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| 16297438617 | Which is typically in greater amount? Solute or solvent? | Solvent, as it is dissolving the solute in the solution | 0 | |
| 16297438618 | Will sucrose conduct electricity in water? Will sodium chloride? | Sucrose (a sugar) will not, as it cannot break up into mobile ions, since it is molecular and thus composed of individual MOLECULES. Sodium chloride, on the other hand, is an ionic compound and will have a molecule-ion attraction w/ the polar molecules of water. Thus, it will be split into the mobile ions: Na+ and Cl- | 1 | |
| 16297438619 | Definition of Dissociation | a general process in which molecules (or ionic compounds such as salts, or complexes) separate or split into smaller particles such as atoms, ions or radicals, usually in a reversible manner | 2 | |
| 16297438620 | Homogeneous mixture | Uniform composition of particles throughout the sample | 3 | |
| 16297438621 | Aqueous | A solution where water is the solvent | 4 | |
| 16297438622 | Why do ionic compounds conduct electricity in water? | Water is a neutral substance, but due to its molecular geometry (polarity), it has a partially positive end and a partially negative end. The partially positive end of the water molecule is attracted to the negative ions of the salt while the partially negative end is attracted to the positive ions of the salt. Ions in water are good conductors of electricity. | 5 | |
| 16297438623 | Polar Molecule: Electrolyte or Nonelectrolyte? | these covalently bonded molecules do have a slight difference in charge across opposite ends of the molecule, but are NOT considered to be electrolytes because they do not form ions when dissolved in water. | 6 | |
| 16297438624 | Acids: Electrolyte or Nonelectrolyte | Electrolyte: Will break up into ions when dissolved in water | 7 | |
| 16297438625 | Bases: Electrolyte or Nonelectrolyte | Electrolyte: Will break up into ions in water | 8 | |
| 16297438626 | Salts: Electrolyte or Nonelectrolyte | Soluble ionic compounds are strong electrolytes, as they break up into mobile ions in water. This is due to the molecule-ion attratcion with polar H2O molecules. | 9 | |
| 16297438627 | Nonpolar Molecule: Electrolyte or Nonelectrolyte | Molecules DO NOT have an overall net charge and thus CANNOT conduct an electric current. Nonpolar molecules do NOT dissolve in water (*like dissolves like*) and WILL NOT conduct. | 10 | |
| 16297438628 | How can one differentiate between two aqueous solutions relative to their electrical conductivity? | Utilize a conductivity apparatus to measure their electrical conductivites. The one that lights the bulb more will be the stronger electrolyte | 11 | |
| 16297438629 | Electrolytes | are solutes that are capable of conducting electricity |  | 12 |
| 16297438630 | Non-electrolytes | are solutes that are not capable of conducting electricity | 13 | |
| 16297438631 | Strong Electrolytes | completely break apart in solution and form ions. Since there are many ions present in solution, these substances are excellent conductors of electricity (ie. strong acids, strong bases, and soluble ionic compounds) | 14 | |
| 16297438632 | Weak Electrolytes | only partially break apart in solution forming ions. Since there are not as many ions present in solution, these substances are weak conductors of electricity (ie. weak acids and weak bases) |  | 15 |
| 16297438633 | Nonelectrolytes | do not break apart at all in solution. Since no ions are formed, these substances cannot conduct electricity at all (ie. molecular compounds and insoluble ionic compounds) |  | 16 |
| 16297438634 | Strong Acids | HI(aq) - HBr(aq) - HCl(aq) - HNO3 (aq) - H2SO4 (aq) - HClO3 (aq) - HClO4 (aq) |  | 17 |
| 16297438635 | Strong Bases | Any Group I metal hydroxide (KOH(aq), NaOH(aq), LiOH(aq), RbOH(aq), CsOH(aq)) The following Group II metal hydroxides • Ca(OH)2 (aq) • Sr(OH)2 (aq) • Ba(OH)2 (aq) |  | 18 |
| 16297438639 | Concentrated Solution | If a solution has a considerable amount of solute present, then it is said to be a concentrated solution |  | 19 |
| 16297438640 | Dilute Solution | If a solution has a very small amount of solute present, then it is said to be a dilute solution | 20 | |
| 16297438643 | Dilution | is a process where a concentrated solution is reduced to a lower concentration by adding more solvent to the sample. Adding more solvent reduces the concentration of solute present per liter of solution |  | 21 |
| 16297438646 | Neutralization | Process where an acid and base react to product water and a salt |  | 22 |
