From the following list of aqueous solutions and water, select the one with the highest boiling point. O 1.5 m CH3OH, methyl alcohol O pure water O 0.75 m (NH4)3PO4 O 1.0 m LİCIO4 O 1.0 m CaSO4

A sample of an ionic solid is dissolved in 1.00 kg of water. The freezing point of the water is -0.01 °C. If three times the mass of ionic solid is dissolved in 1.00 kg of water and the resulting freezing point of the solution is -0.09 °C, which of the following would be possible formulas for the solid: MX, MX2, or MX3, where M represents a metal cation and X an anion with a 1- charge? Explain your reasoning.

Lead levels in drinking water should be no higher than 15 ppb. What is this in mol/L? Assume the density of drinking water is 1.0 g/mL. O 2.0 x 10-⁹ M O 3.1 x 10 ⁹ M O 3.1 x 107 M O 7.2 x 10 8 M O 7.2 x 10 5 M

The freezing point of CCI4 is -22.3°C and the freezing point depression constant is 29.8 °C/m. If a solution of C5H12 in CCI4 freezes at -37.6°C, what is the molality of this solution? O 0.513 0.722 O 2.01 O 5.01 O 1.26

will have the highest boiling point. Of the following, a 0.1 m aqueous solution of NaCl O Al(NO3)3 O K2CrO4 O N22SO4 sucrose

An aqueous solution of a compound used in antifreeze has an osmotic pressure of 0.589 atm at 20.0°C. It is prepared by dissolving 1.14 g of the compound in enough water to make 0.750 L of solution. What is the molar mass of the antifreeze compound? O 62.1 g/mol O 124 g/mol O 82.8 g/mol O 54.4 g/mol O 4.23 g/mol

Which of the following statements concerning factors that affect solute solubility is incorrect?  Gaseous solutes become less soluble in water with increasing temperature Most solid solutes become less soluble in water with decreasing pressure Most Solid solute become more soluable in water with increasing temperature Gaseous solutes become more soluable in water with increasing pressure

Choose the aqueous solution below with the lowest freezing point. All solutions are made of nonvolatile solutes. 0.200 m C6H12O6 0.200 m Al2(SO4)3 0.200 m K3PO4 0.200 m Ca(ClO4)2 These all have the same freezing point

Order the following four aqueous solutions by their freezing point temperature. The concentrations are in molality. Assume complete dissociation of electrolytes. highest freezing point (highest temperature) 0.035 m sucrose, C6H12O6 1 2 3 0.010 m potassium bromide, KBr 4 0.010 m sodium carbonate, Na2CO3 0.015 m calcium chloride, CaCl2 lowest freezing point (lowest temperature)

Which of the following aqueous solutions has the highest osmatic pressure? 1.0 М HСIO4 0.5 M NazSO4 O 1.0 M CaCl2 2.0 M sugar O 1.0 M NaCI