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Conductivity

Conductivity. Unit 4 Topic 6. Solutions. Solutions are made when a solute is dissolved in a solvent . When the solute dissolves it breaks up into its individual particles which then become surrounded by water molecules. Ionic solutions. Ionic compounds are made up of ions.

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Conductivity

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  1. Conductivity Unit 4 Topic 6

  2. Solutions • Solutions are made when a solute is dissolved in a solvent. • When the solute dissolves it breaks up into its individual particles which then become surrounded by water molecules.

  3. Ionic solutions • Ionic compounds are made up of ions. • They dissolve into individual ions in water. This process is called dissociation. • Each individual ion has a charge so when dissociated in water they can conduct.

  4. Ionic solutions • Ionic solutions are called electrolytes because ions can conduct electricity. • The amount of conductivity is directly related to the number of ions in a solution.

  5. Concentration • A 1.0 M solution will conduct more than a 0.01 M solution. • M = Molarity = moles/Liter Capital M

  6. Concentration • If you have a 1.0 M solution of both NaCl and AlCl3, the solution of AlCl3 will have a higher conductivity because it dissociates into more ions. • NaCl  Na+1 + Cl-1 (2 ions) • AlCl3  Al +3 + 3Cl-1 (4 ions)

  7. Covalent compounds • Covalent compounds are made up of individual molecules. • They dissolve into their individual molecules. • They do not dissociate.

  8. Individual molecules are neutral and do not carry a charge so when dissolved in water they do not conduct. • Covalent solutions are called non-electrolytes because they have no charge and cannot conduct.

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