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744.5 g of a nonelectrolyte are completely dissolved in sufficient water to make 1.50 L of an aqueous solution at 25.0oC. The osmotic pressure of the solution is 59.9 atm. What is the molar mass of
Use the dipole moments of HCl and HF ( HCl = 1.08, HF = 1.82) together with the percent ionic character of each bond ( HCl = 20% ionic, HF = 45% ionic) to estimate the bond length in each molecule.
An aqueous solution is 22.0% by mass ethanol, CH3CH2OH, and has a density of 0.966 g/mL. What is molality of ethanol
What would you run as controls to be certain the ferric chloride test was working as predicted? What results would you expect for your control tubes?
An unidentified organic compound X, containing C,H, and O was subjected to combustion analysis. When 228.4 mg of pure X was burned 627.4 mg of CO2 and 171.2 mg of H2O were obtained. Determine the si
At room temperature however, aspirin is not soluble in this particular solvent but all the impurities remain soluble. Describe how to use this solvent to purify aspirin crystals away from the impuri
What is the pH at the point during a titration when 34 mL of 0.200 M HCl has been added to 33 mL of 0.0500 M NH3 solution? HCl is strong acid, Kb = 1.8 × 10-5 for NH3.
A 4.70 g nugget of pure gold absorbed 278 J of heat. The initial temperature was 28.0°C. What was the final temperature?
Calculate the heat that must be supplied to 10.8 g of Ne at .15 atm to raise its temperature from 28C to 51C at constant pressure. Assume that neon behaaves as an ideal gas.
When 25.0g os H2O reacts with 65g of Fe, which is the limiting reactant? How much excess reactant is used when the reaction is completed? What mass in grams of black iron oxide is produced?
What is the boiling point of a mixture composed of 95.0 g HOCH2CH2OH (ethylene glycol) and 205 g H2O? The boiling point elevation constant for H2O is 0.512 °C/m.
A solution is prepared by adding 60.0 mL of 0.060 M HBr to 180.0 mL of 0.70 M HI. Calculate the concentrations of all species in this solution. HBr and HI are both considered strong acids.
0.158g of a barium halide is completely precipitated out of H2SO4 and 0.124g of barium sulfate are produced. What is the true formula of the compound?
A solid sample containing some Fe+2 ion weighs 1.062g. It requires 24.12mL 0.01562 M KMnO4 to titrate the Fe+2 in the dissolved sample to a pink end point. How many grams of iron are there in the sa
A 265- flask contains pure helium at a pressure of 755 . A second flask with a volume of 465 contains pure argon at a pressure of 712 .If the two flasks are connected through a stopcock and the stop
A stock solution is prepared by adding 25 mL of 2.2 M AlCl3 to enough water to make 75 mL. What is the Cl- concentration of 25 mL of the stock solution?
Calculate the temp in degree celcius after thermoequillibrium is reached, assume no heat lost to the surroundings. The enthalpy of fusion of ice is molar heat = 6.007 kJ/mol, and the molar heat capa
The total molarity of acid and conjugate base in this buffer is 0.100 . A student adds 9.00 of a 0.250 solution to the beaker. How much will the pH change? The of acetic acid is 4.760.
A 1.000 g sample of a compound containing C, H and O is burned in excess oxygen, producing 1.783 g CO2 and 0.734 g H2O. Determine the empirical formula of the compound. A. B. C. D. E. C4H12O4 C3H6O
When Dr. Farrell was a graduate student, he prepared a buffer of pH = 8.0 from Sodium Acetate. Why would the casual observer to this buffering faux pas think he had the intellectual agility of a sm
Use the initial volume of acetic acid, the volume of NaOH required to reach the equivalence point and the value of the molarity of NaOH that you obtained when you standardized this solution against
If a 128 gram sample of H2O at 75 degrees Celsius were mixed with a 55 gram sample of H2O at 38 degrees Celsius, what would the final temperature of the mixture be?
solution of water (K_f}=1.86 C/m) and glucose freezes at - 2.35 C. What is the molal concentration of glucose in this solution? Assume that the freezing point of pure water is 0.00 C.
How many alpha and beta particles are emitted in the decay series that begins with 237Np and finally produces the stable isotope 209Bi?