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If the freezing point of the solution had been incorrectly read 0.3 degrees lower than the true freezing pont, would the calculated molar mass of the solute be too high or too low? Explain.
CaCO3 (100.1 g/mol) has a solubility of 0.018 g/100 mL in water at 35?C. What is the value of Ksp at this temperature?
Calculte w and delta E for the vaporization of 1.00 mol water at 100 degrees celsius and 1.00 atm pressure.
Calculate the concentration of all ionic species at equilibrium after adding 1 g sodium acetate to 0.1 L of a 0.1 M solution of acetic acid. Assume volume stays constant and conditions are at standard state
at 25 degrees C a saturated solution of a metal hydroxide has a pH of 9. What is the value of the solubility-product constant (Ksp) of M(OH)2 at 25 degrees C?
What is the resulting temperature when 35 g of water at 75C is mixed with 15 g of water at 15C? (The specific heat of water is 4.184 J/g x C.)
Which of the following is the most effective buffer system for a pH value of 4.45?
Sulfur dioxide (SO2) is an unwelcome result of burning soft coal in power plants. Some of the SO2 ends up as sulfuric acid in acid precipitation.
Calculate mass, mole fraction and avg. molecular weight of air, Calculate the constituent (a) mass, (b) mole fraction (c)average molecular weight of air at 25 degree centigrade, 1 atm, and molar density of all listed gases
Solid NaI is slowly added to the solution that is 0.010 M in Cu and 0.010 in Ag a) which compound will begin to precipitate first? b) calculate Ag when CuI just begins to precipitate? c) what precipitate of Ag remains in the solution at this point..
what mass of H2O is required to form 1.6 l of O2 at a temperature of 273 k and pressure of .936 atm
when NaOH is added to this solution, a white precipitate forms. Using an equation, provide the identity of the white precipitate and explain its formation.
Assume that a particular reaction evolves 241 {rm kJ} of heat and that 33 {rm kJ} of PV work is gained by the system.
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