6. What is the mole fraction of 1.98 m Fe(NO3)3(aq)? The molar mass of Fe(NO3)3 is 241.9 g/mol and the molar mass of water is 18.02 g/mol. 0.0345 0.0641 0.324 0.479 0.863 7. Which of the following statements are CORRECT? 1. Solubility is the concentration of solute in equilibrium with undissolved solute in a saturated solution. 2. If two liquids mix to an appreciable extent to form a solution, they are immiscible. 3. If two liquids mix completely in any proportion to form a solution, the resulting solution is supersaturated. 1 only 2 only 3 only 1 and 2 2 and 3 8. Which of the following compounds is expected to have the strongest ionic bonds? RbI RbF LiF CsBr 9. What is the mole fraction of MgCl2 in a solution that is 11.04% by mass MgCl2(aq)? The molar mass of MgCl2 is 95.21 g/mol. 0.02295 0.02349 0.1104 0.1160 1.303 10. What mass of Cu(NO3)2 must be added to 1.00 kg H2O to prepare 97 ppm Cu2+(aq)? 3.3 ´ 10-4 g 5.2 ´ 10-4 g 9.7 ´ 10-3 g 0.033 g 0.29 g 1
1. Which of the following properties of water can be attributed to hydrogen bonding? 1. high heat of vaporization 2. high surface tension 3. higher density of liquid versus solid 1 only 2 only 3 only 1, 2, and 3 12. Ideally, colligative properties depend only on the concentration of solute particles in a solution. identity of the solute particles in a solution. color of a solution. hydrated radii of the molecules or ions dissolved in a solution. partial pressure of the gases above the surface of a solution. 13. The specific heat capacity of silver is 0.235 J/g K. Its melting point is 962 C and its enthalpy of fusion is 11.3 kJ/mol. What quantity of heat in joules is required to change 5.00 g of silver from a solid at 25 C to a liquid at 962 C? 2,300 joules 345 joules 1,620 joules 902 joules 14. What mass of NaCl must be dissolved in 65.0 grams of water to lower the freezing point by 7.50 °C? The freezing point depression constant, Kfp, for water is -1.86 °C/m.