Please write (For each) the resulting reactions, molecular equations, ionic equatons, and net ionic equations. No need to show work. Thank you!

[1] copper(II) sulfate + sodium hydroxide

[2] copper(II) sulfate + sodium carbonate
[3] copper(II) sulfate + lead(II) nitrate
[4] copper(II) sulfate + barium chloride
[5] copper(II) sulfate + sodium phosphate
[6] sodium carbonate + sulfuric acid
[7] sodium carbonate + hydrochloric acid
[8] cadmium(II) chloride + sodium sulfide
[9] cadmium(II) chloride + sodium hydroxide
[10] nickel(II) chloride + sodium acetate
[11] nickel(II) chloride + silver(I) nitrate
[12] nickel(II) chloride + sodium carbonate
[13] sulfuric acid + sodium hydroxide
[14] sulfuric acid + sodium acetate
[15] ammonium chloride + sodium hydroxide
[16] barium chloride + sodium phosphate
[17] lead(II) nitrate + sulfuric acid
[18] lead(II) nitrate + sodium sulfide
[19] sodium sulfide + hydrochloric acid
[20] potassium chloride + sodium nitrate

A mixture of gases contains 8.23 g of N2, 8.80 g of H2, and 6.96 g of NH3. If the total pressure of the mixture is 3.05 atm, what is the partial pressure of each component?

At 650 K, the reaction MgCO3(s)?MgO(s)+CO2(g) has Kp=0.026. A 12.8L container at 650 K has 1.0g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.900L .

Find the mass of MgCO3 that is formed.

Consider the titration of a 27.3 −mL sample of 0.125 M RbOH with 0.105 M HCl. Determine each of the following.

1. the initial pH

2. the volume of added acid required to reach the equivalence point

3.the pH at 5.6 mL of added acid

4. the pH at the equivalence point

5. the pH after adding 4.9 mL of acid beyond the equivalence point

You add 0.535 g of NaOH to 100.0 mL of water at 25

An organic compound contains carbon, hydrogen, and sulfur. A sample of it with a mass of 2.712 g was burned in oxygen to give gaseous CO₂, H₂O, and SO₂. These gases were passed through 311.2 mL of an acidified 0.0200 M KMnO₄ solution, which caused the SO₂ to be oxidized to SO₄^2-. Only part of the available KMnO₄ was reduced to Mn²⁺. Next, 31.12 mL of 0.0300 M SnCl₂ was added to 31.12 mL portion of this solution, which still contained unreduced KMnO₄. There was more than enough added SnCl₂ to cause all of the remaining MnO₄^- in the 31.12 mL portion to be reduced to Mn²⁺. The excess Sn²⁺ that still remained after the reaction was then titrated with 0.0100 M KMnO₄, requiring 0.02095 L of the KMnO₄ solution to reach the end point. Based upon all this data, the percentage of sulfur in the original sample of the organic compound that had been burned is___%.

The iodination of acetone, CH3COCH3, in aqueous solution is catalyzed by the hydrogen ion H+:

I2+CH3COCH3H+?HI+CH3COCH2I

The reaction can be followed visually by adding starch. The purple starch-iodine complex forms immediately, then disappears when the iodine has been consumed. The kinetics of the reaction may be determined by recording the time required for the color to disappear, which is the time required for the iodine, I2, to be consumed.

The following data were acquired in an iodination experiment involving acetone. All reaction times are in terms of the rate of disappearance of I2.

part A

In the general rate law

rate=k[I2]^X[H+]^Y[CH3COCH3]^Z

what are the values of X, Y, and Z?

how to calculate the equilibrium concentration using absorption data and the best fit line from the beer's law

5. If the sulfuric acid and nitric acid in rainwater are capable of adversely affecting soil, trees, and fish, why doesn’t this same acid adversely affect people when they walk in the rain? 6. Which do you feel is likely to be more acidic: acid rain or acid fog? Explain your reasoning.

EXPERIMENT #4 – PREPARATION OF o-CHLOROBENZOIC ACID

1. PREPARE A SOLUTION OF CuCl AS FOLLOWS: Dissolve CuSO4∙5H2O (2.34 g) and pure NaCl (0.62 g) in water (8 mL) in a 50 mL Erlenmeyer flask. Warm on a hot plate to dissolve. Add a solution of sodium bisulphite (0.56 g) in water (6 mL) to the hot solution, with constant shaking over a period of about 5 minutes. Cool to room temperature in an ice bath, and decant the supernatant liquid from the colourless CuCl. Wash the precipitate twice by decantation with water containing a little (approximately 1% (v/v) solution) sulphurous acid (HSO3 ‐ + H+ →H2SO3), to prevent oxidation. Dissolve the CuCl in concentrated HCl (4 mL). Stopper the flask and cool in an ice‐salt mixture (0‐5oC) while the diazonium salt is being prepared.

2. PREPARE A DIAZONIUM SALT AS FOLLOWS: In a 125 mL conical flask, dissolve o‐ aminobenzoic acid (anthranilic acid, 0.94 g) in a solution containing conc. HCl (1.4 mL) and water (8.2 mL). Cool the solution to 0 oC. Slowly add a cold solution of NaNO2 (0.46 g) in water (1.6 mL). Do not allow the temperature to rise above 10 oC during this procedure. Add a small amount of urea (a few crystals) to the mixture and cool the resulting solution in an ice bath.

3. PREPARE o-CHLOROBENZOIC ACID AS FOLLOWS: Transfer the cold CuCl solution to a 150 mL beaker. Slowly add, with stirring (use long glass rod), the cold diazonium salt solution to the cold CuCl solution. Watch for foaming. Allow the mixture to stand for 20 minutes at room temperature with frequent stirring. Vacuum filter the precipitated o-chlorobenzoic acid and wash the product with a small amount of cold water.

4. RECRYSTALLIZE AS FOLLOWS: Clean the Buchner funnel and place it along with a 500 mL vacuum flask into the oven at 105 oC. In a 150 mL beaker, add the crude product, a small amount of charcoal, water (~20 mL) and ethanol (~2.6 mL). Heat to a gentle boil, stirring the mixture periodically. When the product has dissolved, quickly filter through the hot Buchner funnel (PRERINSE FILTER PAPER WITH BOILING WATER) in order to remove the charcoal before the o‐chlorobenzoic acid is allowed to 26 crystallize. Allow to cool to room temperature. Vacuum filter the recrystallized product. Dissolve a few crystals of the product in ethanol and spot it on a TLC plate and label it “R”. Likewise dissolve a few crystals of anthranilic acid in ethanol and spot that on a TLC plate as well, labelling it as “SM”. Develop the TLC plate as usual, taking note of the solvent used. Determine the m.p. and percent yield of the dried product next week while doing experiment #5.

If the experiment were to be performed exactly this way, how would one determine the limiting reagent of the reaction for the percent yield calculation? What should be the limiting reagent of this reaction? When I ran this experiment, I was able to form 0.43 g of product.

Thanks for your help!

Scenario: You are an engineer supervising the work on a brownfield remediation project. Just before the close of business, as you are grabbing your coat, you notice one of your coworkers left some stock solutions out on the bench. Thinking you can quickly put them away and then go home, you walk over to do so, but you discover instead that the labels have not been put on the stock containers. There are labels on the counter, in front of the containers, but they have not been printed yet. There are four colorless glass containers, two of which contain a clear, colorless solution. The other two solutions have a dark bluish-green color. Over to the right are a number of containers that had been used recently. These containers contain chemical compounds, in solid form, that are commonly used in your lab. They are: barium nitrate, nickel (II) chloride, potassium nitrite, iron (III) nitrate, lithium sulfate, aluminum nitrate, sodium bromide, lead (II) chloride, calcium nitrate and magnesium fluoride. Can you identify the contents of the containers and put correct labels on the containers? Design a flowchart to show how you would test the solutions to determine what they might be. The flowchart must clearly list the chemicals needed for each test as well as show the expected test results.

One mole of an ideal monatomic gas is expanded from an initial state at 3 bar and 450 K to a final state at 2 bar and 250 K. There are two different paths for this expansion:
path 1: (1 mole ideal gas, 3 bar, 450 K) → (1 mole ideal gas, 3 bar, 250 K) → (1 mole ideal gas, 2 bar, 250 K)
path 2: (1 mole ideal gas, 3 bar, 450 K) → (1 mole ideal gas, 2 bar, 450 K) → (1 mole ideal gas, 2 bar, 250 K)

Part A

Specify the paths carefully.

Check all that apply.

Part B

Calculate w for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part C

Calculate q for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part D

Calculate w for the path 2.

Express your answer to three significant figures and include the appropriate units.

Part E

Calculate q for the path 2.

Express your answer to three significant figures and include the appropriate units.

Part F

Calculate ΔU for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part G

Calculate ΔS for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part H

Calculate ΔU for the path 2.

Express your answer to three significant figures and include the appropriate units.

Part I

Calculate ΔS for the path 2.

Express your answer to three significant figures and include the appropriate units.

alkynes can be hydrated in the presence of acid and HgSO4 by electrophilic addition of the molecule of water to the triple bond.The reaction proceedes by way of carbocation intermediate. Hydration of acetylene produces acetaldehyde. Outline the steps that occur in this transformation

You mix 28.0 mL of 0.298 M FeCl₃ with 39.5 mL of 0.423 M NaOH. What mass of Fe(OH)₃ (in grams) will precipitate from this reaction mixture?

One of the reactants (FeCl₃ or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)₃ has been precipitated?

Calculate the freezing point of a solution containing 13.2 gg FeCl3FeCl3 in 159 gg water.

Calculate the boiling point of the solution above.

Calculate the freezing point of a solution containing 5.9 %% KClKCl by mass (in water).

Calculate the boiling point of the solution above.

Calculate the freezing point of a solution containing 0.151m MgF2

Calculate the boiling point of the solution above.