The solubility of sodium acetate at 20° C is 46.5 g per 100 grams of water. When 50.0 g of sodium acetate is mixed with 100 grams of water at 20° C, a solution containing dissolved sodium acetate and some undissolved sodium acetate results. This solution is best described as: Saturated     Supersaturated     Unsaturated

Colligative properties are those that depend on the number of solute particles. Because electrolytes dissociate into ions, the concentration of particles in the solution is greater than the formula-unit concentration of the solution. For example, if 1 mol of NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at - 14.5 °C? The freezing point for pure water is 0.0 °C and Kf is equal to 1.86 °C/m. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) However, complete dissociation of electrolytes does not always occur. The extent the van't Hoff factor, i: dissociation is expressed by HA moles of…

The solubility of a compound is 84 g per 100.0 g solvent at 25 °C. If 84 g of the compound is dissolved in 200.0 g of solvent at 25 °C, the solution is dilute unsaturated saturated supersaturated

A salt has a molar solubility of 4.18 M at 21.0°C. What is the the maximum amount of salt (in moles) that can dissolve in 1.495 L of solution before the solution becomes supersaturated at 21.0°C? Assume the salt has a molar mass of 55.44 g/mol. Report your answer to 2 decimal places.

If a 24 g sample of a nonelectrolyte is dissolved in 156 g of water, the resulting solution will freeze at –1.13°C. What is the molar mass of the nonelectrolyte?

10.0 g ZnCl2 is dissolved in 100.0 g of water at 23.6 °C. The solution reaches a temperature of 36.5 °C. What is the molar heat of dissolution for ZnCl2? Assume the specific heat capacity of the solution is the same as pure water, 4.184  J/g·°C.

A solution is made using 95.0 g of potassium nitrate in 300. mL of water at 70.0 ℃.  If the solution is quickly cooled to to 20.0 ℃, how many grams of potassium nitrate precipitate out?

< 11 of 19 I Review Constants | Periodic Table Part B A student placed 16.0 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve the glucose by swirling, then carefully added additional water until the 100. mL mark on the neck of the flask was reached. The flask was then shaken until the solution was uniform. A 45.0 mL sample of this glucose solution was diluted to 0.500 L. How many grams of glucose are in 100. mL of the final solution? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? Value Units

An aqueous zinc bromide solution (ZnBr2) boils at 100.250 °C.  What is the molality of this solution?  The Kb of water = 0.512 °C/m.    ΔT = Kf * m * i       0.488 m     0.512 m     0.252 m     0.163 m

The freezing point of acetic acid is 17.0 °C, and its Kf is 3.90 °C·kg/mol.  If dissolving an amount of solute into 4.862 g of acetic acid results in a solution having a freezing point of 15.9 °C, how many moles of solute are in the solution?