Two beakers are placed in a small closed container at 25 °C. One contains 416 mL of a 0.112 M aqueous solution of C6H12O6; the second contains 242 mL of a 0.266 M aqueous solution of C6H12O6. Small amounts of water evaporate from both solutions. As time passes, the volume of solution in the second beaker gradually (Increases or decreases) and that in the first gradually (increases or decreases). If we wait long enough, what will the final volumes and concentrations be?

Sodium chloride is often used to prevent icy roads and to freeze ice cream. What are the boiling point and freezing points of 0.034 m aqueous solution of sodium chloride? Kb = 0.512 °C/m ; Kr= %3D 1.86 °C/m.

You are analyzing 100 g of a solution that contains 12.5 g of the ionic compound KBr (MM = 119.0 g/mol) in water.  Here is some useful information:  KFP of water is 1.86 °C/m; KBP for water is 0.512 °C/m.  The density of the solution is 1.094 g/mL. Calculate the boiling point of this solution (bp of water is 100.0°C).   Calculate the osmotic pressure (in atm) of this solution at 25°C.

[References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. K₁ (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.95 grams of the compound were dissolved in 293.3 grams of ethanol, the solution began to boll at 78.570 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Congage Learning Cengage Technical Support Previous Next Save and Exit