Be sure to answer all parts.

The equilibrium constant Kc for the Reaction:

H2(g) + CO2(g) <--> H2O(g) + CO(g) is 4.2 at 1650 C. Initially 0.87 mol H2 and 0.87 mol CO2 are injected into a 4.9 L flask. Calculate the concentraion of each species at equilibrium

Equilibrium concentration of H2: ____ M

Equilibrium concentraion of CO2: ___ M

Equilibrium concentraion of H2O: _____M

Equilibrium concentration of CO: ______M

A 350.0 −mL buffer solution is 0.170 M in HFand 0.170 M in NaF.

A) What mass of NaOH could this buffer neutralize before the pHrises above 4.00?

B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?

Sodium fluoride is added to many municipal water supplies to reduce tooth decay. Calculate the pH of a 0.00307 M solution of NaF, given that the K_a of HF= 6.80 x 10^-4 at 25 degree celcius.

What is the effect of the following changes in the O2 affinity of hemoglobin? (a) A drop in the pH of blood plasma from 7.4 to 7.2. (b) A decrease in the partial pressure of CO2 in the lungs from 6 kPa (holding one’s breath) to 2 kPa (normal). (c) An increase in the BPG level from 5 mM (normal altitudes) to 8 mM (high altitudes). (d) An increase in CO from 1.0 part per million (ppm) in a normal indoor atmosphere to 30 ppm in a home that has a malfunctioning or leaking furnace.

An HNO3(aq) solution has a pH of 1.61. What is the molar concentration of the HNO3(aq) solution?

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Ethanol (C₂H₅OH) and gasoline (assumed to be all octane, C₈H₁₈) are both used as automobile fuel. If gasoline is selling for $3.19/gal, what would the price of ethanol have to be in order to provide the same amount of heat per dollar? The density and ΔH

of octane are 0.7025 g/mL and −249.9 kJ/mol and the density and ΔH

of ethanol are 0.7894 g/mL and −277.0 kJ/mol, respectively. Assume that the products of combustion are CO₂(g) and H₂O(l). (1 gal = 3.785 L)

When 0.653 L of Ar at 1.20 atm and 227°C is mixed with 0.278 L of O2 at 501 torr and 127°C in a 400. mL flask at 27°C, what is the pressure in the flask?

How many grams of each of the following per kilogram of water in your car radiator are needed to give equal protection against freezing down to -10.0 Degrees Celcius.

A: Methy Alchohol ( CH3OH) Boiling point = 64.6 C
B Ethyele glycol C2H4 )oh)2 Boiling point 197.2 C

C: In spite of the higer cost, what advantage does ethylene glycol possses over metyhly alchol as a winter antifreeze and/or suimmer coolant? Hint conisder the physical properties of each.

The B4O5(OH)4^2- ion, present in 5.0-Ml of a saturated Na2B4O5(OH)4 solution at a measured temperature, is titrated to the bromocresol endpoint with 3.25 mL of 0.291 M HCl.

a) How many moles of B4O5(OH)4^2- are present in the sample?

b) What is the molar concentration of B4O5(OH)4^2- in the sample?

c) Calculate the Ksp for Na2B4O5(OH)4 from this data.

d) What is the free energy change for the dissolution of Na2B4O5(OH)4 at this temperature?

a)Determine the limiting reagent in aspirin synthesis given 3g of salicylic acid. b)Based on your answer, calculate the maximum weight of aspirin that you could prepare. c)As is true for most "organic" reactions the synthesis you do here is an equilibrium reaction. What steps could you take to improve the yield. d)The solubility of aspirin in ethanol is approximately 40g/100 mL at room temperature. If you had a 100% yield, how many milliliters of ethanol would you need to dissolve your product for the recrystallization step?

Construct the titration curve, for the titration of 50.0 mL of 0.125 M trimethylamine with 0.175 M HCL(aq). Please draw a graph and show all work.

a) Calculate the initial pH of the solution in the flask?

b) Calculate the pH of solution mixture after 15 mL of titrant is added?

c) Calculate the pH at the equivalence volume?

d) Calculate the pH at of the mixture after 45 mL of titrant is added?

e) Calculate the pH of the mixture after 60 mL of titrant is added?

Please help.. this is problem from my review sheet for the exam and I have no idea how to do it. Please show full work so I can understand it.

You need to prepare an acetate buffer of pH 5.87 from a 0.841 M acetic acid solution and a 2.92 M KOH solution. If you have 975 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a bufer of pH 5.87? The pKa of acetic acid is 4.76.

the standard free energy change for the decomposition of two moles of hydrogen peroxide at 25^​o​ C is -224 kJ.

2H_​2O_​2(l) -> 2 H_​2O(l) + O_​2 (g)           delta G^​o = -224kJ

a.      Calculate the equilibrium constant for the reaction

b.      What is the chemical significance of the value of the equilibrium constant?

c.       The standard enthalpy change, delta H^​o , for decomposition of hydrogen peroxide is + 196.1 kJ. Determine the standard entropy change, delta S^_​​o, for the reaction at 25^o ​C?

d.      i) what is the significance of the standard free energy change?

         ii) What is the significance of the standard enthalpy change?

         iii) What is the significance of the standard entropy change?

Procedure Reaction 1: Dissolving the Copper 1. Obtain a clean, dry, glass centrifuge tube. 2. Place a piece of copper wire in a weighing paper, determine the mass of the wire and place it in the centrifuge tube. The copper wire should weigh less than 0.0200 grams. 3. In a fume hood, add seven drops of concentrated nitric acid to the reaction tube so that the copper metal dissolves completely. Describe your observations in the lab report. (Caution, Concentrated nitric acid and nitrogen dioxide are very corrosive. Either will turn your skin yellow on contact. Do not leave any spills on the lab bench or in the fume hood.) 4. When the copper has dissolved, add seven drops of distilled water to the tube. Reaction 2: Preparation of Copper(II) Hydroxide 1. Add 15 drops of 3.0 M aqueous sodium hydroxide to the tube. Make sure that the reactants are well mixed. Shake the tube carefully or gently flick the bottom of the tube with your finger. Remember that the contents of the tube may still be corrosive. 2. Add a second 15 drops of NaOH(aq), mix well, and record your observations. If you have two layers at this point it means that you have not mixed the solution well enough. 3. Centrifuge the reaction mixture. 4. The liquid at the top of the centrifuged mixture is called the supernatant while the solid is called a precipitate. Before separating the supernatant from the precipitate it is necessary to ensure that all of the copper(II) hydroxide has been precipitated. The supernatant should be clear and colorless indicating the absence of any Cu+2 ions in the solution. It should also be basic due to an excess of OH- ions. Using a clean glass stirring rod, transfer a drop of the supernatant onto a piece of red litmus paper. If the litmus paper turns blue then the solution is basic and enough NaOH has been added. If the paper does not turn blue, add more NaOH, mix well, recentrifuge, and repeat the litmus paper test until the paper does turn blue. 5. An efficient separation of supernatants and precipitates is key to obtaining a good final yield of copper. The supernatant liquid can be separated from the precipitate by expelling the air from the bulb of a Pasteur pipet, inserting the tip of the pipet into the supernatant, then gently sucking the supernatant into the pipet. If you expel air or liquid into the precipitate with the pipet, you will stir up the precipitate and will have to repeat the centrifugation step. Remove as much liquid as possible and discard it in the waste container provided on the instructor’s cart. It is better to leave a small amount of supernatant liquid than to remove some of the copper(II) hydroxide precipitate. Reaction 3: Formation of Copper(II) Oxide 1. Set up a hot water bath by placing a beaker of water on a hotplate, placing an iron ring around the beaker, and heating the water to boiling. 2. Place the centrifuge tube containing the copper(II) hydroxide into the boiling water. Carefully hold the tube with a test tube clamp so that it doesn’t get water into it. Record your observations. Reaction 4: Formation of Copper(II) Sulfate 1. Add 20 drops of 3.0 M H2SO4 to the solid in the centrifuge tube. Stir carefully to ensure that the copper(II) oxide dissolves completely. Complete dissolution of the mixture will require thorough mixing and possibly heating of the solution. 2. Obtain the mass of a small, clean, glass test tube as accurately as possible. 3. Transfer the liquid from the centrifuge tube into the test tube. Rinse the centrifuge carefully with 1.0 mL of distilled water and transfer the rinse into the test tube containing your sample. 4. Record your observations on the data sheet. Reaction 5: Formation of Copper Metal 1. Add a small quantity of zinc powder to the sample solution. Continue adding zinc in small quantities until the solution loses the blue copper(II) color. Any excess zinc added will need to be removed so don’t add it too quickly or in large quantities. When the solution has turned colorless, add several drops of 3.0 M H2SO4 to the tube to dissolve any left over zinc. You can tell that the zinc has dissolved when addition of sulfuric acid does not generate bubbles. 2. Allow the copper metal to sink to the bottom of the tube and carefully remove the supernatant liquid using a Pasteur pipet. 3. Wash the red-brown copper metal in the tube with 1.0 mL of water. Allow the copper metal to settle to the bottom and remove the excess water. Repeat this rinsing process two more times. 4. Describe your observations on the data sheet. Drying the copper metal 1. After removing as much of the third rinse water as possible you are ready to dry the metal. This must be done carefully in a cool Bunsen Burner flame. If the tube is heated too quickly there is a risk of ejecting the contents of the tube as the water boils. Also, if the flame is too hot you may convert the copper metal back into black copper(II) oxide. The objective is to drive the water from the tube as steam. Make sure that as water condenses on the walls of the tube that you continue to heat until all of the water if gone from the tube. 2. Once all of the water is removed from the tube, cool the tube and its contents then determine the mass of copper by weighing the tube and subtracting the tube + copper weight from the weight of the empty tube (Reaction 4 step 2). If the mass of copper is higher than the original mass of the copper wire it either contains water or zinc or has been converted to copper(II) oxide. Excess water can be removed by reheating the tube and reweighing to constant mass. Excess zinc requires addition of sulfuric acid followed by re-rinsing with water and re-drying. Chemistry 1215 Experiment 9 Lab Report Name ______________________________ Data Sheet Mass of copper wire _______________ Mass of clean, dry test tube _______________ Mass of test tube plus copper _______________ Mass of final copper sample _______________ Percent recovery of copper. Show all calculations. Observations 1. Describe your observations for Reaction 1 including colors, gases formed, etc. 2. Describe your observations for Reaction 2 including colors, gases formed, etc. 3. Describe your observations for Reaction 3 including colors, gases formed, etc. Estimate the temperature of the decomposition of Copper(II) hydroxide. 4. Describe your observations for Reaction 4 including colors, gases formed, etc. 5. Describe your observations for Reaction 5 including colors, gases formed, etc. Write a brief discussion of your results including a statement of the final percent recovery of copper and a discussion of reasons why the recovery differs from 100%. Chemistry 1215, Experiment #9; Copper and its compounds, Pre-lab Name ____________________________________ 1. Write a balanced chemical equation including phase labels for the reaction between aqueous copper (II) nitrate and aqueous sodium hydroxide. 2. Nitrogen monoxide (NO) and nitrogen dioxide (NO2) are toxic, corrosive gases that significantly lower blood pressure when inhaled. How are these gases produced in today’s experiment? What should you do to protect yourself against their toxicity? 3. Iron reacts with oxygen from the atmosphere to produce iron (III) oxide, also known as rust (Fe2O3). What chemical species is oxidized in this reaction? What is the reducing agent? Jaffrey Zagnut couldn’t find any nitric acid so he tried to dissolve his copper sample in hydrochloric acid instead. Unfortunately his copper wouldn’t dissolve in HCl. Why will copper dissolve in nitric acid but not in hydrochloric acid (after all, HCl is a stronger acid than HNO3). Chemistry 1215, Experiment #9; Copper and its compounds, Post-lab Name ____________________________________ 1. Copper (II) hydroxide is converted into copper (II) oxide by heating the test tube containing Cu(OH)2 in a hot water bath. Is it necessary to use distilled water in this water bath? Why or why not? 2. Copper metal doesn’t “rust” in the presence of oxygen at room temperature. However, it will react with O2 at elevated temperatures. Write a balanced chemical equation describing the formation of copper (II) oxide when copper metal is heated in air. 3. When zinc is dissolved in sulfuric acid a gas is produced. What is the chemical identity of this gas? How is it produced? 4. Jaffrey Zagnut started with a 0.032 g sample of copper which he took through the series of reactions described in this experiment. At the end of the experiment he obtained 0.038 g of a black product. What was his percent yield? What is the most likely source of the error in his experiment? (Hint: consider question 2 above)