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Solutions/Solubility
| Term | Definition |
|---|---|
| Solute | the compound dissolved in the solvent |
| Solvent | the most common compound in a solution, typically water in a liquid solution |
| Solution | combination of solute and solvent |
| Strong Electrolyte | Substance that completely ionizes in water and therefore is able to conduct an electric current |
| Weak Electrolyte | Substance the only partially ionizes in water and therefore is only able to conduct a weak electric current |
| Nonelectrolyte | Substance that does not ionize in water, allowing no current to conduct through the solution |
| Molarity | moles solute/liter solution |
| Molality | moles solute/kilogram solvent |
| Normality | moles of acidic protons/liter solution OR moles of basic hydroxides/liter solution. Helps emphasize strength of acids and bases that have more than one H+/OH- |
| Solubility Rule #1 | Most nitrate salts (NO3-) are soluble. |
| Solubility Rule #2 | Most salts containing alkali metal ions (Li+, Na+, K+, Cs+, Rb+) and the ammonium ion (NH4+) are soluble. |
| Solubility Rule #3 | Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag+, Pb2+, and Hg2^2+. |
| Solubility Rule #4 | Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, Hg2SO4, and CaSO4. |
| Solubility Rule #5 | Most hydroxides are only slightly soluble. The important soluble hydroxides are NaOH and KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble. |
| Solubility Rule #6 | Most sulfide (S^2-), carbonate (CO3^2-), chromate (CrO4^2-), and phosphate (PO4^3-) salts are only slightly soluble, except for those containing the cations in Rule 2. |
| Net Ionic Equation | Chemical equation of a reaction in which any spectator ions are removed (so in a precipitation reaction, the ions that do not precipitate are left out of equation) |
| ppm | parts per million, 10^-6 parts solute in a solution |
| ppb | parts per billion, 10^-9 parts solute in a solution |
| unsaturated | a solution in which more solute can be added and dissolved |
| saturated | a solution in which more solute added will not be dissolved and will remain solid |
| super saturated | a solution in which more solute is dissolved than would be possible under normal circumstances |
| dilute | a solution that has less solute dissolve, weak solution (i.e. weak coffee) |
| concentrated | a solution that has more solute dissolved, strong solution (i.e. strong coffee) |
| freezing point depression | the lowering of the freezing point of a solution due to amount of solute dissolved in the solution |
| boiling point elevation | the raising of the boiling point of a solution due to amount of solute dissolved in a solution |
| freezing point depression equation | deltaT = Kf*i*m. deltaT is the temp change from the freezing point of the pure solution, Kf is the molal freezing point depression constant, i is the number of ions produced by the solute when dissolved, and m is the molality of the solute |
| boiling point elevation equation | deltaT = Kb*i*m. deltaT is the temp change from the boiling point of the pure solution, Kf is the molal boiling point elevation constant, i is the number of ions produced by the solute when dissolved, and m is the molality of the solute |
| Osmosis | the passing of a solvent through a semi-permeable membrane toward the side containing a solution of higher concentration |
| osmotic pressure | the pressure that would have to be applied to a pure solvent to prevent it from passing into a given solution by osmosis, often used to express the concentration of the solution. |
| vapor pressure | The vapor pressure of a liquid is the equilibrium pressure of a vapor above its liquid (or solid); that is, the pressure of the vapor resulting from evaporation of a liquid (or solid) above a sample of the liquid (or solid) in a closed container. |
Created by:
shudonmiller
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