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Will a precipitate of Cu(OH)2 (Ksp = 1.6x10-19) form when 10.0 mL of 0.010 M NaOH is added to 1.00 L of a 0.010 M CuCl2 solution
Calculate the maximum amount of thorium ion that could be present in a waste water, if it is made 0.1500 M in oxalate ion. Assume the oxalate is present in stoichiometric amount, compared to the tho
Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to 20.0 mL of 0.100 M NH3
The solubility of O2 in water is 0.590 g/L at an oxygen pressure of 15 atm. What is the Henry's law constant for O2 (in units of L atm/mol)
For a solution of hexane (C6H14) and chloroform (CHCI3), would you expect it with respect to Raoult's law to be relatively ideal, to show a positive deviation, or to show a negative deviation
what is the boiling-point change for a solution containing 0.360 mol of naphthalene (a nonvolatile, nonionizing compound) in 256.0 g of liquid benzene? (Kb=2.53 celsius/m for benzene).
Calculate the osmotic pressure (in torr) of 5.48 L of an aqueous 0.136 M solution at 25 celsius if the solute concerned is totally ionized into three ions (for example, it could be Na2SO4 or MgCI2).
Write net Bronsted equations that show the acidic or basic nature of the following substances, given the pH. For polyprotic acids, only show one proton transfer. Remember that spectator ions are not
calcualte the pH at one-half the equivalence pont and at the equivalence point for a titration of 50 mL of 0.100M acetic acid with 0.100M NaOH
what is the equilibrium pressures for each of the gases if the initial partial pressures are PHF = .500 atm, PH2=1.00x10^-3 atm, and PF2=4.00x10^-3 atm
Write a mechanism for the reaction of an alkyl halide with alcoholic silver nitrate which depicts the type of substitution which occurs. Explain how this mechanism accounts for the relative rate of
The largest estimate for the amount of water on the moon is currently 1000parts per million (i.e 1000g water per 1000000g of salt). if the moon is made primarily of a pyroxene mineral with formula F
A student is conductiong this experiment, but forgets to temper the lid. therefore it breaks while the hydrate is being heated. the student thinks carefully and replaces the old lid with a new one,
Explain how the calculated formula of the hydrate would be changed if water from the air is absorbed by the hot dry sample as it cools.
In the electrolysis of KI, NaBr, pure elemental iodine potassium, and soduim cannot be isolated. Discuss by using equation I2(s) I^-(ag)>I3^-(ag) Iodine equation
Calculate the standard free energy change and the equilibrium constant for the following reaction at 25°C: (all aqueous solutions are 1 M) Au(s) + Ca2+ (aq) ? Au3+(aq) + Ca(s)
Using terms in the Hartree-Fock energy expression, explain why the lowest-energy triplet state of the He atom is higher in energy than the singlet state.
What wavelength is expected for light composed of photons produced by an n=3 to n=1 transition in a hydrogen?
Calculate the concentration of each reactant in trials 1 through 5 after the flasks contents have been combined but before the reaction takes place.
what is the pH of a solution made by adding 5.42grams of potassium nitrite, to 727mL of .178 M nitrous acid(assume no change in volume takes place) and what is the pH of the solution after adding 49
We electrolyze a solution containing M2O7(3-) for 43.30 hr using a current of 2.685 amp to isolate M(s), which has an atomic weight of 215.22. How many grams of M(s) will be produced if we operate t
The value of Ka in water at 25 degrees Celcius for benzoic acid, C6H5COOH (aq), is 6.3 x10-5 M. Calculate the pH and the concentration of the other species in a 0.0200-M aqueous solution of C6H5COOH
why during a GC is the boiling point for some samples higher than the final temperature used during the run yet these samples still run
Report each to three significant figures in scientific notation. Given this data for the decomposition of urea in an acidic solution, calculate each of the following assuming Arrhenius behavior.