of shifting equilibria by Le Chatelier's Principle. Write the equation for the equilibrium involved in each case.

a.) barium chromate, BaCrO4, is insoluble in basic solution but dissolves readily in acidic solution.

b.) The addition of NaOH to the iron (III)- thiocyanate equilibrium causes the red color to disappear and a rust colored precipitate to form.

c.) The solubility of lead chloride, PbCl2, in 0.10 M HCl is much lower than in pure water.

d.) Limestone, CaCO3, is an insoluble salt but will dissolve in acid.

e.) For part C, how does the rate of the reaction vary as the temperature is increased? Explain.

Balance the following skeleton reactions and identify the oxidizing and reducing agents:
MnO4-(aq) + CN-(aq) --> MnO2(s) + CNO-(aq) [basic]

Can you balance these redox equations? I am having trouble figuring out the process of adding extra products to make them work.

ClO₃^- + Cl^- -----> Cl₂ + ClO₂^-

Cr₂O₇^2- + C₂O₄^2- -----> Cr³⁺ + CO₂

Tungsten trioxide (WO3) has a rich yellow color and is often used as a pigment in ceramics and paints. In order to test a ceramic vase for its WO3 content, a 10.05 g sample of the vase was ground and reduced with Pb(Hg) to convert any WO3 to W3 . The resulting W3 was transferred to 500.0 mL of 1.00 M HCl. A 100.00 mL aliquot of the HCl solution required 13.50 mL of 0.08202 M potassium permanganate (KMnO4) to reach the purple endpoint. A blank required 0.06 mL. Balance the reaction below and determine the percent WO3 in the ceramic sample.

3. Calculate the density of NO at STP and at 20.0 C and 720 torr.

4. The volume of a mass of gas is 300 ml at 25 C and 685 torr. What volume will the gas occupy at STP?

5. Calculate the weight of hydrogen in 750 ml of hydrogen gas collected over water at 25.0 C and 0.895 atm. (vp of water at 25 C = 23.0 mm)

1. Vinegar consists of acetic acid, CH3COOH, and water. Write out the equilibrium expression for acetic acid reacting with water.

2. Citric acid, H3C6H5O7, contributes to the acidity of many foods. Write out the equilibrium expression for citric acid reacting with water to lose one acidic proton.

A scientist would like to use thermal diffusion to dope the silicon wafer. He decides to deposit 10 nm Boron on the surface and heat up the wafer to allow Boron to diffuse into the wafer. What technique do you recommend him to use to deposit high purity Boron on the surface? Explain what are the machines he could use and what kind of precursors he needs to use.

The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and oxygen. A 1.126 g sample of BHT was combusted in an oxygen rich environment to produce 3.373 g of CO2(g) and 1.105 g of H2O(g). Insert subscripts below to appropriately display the empirical formula of BHT.

Use the information provided in appendix to answer the following questions:

a) Calculate the K_b of Acetate ion

b) Calculate the pK_a of the anilinium ion (C₆H₅NH₃⁺)

c) Calculate the K_b of NO₂^-

d) Calculate the pK_b of the benzoate ion

A certain weak acid, HA, has a Ka value of 2.0×10⁻⁷.

Part A: Calculate the percent ionization of HA in a 0.10 M solution.

Part B: Calculate the percent ionization of HA in a 0.010 M solution.

Calculate the standard heat of reaction for the dehydrogenation of cyclohexane to benzene in the vapor phase.

C₆H₁₂ = C₆H₆ + 3 H₂

The reactor for this system operates at 70% conversion of cyclohexane. If the feed rate is 4000 kg of pure C₆H₁₂ per hour at 100oC, determine the rate of heat addition to or removal from the reactor that is required if the product gases leave the reactor at 300^oC.

​When a 1.50 g sample of aluminum metal is burned in an oxygen atmosphere, 2.83 g of aluminum oxide are produced. However, the combustion of 1.50 g ultrafine aluminum in air results in 2.70 g of a product, which is a mixture of 80% aluminum oxide and 20% aluminum nitride (% by mass). Use this information to determine the empirical formulas of aluminum oxide and luminum nitride.