Chemistry, Ch. 13: Solutions Vocabulary Soluble Solvent Solute Suspension Electrolyte Saturated solution Unsaturated solution Supersaturated solution Solubility Miscible Immiscible

Vocabulary *Soluble: Capable of being dissolved *Solvent: The dissolving medium in a solution (thing that does the dissolving) *Solute: The substance dissolved in a solution *Suspension: Particles in a solvent are so large that they settle out unless mixture is constantly stirred

Vocabulary Electrolyte: Substance that dissolves in water to give a solution that conducts electric current *Unsaturated solution: Solution that contains less solute than a saturated solution under the existing conditions *Saturated solution: Solution contains the maximum amount of dissolved solute

Vocabulary *Supersaturated solution: Solution that contains more dissolved solute than a saturated solution contains under the same conditions *Solubility: The amount of substance required to form a saturated solution with a specific amount of solvent at a specified temperature

Vocabulary Miscible: Liquids that dissolve freely in one another in any proportion Immiscible: Liquid solutes and solvents that are not soluble in each other

Kool-Aid Contents: Which is it? The sugar in Kool-Aid: solute The water in Kool-Aid: solvent Video: supersaturated solution immiscible

Which is it? electrolyte suspension

Solubility Graphs (Fig. 13-15) Not all solutes have the same solubility

What mass of KClO3 will dissolve in 100 g of water at 10°C? If a solution has 15 g of KNO3 dissolved in 100 g of water at 10°C, is it unsaturated, saturated, or supersaturated? Unsaturated

What is the maximum mass of KNO3 that will dissolve in 500 g of H2O at 40°C? 64g KNO3 = x 100g H2O 500g H2O 320g KNO3

Molarity Measure of concentration of a solution Molarity = moles of solute L of solution Abbreviated: M (“molar”) 3M HCl = “3 molar” HCl = 3 moles HCl 1 L solution

Example 1 2 moles NaCl = 0.57 M NaCl 3.5 L You have 3.5 L of solution that contains 2 moles of sodium chloride. What is the molarity of the solution? 2 moles NaCl = 0.57 M NaCl 3.5 L

Example 2 You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain? 0.5 M = x 0.8 L x = 0.4 mol HCl

Example 3 You have 4.5 L of solution that contains 175 g of copper (II) sulfate. What is the molarity of the solution? 175 g CuSO4 1 mol CuSO4 = 1.10 mol CuSO4 159.62 g CuSO4 1.10 mol CuSO4 = 0.24 M CuSO4 4.5 L