Describe a way in which you use organic compounds in your home or work environment. Choose a compound that is classified as an amide, amine, thiol, carboxylate, and halocarbon. Let’s see how many different examples can be described.
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1. The mole fraction of an aqueous solution of calcium sulfate is 0.225. Calculate the molarity (in mol/L) of the calcium sulfate solution, if the density of the solution is 1.05 g mL-1.
2. Determine the mole fraction of potassium acetate in a 7.19 M aqueous solution of potassium acetate. The density of the solution is 1.30 g mL-1.
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Identify the priincipal intermolecular forces in each of the following substances: HF, C4H8, NCl3, Br2, HI
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Calculate the volume (in mL) of 0.170 M NaOH that must be added to 341 mL of 0.0555 M 3-(N-Morpholino)propanesulfonic acid (MOPS) to give the solution a pH of 7.55. The pKa of MOPS = 7.18.
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In a Sodium Borohydride reduction of 9-fluorenone to 9-fluorenol, methanol is used as the solvent because it will not react with the products and reactants and because the products and reactants are very sluble in methanol. Would 2-propanone also be a suitable solvent for this reaction? Why/Why not?
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what would you expect the vapor temperature to be after collecting 5ml of distillate in a mixture containing 10ml of acetone (bp 56C) and 10ml of water (bp 100C) for a fractional distillation? What would the vapor temperature be in a simple distillation?
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Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 ∘C of 1.0×10−5s−1.
Calculate the partial pressure, in atm, of O2 produced from 1.15 L of 0.592 M N2O5 solution at 45 ∘C over a period of 24.3 h if the gas is collected in a 12.1-L container. (Assume that the products do not dissolve in chloroform.)
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As a technician in a large pharmaceutical research firm, you need to produce 400. mL of 1.00 M a phosphate buffer solution of pH = 7.36. The pKa of H2PO4− is 7.21. You have 2.00 L of 1.00 M KH2PO4 solution and 1.50 L of 1.00 M K2HPO4 solution, as well as a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution?
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Can an alkene have the same formula as a cycloalkane? Explain.
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All amino acids have a carboxylic group and amino group. Why is it impractical to try and determine the pKa of the carboxylic group?
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Calculate the pressure exerted by 2.64 moles of CO2 confined in a volume of 4.09 L at 454 K. What pressure is predicted by the ideal gas equation? The van der Waals constants for CO2 are a = 3.59 atm · L2/mol2 and b = 0.0427 L/mol.
van der Waals equation:
Ideal gas equation:
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What is the function of bile salts in digestion?
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Which of the following redox reactions do you expect to occur spontaneously in the reverse direction? (Hint: The reactions are occurring under standard conditions (1 M for the aqueous ions).)
Check all that apply.
| 2Ag+(aq)+Ni(s) ? 2Ag(s)+Ni2+(aq) | |
| Ca2+(aq)+Zn(s) ? Ca(s)+Zn2+(aq) | |
| 2Al(s)+3Pb2+(aq) ? 2Al3+(aq)+3Pb(s) | |
| Fe(s)+Cr3+(aq) ? Fe3+(aq)+Cr(s) |
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Calculate the pH for the titration of 40.00ml of 0.1000M solution of ethylamine (C2H5NH2) with 0.1000M HCl for the following volumes of added HCl: Kb for ethylamine = 6.4X10-4
Volumes; 0.00ml; 20.00ml; 40.00ml and 50.00ml
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Fundamentals Of Analytical Chemistry 9th Edition - Skoog
Balance the net ionic equation of the following redox reaction using half-reaction method. Show the steps.
Cr(OH)3 + ClO3- --------> CrO42- + Cl- (basic medium)
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