What mass of water is needed to dissolve 34.8 g of copper(II) sulfate in order to prepare a 0.521 m solution?

• 0.418

• 0.419

• 0.420

• 0.421

The vapor pressure of water at 20° C is 17.5 torr. What is the vapor pressure of water over a solution containing 300. g C6H12O6 and 455 g of water?

• 16.4 mm Hg

• 16.5 mm Hg

• 16.6 mm Hg

• 16.7 mm Hg

Calculate the freezing point of a solution made from 32.7 g of propane, C3H8, dissolved in 137.0 g of benzene, C6H6. The freezing point of benzene is 5.50° C and its Kf is 5.12° C/m.

• -22.2° C

• -22.3° C

• -22.4° C

• -22.5° C

Calculate the boiling point of a solution made from 227 g of MgCl2 dissolved in 700. g of water. What is the boiling point of the solution? Kb = 0.512° C/m.

• 105.24° C

• 105.34° C

• 105.44° C

• 105.54° C

Calculate the concentration of nitrogen gas in a 1.00 L container exerting a partial pressure of 572 mm Hg at room temperature. Henry’s law constant for nitrogen at 25° C is 6.8 x 10-4 mol/L·atm

• 5.1 x 10^-4 M

• 5.1 x 10^-5 M

• 5.1 x 10^-6 M

• 5.1 x 10^-7 M

A solution contains 21.6 g of a nonelectrolyte and 175 g of water. The water freezes at -7.18° C and Kf = 1.86° C/m. Is the nonelectrolyte CH3OH or C2H5OH?

• CH₃OH

• C₂H₅OH

Find the molarity of all ions in a solution that contains 0.165 moles of aluminum chloride in 820. ml solution.

Find the molarity of each ion present after mixing 27 ml of 0.25 M HNO3 with 36 ml of 0.42 M Ca(NO3)2

Find the molarity of each ion present after mixing 35 ml of 0.42 M K₂SO₄ with 27 ml of 0.17M K₃PO₄.

a solution consists of 3.88 g benzene,C6H6 , and 2.45 g toluene ,C6H5CH3. The vapor pressure of pure benzene at 20. °C is 75 mm Hg and that of toluene at 20.0 °C is 22 mmHg. Assume that Raoult’s law holds for each component of the solution.

Calculate the mole fraction of benzene in the vapor.. ( molar mass of benzene= 78.0 g/mole and toluene = 92.0 g/mole.)