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Understanding Solutions: Solvents, Solutes, and the Dissolving Process

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sheng
9 diapositives · 232 Views · Jul 13, 2014

This chapter delves into the formation of solutions, defining them as homogeneous mixtures of solutes and solvents, and discussing the roles of ionic and molecular compounds in dissolving processes. It explains how polarity affects solubility, illustrating the principle of "like dissolves like," and provides insights into the functionality of different solvents like water, ethanol, and non-polar solvents used in dry cleaning. Additionally, it explores terms of concentration such as unsaturated, saturated, and supersaturated solutions, and the effects of temperature on solubility.

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  1. Chapter 15 Forming Solutions • Recall a solution is a homogeneous mixture of a solute and a solvent. • The substance present in the largest amount is the solvent. • The solute solvent combination can be any state: solid, liquid, or gas. • If water is the solvent, it is referred to as an aqueous solution.

  2. The Dissolving Process • When an ionic substance dissolves water separates the cation from the anion and both become the solute in the solution. • Soluble ionic compounds are more attracted to the polar water molecule than to the ionic complement in the crystal. • Insoluble ionic compounds are more attracted to each other than to the water molecule.

  3. The Dissolving Process • Molecular solutes dissolve in water if they have similar bonding characteristics as polar water. • Ethanol, C2H5OH, dissolves in water because the O-H bond is similar in polarity to the O-H bond in water. • “Likes dissolve like” • Oil is a non-polar substance made with non polar bonds between C and H so it is NOT soluble in water.

  4. “Dry” Cleaning • Dry Cleaning uses a non-polar solvent to dissolve the dirt and substances from your clothes. Many fabrics require this type of solvent. • Tetrachloroethylene Cl2C=CCl2 is used for the dry cleaning of fabrics. It is non-polar because the molecule is symmetric and the electrons are shared more equally than in water.

  5. Concentration Terms • Unsaturated • More solute can be put into the solution. • Saturated • The maximum amount of solute is placed in the solution. • Supersaturated • More than the maximum amount of solute is placed in the solution.

  6. Saturation • A solution is said to be saturated when you have the maximum amount of solute in the solvent. • At the point of saturation the solvent no longer has the availability to break apart the solute. • If more solute is placed in the solution a state of dynamic equilibrium is reached. • The additional solute will dissolve, however the dissolved solute will fall out of the solution at the same rate.

  7. Supersaturation • Changing the temperature of the solution will affect the amount of solute allowed in the solvent. • Increasing the temperature will increase the solubility of endothermic dissolving processes. • Most solids are endothermic like this. • Decreasing the temperature will increase the solubility of exothermic dissolving processes. • Most gases are exothermic like this. • A solution becomes supersaturated by saturating it then lowering/raising the temperature.

  8. Vitamins • Water soluble (polar) vitamins like Vitamin C are water soluble and can be taken daily without concern. Your body excretes any excess though the kidneys. • Fat soluble (nonpolar) vitamins like Vitamin A are fat soluble and are stored in the tissue. It is possible to overdose on fat soluble vitamins because your body has a harder time removing the excess. • Follow recommended amounts!

  9. Homework • Terms Chapter 14 • Pg. 555 [4-11]