7. Assuming complete dissociation, what mass of iron(III) chloride (molar mass = 162.20 g/mol) needs to be added 255 mL of water at 35 °C to cause an osmotic pressure of 2.60 mmHg?

At 70 °C, the solubility of an unknown solute is 65.7 g/100.0 g of water. What mass of the solute can dissolve in 125.5 g of water at the same temperature?

The solubility limit of a solute at 20. °C and 1.0 atm is 13.8 g of solute per 1 L of water. What will MOST likely happen when 12.0 g of solute are added to 1 L of pure water and the solution is mixed well (at the same conditions)?

At 25 °C, the solubility of NaCl is 36.0g/100g H20. How much NaCl can dissolve in 450 g of water at that temperature? * 8.0 g 162 g 0.080 g O 1.62 g

The freezing point of a liquid will change when a solute is added. Explain how the addition of salt impacts the boiling point of water. Calculate the freezing point change for a given concentration. Given that water's freezing point is 0.00°C and the freezing point depression constant (Kf) is 1.86 °C·kg/mol, calculate the freezing point depression for a 2.80 molal solution (moles/kg) of CaCl, in water. Assume ideal behavior of the ions. 21 MacBook Air 吕0 888 F1 F2 F3 F4 F5 F7 ! @ $ % & 1 3 6. 7 8. Q W E R Y

When 4.13 g of a certain molecular compound X are dissolved in 35. g of cyclohexane (C6H₁2), the freezing point of the solution is measured to be 3.7 °C. Calculate the molar mass of X.

Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?

-A solution is made by dissolving 16.0 g of CaCl2 in 4560 g of water.Calculate the freezing point of this solution.   -Calculate the osmotic pressure of a 0.75 M solution of ferric nitrate, Fe(NO3)3, at 25 oC

A 1.35 m aqueous solution of Compound X had a boiling point of 102.8°C. Which one of the following is most likely to be Compound X? Hint: The boiling point elevation constant for water is 0.52°C/m. Na3PO4 CaCl₂ X OKCI CH3CH₂OH

The freezing point of a solution that contains 1.1 g of an unknown compound, (A), dissolved in 12 g of benzene is found to be 2.97 °C. The freezing point of pure benzene is 5.48 °C. The freezing point depression constant of benzene is 5.12 °C/molal. What is the molecular weight of the unknown compound?