Calculate the mole fraction of solute and solvent in a 30% aqueous sugar solution (C12H22O11). Note: An aqueous solution is a solution where water is the solvent.

What is the molarity (M) of 0.012 mole fraction NaNO3(aq)? Density of solution = 1.05 g/cc, molar mass of NaNO3 = 84.9947 g/mil, molar mass of H2O = 18.015 g/mol.

A certain liquid X has a normal freezing point of 7.00°C and a freezing point depression constant =Kf 7.41·°C·kgmol−1. A solution is prepared by dissolving some iron(III) chloride (FeCl3) in 700.g of X. This solution freezes at 3.5°C. Calculate the mass of FeCl3 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits.

The molal boiling point elevation constant K = 1.15 °C·kg⋅mol the solution boils at 145.4 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10 1 for a certain substance X. When 14.4 g of urea Ś ((NH,),CO) (NH₂) CO) are dissolved in 150. g of X,

10. Determine the freezing point of a solution with 14.21 g of C₁₂H₂2O₁1 in 210.8 g of water, knowing that the freezing point of water is 0 °C, and K-1.86 °C/m.

Determine the mass percent composition of a solution made by dissolving 55.6 g of KF in 898 g of H2O.

. Throat spray is used in relieving pain and imritation caused by sore throat, sore mouth, or canker sores. It is composed of a diluted solution of Phenol in water. The mass percent of the usual throat spray is 1.40% C6H5OH in water. The density of the Phenol solution and Water are known to be 0.9956 g/ml and 1.00 g/ml respectively. Calculate the Molarity of the solution.

Determine the molality of a 25% sodium thiosulfate, Na2S2O3, solution.

A certain liquid X has a normal boiling point of 92.90°C and a boiling point elevation constant Kb=2.15·°C·kgmol−1. Calculate the boiling point of a solution made of 30.g of potassium bromide (KBr) dissolved in 800.g of X. Round your answer to 3 significant digits.

A certain liquid  X  has a normal boiling point of  105.30°C  and a boiling point elevation constant  =Kb1.13·°C·kgmol−1 . Calculate the boiling point of a solution made of  52. g  of zinc chloride ( ZnCl2 ) dissolved in  450.g  of  X .