CHEMISTRY TOPIC SUMMARY Name: ________________________ Block: ________ Date: _______________ Topic N: Solutions Purple Packet Textbook Reference Pages 165-176 Chapter 15 Purpose The majority of chemical processes are reactions that occur in solution. Important industrial processes often utilize solution chemistry. "Life" is the sum of a series of complex processes occurring in solution. Air, tap water, beverages, and household ammonia are common examples of solutions. A solution is a homogenous mixture of substances with variable composition. The substance present in the major proportion is called the solvent, whereas the substance present in the minor proportion is called the solute. It is possible to have solutions composed of several solutes. The process of a solute dissolving in a solute is called dissolution. In this topic, we will learn about the basic properties of solutions, how to prepare standard solutions and how to use stoichiometry in solution chemistry. We will also learn what affects solubility including temperature, pressure, and the nature of the solute and solvent. Schedule A or B Due In-Class N/A Worksheet 1 (pp. 169-170) Worksheet 2 (pp. 171-172) Review Worksheet (pp. 175 – 176) Vocabulary Solution Solvent Solutes Aqueous Solution “Like Dissolves Like” Concentration Solubility HW Assignments Solutions Notes Notes Lab Worksheet 3 (173-174) Lab Review Test Saturated Unsaturated Concentrated Dilute Solution Supersaturated Mass Percent Molarity Standard Solution Dilution (M1V1 = M2V2) Worksheet 1 (pp. 169-170) Worksheet 2 (pp. 171-172) Review Worksheet (pp. 175 – 176) TBD Colligative Property Freezing Point Depression Boiling Point Elevation Effect of Temperature on Solubility Effect of Pressure on Solubility Solubility Curve CHEMISTRY TOPIC SUMMARY Name: ________________________ Block: ________ Date: _______________ By the end of these Topics, you should be able to demonstrate proficiency in the following areas: Essential Understandings The concepts developed in this standard include the following: Molarity = moles of solute/L of solution. [ ] refers to molar concentration. When solutions are diluted, the moles of solute present initially remain. The saturation of a solution is dependent on the amount of solute present in the solution. Solutions can be a variety of solute/solvent combinations: gas/gas, gas/liquid, liquid/liquid, solid/liquid, gas/solid, liquid/solid, or solid/solid. Polar substances dissolve ionic or polar substances; nonpolar substances dissolve nonpolar substances. The number of solute particles changes the freezing point and boiling point of a pure substance. A liquid’s boiling point and freezing point are affected by changes in atmospheric pressure. A liquid’s boiling point and freezing point are affected by the presence of certain solutes. Knowledge, and Skills In order to meet this standard, it is expected that students will: perform stoichiometric calculations involving the following relationships: - mole-mole mass-mass mole-mass mass-volume mole-volume; volume-volume perform calculations involving the molarity of a solution, including dilutions. interpret solubility curves. examine the polarity of various solutes and solvents in solution formation.