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Electrical Conductivity

Electrolytes and pH. Electrical Conductivity. Electrolyte: a substance that when dissolved in water allows an electric current to flow through the solution. Example: table salt Some substances can be dissolved in water but do not conduct electricity called nonelectrolytes . Example: Sugar

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Electrical Conductivity

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  1. Electrolytes and pH Electrical Conductivity

  2. Electrolyte: a substance that when dissolved in water allows an electric current to flow through the solution. Example: table salt • Some substances can be dissolved in water but do not conduct electricity called nonelectrolytes. Example: Sugar • Electrical conductivity of a solution is a measure of its ability to allow an electric current to flow through it. Electrolyte

  3. Solutions that contain electrolytes are electrolytic solutions. • Batteries are an example of an electric cell. • Containing an electrolytic solution that conducts electricity • Batteries conduct electricity between two poles Electrolytic solutions

  4. A physical change; the separation of a dissolved compound into two ions of opposite charges • Example: Sodium chloride (NaCl) dissociates into Na+ and Cl- • If sodium chloride dissolves in water, all of its properties are conserved • When a nonelectrolyte solution is dissolved, no ions are produced dissociation

  5. NaCl(s)→Na+ (aq) + Cl- (s)=solid (aq)= aqueous solution H2O indication that the solute was placed in water Sodium Chloride Example H2O

  6. Ions conduct electricity • Electrodes connected to a power supply in an electrolyte solution • Positive ions migrate toward the negative electrode • Negative ions migrate toward the positive electrode Cont...

  7. Acids: A compound that produces H+ ion when dissolved in water. We can easily reconize acids because their molecular formulas start with “H” Base: A compound that produces OH- ions when dissolved in water. We can easily recognize bases because their molecular formula ends with “OH” A salt is an ionic compound that forms ions (other than H+ and OH-) when dissolved in water. We will work with neutral salts TypesAcids – Bases - Salts

  8. Common acids: fruit juice, soft drinks, gastric juices • Exception to the rule acetic acid...vinegar! CH3COOH • Why? • Doesn`t start with Hydrogen Acids

  9. Common examples: heart burn medications, cleaning products, blood Usually begins with a metal and ends with OH Exception Ammonia: NH3 bases

  10. Salts made up of metal and one or more nonmetal • Not all salts dissolve easily in water • Electrolytic dissociation are important to us! • Vital to survival Salts

  11. IdentifyAcid – Bases - Salts

  12. Properties

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