How many ions results from the ionization of one molecule in water solutions?

The freezing point of an aqueous solution of barium nitrate is -2.65°C. Determine the apparent molal concentration of barium nitrate.

A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute solution. The vapor pressure of pure CCI4 is 33.85 torr at 298 K. The Henry's Law constant when the concentration of Br2 is expressed as a mol fraction is 122.36 torr. Calculate the mole fraction of Br2 in the vapor when it's in equilibrium with a solution that has a mole fraction of Br2 equal to 0.050, having the assumption that the vapor still behaves as an ideal gas.

A 1.10 g sample of an unknown compound reduces the freezing point of 75.22 g benzene from 5.53 to 4.92 ºC.  What is the molar mass of the compound?                       The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is -0.072 ºC.  What would you expect the normal boiling point of this same solution to be?                         Predict the approximate boiling points of 0.10 m solutions of the following solutes dissolved in water (Kb (H2O) = 0.512 ∞C/m): Al(NO3)3 (aluminum nitrate)   CH2O (formaldehyde)   RbI (rubidium iodide)   C6H6 (benzene)               Calculate the van’t Hoff factor, i, for the following weak electrolyte solution: 0.050 m HCHO2, which begins to freeze at -0.0986 ∞C.                           Calculate the vapor pressure at 25 ∞C of a solution containing 255 g of the nonvolatile solute, glucose, C6H12O6, in 1.50 kg of H2O.  The vapor pressure of water at 25 ∞C is 23.8 mmHg.                           Calculate the…

At a certain temperature the vapor pressure of pure benzene and pure toluene are 380 torr and 130 torr, respectively. If the mole fraction of benzene is 0.48, what is the total vapor pressure.

At a certain temperature the vapor pressure of water is 25.0 torr. A glucose solution is prepared by mixing 5.00 g of glucose and 2.00 moles of water. What is the expected vapor pressure of the solution? Molar mass of water = 18.02 g/mol and molar mass of glucose = 180.2 g/mol a) 0.342 torr b) 3.05 torr c) 22.0 torr d) 24.7 torr

A metal, M, of atomic mass 96 amu reacts with fluorine (19 amu) to form a salt that can be represented as MFx.To determine x, you decide to dissolve 9.18 g of the unknown MFx solid in 100.0 g of water and measure thefreezing point depression. You found that the freezing point for this solution was -4.46°C. Assuming the saltcompletely dissolves and dissociates in solution and the freezing point of water 0.00°C, determine the formulaof the salt (i.e. what is the value of x).

A 10.00 mL sample of ethanol is added to 250.0 mL of water in order to observe the freezing point depression of the water. Consider the possible errors in this experiment, and determine whether each would cause the freezing point of the water to increase, decrease, or remain the same compared with the expected results. It is discovered that the 10.00 g ethanol sample is actually 95% ethanol and 5% water.   The ethanol sample is left out for several minutes before being added to the water, allowing a significant amount to evaporate.   Instead of starting the experiment with room temperature water, the experiment is started with cold water.   Some of the water is splashed out of the container before the ethanol is added.   Some of the ethanol and water solution is spilled out of the container during temperature measurement.

The normal boiling point of a certain liquid X is 121.00 °C, but when 0.12 kg of benzamide (C,H,NO) are dissolved in 800. g of X the solution boils at 122.9 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. °C· kg x10 K, = || mol