Honors Chemistry

Chapter 13-14 Study Guide

Can you:

• Describe how a molecular solid, such as sugar, is able to dissolve in a liquid such as water.
• Define solution, solute, solvent, solvation, hydration, heat of solution, electrolyte, solubility, saturated, unsaturated, supersaturated, crystallization, effervescence, concentration, percent by weight, molarity, molality.
• Describe the dissolving process in terms of bonds being made and broken, and heat energy being released or absorbed, then explain how the overall dissolving process could be exothermic or endothermic.
• Describe how dissolving an ionic solid is different than dissolving a molecular solid, including how ionic compounds exist in solution.
• List the factors that affect the solubility of a solid in a liquid, and a gas in a liquid, and explain why those factors affect the solubility.
• Explain how you might prepare a supersaturated solution by dissolving a solid in a liquid, why it’s an unstable state, and what will eventually occur to the solution.
• Explain how a solution of a gas dissolved in a liquid could become supersaturated, and how effervescence occurs in a solution like this.
• Explain how solubility is related to a saturated solution.
• Explain the processes that are taking place in a saturated solution, and how these are related to the concept of dynamic equilibrium. Include both solid in a liquid and gas in a liquid.
• Explain why agitating (stirring) a liquid as you attempt to dissolve a solid makes the solid dissolve faster.
• Explain why smaller crystals of solid dissolve faster than larger crystals.
• Explain why a solid dissolves faster in warm liquids than in cool liquids.
• Calculate percent by weight given the mass of solute and solvent.
• Do calculations using the molarity formula.
• Do mole problems involving solution concentration (molarity).
• List the colligative properties.
• Explain why dissolving a solute in a liquid lowers the liquid’s melting point.
• Explain why dissolving a non-volatile solute in a liquid raises its boiling point.
• Explain osmotic pressure.
• Explain why a mixture of ice and water gets colder when salt (or any other solute) is added.
• Explain how concentration is related to colligative properties.
• Calculate the molality of a solution.
• Use solubility rules to predict the solubility of ionic compounds, and the formation of precipitates from mixtures of solutions containing ionic compounds.
• Write balanced molecular, total ionic and net ionic equations for precipitation reactions involving ionic compounds. Be able to explain how the formula for the precipitate is determined.