How many liters of a 5.00 M solution of Na3PO4 are needed to have 4.00 osmoles ? First we need the equation for dissolving the salt, Na3PO4 + 3 Na+1 + PO,3 An osmole is a mole of dissolved particles the conversion factor is 1 mol = osmol First convert osmoles into moles 1 mol osmol)(- mol osmol Then calculate the liters 1 L mol)(- mol

Isopropyl alcohol is mixed with water to produce a 33.0% (v/v) alcohol solution. How many milliliters of each component are present in 805 mL of this solution? Assume that volumes are additive.

I need to clear my head with # 6 but I’m stuck can h please help me to understand

4. What is the osmotic pressure of a solution if 1.50 grams of BaCk has been mixed in a 200mL of 0.50M solution of BaCl2? The temperature of the solution is 45°C. 5. What is the vapor pressure lowering of the resulting solution in problem 4 if the vapor pressure of the solvent is 5.00 atm? Assume that the volume of the solvent is the volume of the solution. 6. A student was requested to prepare a 500mL of 0.5N solution of MgSO.. The lab teacher required the student to change the concentration of the solution by adding 2.50 grams of MgSO. The boiling point of water was determined to be 98.5°C while the freezing point was noted at 0.50 °C. What is the final concentration of the solution expressed as molality (m) after adding extra MgS0.7 What is the boiling point and freezing point of the solution? (Use the Ko and Ki values from any reference.) Assume that the volume of the solvent is also the volume of the solution.

0.9% (w/v) sodium chloride (MW = 58.44 g/mol) solution (normal saline solution) has an osmotic pressure of 3.91 atm at 25º C.  What is the molality of the aqueous solution if the density of sodium chloride is 2.16 g/ml? 0.160 m                      6.25 m                   1.55 m                  1.91 m

Please provide only typed answer solution no handwritten solution needed allowed

10 g of glucose (π1), 10 g of urea (π2) and 10 g of sucrose (π3) are dissolved in 250 mL of water at 300 K (π = osmotic pressure of solution). The relationship between the osmotic pressures of the solutions is: π3 > π1 > π2 π1 > π2 > π3 π2 > π1 > π3 π2 > π3 > π1

Which solution would have the highest osmotic pressure, all measured at the same temperature? A) 0.10M KBr B) 0.10M C6H12O6 C) pure water D) 0.10M Na2SO4 E) all have the same osmotic pressure

When 3.25 g of a nonelectrolyte solute is dissolved in water to make 165 mL of solution at 24 °C, the solution exerts an osmotic pressure of 879 torr.What is the molar concentration of the solution? MHow many moles of solute are in the solution? molWhat is the molar mass of the solute? g/mol

0.9 gms NaCI + pure water = 100 mls total   Determine the approximate osmol