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Electrolytes

Learn about electrolytes and how they form ions in solution, allowing water to conduct electric current. Discover the differences between strong, weak, and non-electrolytes and their impact on conductivity. Explore examples of each type and their behavior in water.

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Electrolytes

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  1. Electrolytes Pre lab

  2. Electrolytes: a quick review • Electrolytes form ions in solution. • Ions allow water to conduct electric current • Three types of electrolytes: strong , weak, and non-electrolytes.

  3. Strong Electrolytes • Strong electrolytes ionize completely in water. • More ions in the water, more conductivity. • Strong electrolytes include: • Strong acids HCl H+ + Cl- • Strong bases NaOH Na+ + OH- • Soluble salts CaCl2 Ca2+ + 2Cl-

  4. Weak Electrolytes • Weak Electrolytes do not ionize completely in water. • Fewer ions, therefore less conductivity. • Weak electrolytes include: • Molecular acids • HC2H3O2 (aq) H+(aq)+C2H3O2 –(aq) • Slightly soluble salts • PbI2(s) Pb2+ (aq )+ 2I- (aq)

  5. Non Electrolytes • Non Electrolytes do not ionize in water: • They include alcohols, sugars and other covalent compounds • C12H22O11(s) C12H22O11(aq)

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