University:
University of North Dakota
Course:
CHEM 121 | General Chemistry I
Academic year:

2023
Views:

341

Pages:

3
Author:

Nigel Sherman

Chemistry 1213 Notes Solution Basics: What is a solution? Mixture of two or more substances uniformly dispersed throughout a single phase What does it mean when something is soluble? Substance is capable of being dissolved What is the difference between homogenous and heterogeneous? Homogenous solutions look the same throughout like the salt water. Heterogeneous mixtures are non-uniform throughout. Components of a Solution: What is a solvent? The solvent is the dissolving medium in a solution What is a solute? The solute is the substance dissolved in a solution. Types of Solutions: What is a suspension? Particles in a solvent are so large that they settle out unless constantly stirred. What is a colloid? Particles are intermediate in size What is an electrolyte? Substance that dissolves in water to give a solution that conducts electrical current What is an alloy? Mixture of metals The Process of Dissolving: What factors affect how quickly you can dissolve a solute in a solvent? • • • Increasing the Surface Area of a Solute Stirring a solution Heating a solvent Saturation of Solutions: What is a saturated solution? Solution that contains maximum amount of dissolved solute What is an unsaturated solution? Solution that contains less solute than a saturated solution What is a supersaturated solution? Solution that contains more dissolved solute than a saturated solution under the same conditions. Will it dissolve? The general rule for determining whether something is soluble is Like dissolves like This means that polar solvent will dissolve polar solutes; nonpolar solvents will dissolve nonpolar solutes. How do we determine whether something is polar or nonpolar? Look at the electronegativity differences and the molecular shape. Example Problem #1: Will it dissolve? Write whether the following solid compounds will be soluble or insoluble in water? (a) Anthracene, 𝐶14 𝐻10 Nonpolar (b) Cupric Sulfate, 𝐶𝑢𝑆𝑂4 Polar (ionic) (c) Lactic acid, 𝐻𝐶3 𝐻5 𝑂3 Polar Liquids in Solution: Will it mix? What does miscible mean? Liquids that dissolve freely in one another in any proportion What does immiscible mean? Liquids that are not soluble in each other Gases in Solution: Mass Using the table to the right, describe what happens to the solubility of a gas as mass increases? As mass increases, the solubility of a gas increases Why does this trend occur? The amount of london dispersion forces increase which leads to an increased amount of attraction between solute and solvent. Gases in Solution: Adding Pressure Would the solubility of a liquid or solid change with pressure? Does not change significantly How would a gas be different than a liquid or solid? A gas can be affected more by pressure because of its properties What is the relationship we see regarding solubility of a gas in a liquid vs. pressure? As pressure increases, the solubility of that gas in a liquid increases What does Henry’s Law state? Henry’s Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.