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Understanding Aqueous Solutions in General Chemistry

Dive into the world of aqueous solutions with this introductory guide to homogeneous mixtures, solubility, electrolytes, and more. Learn about the interaction between solutes and solvents, the concept of dissociation, and the properties of strong and weak electrolytes.

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Understanding Aqueous Solutions in General Chemistry

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  1. Aqueous Solutions

  2. Solution • Homogeneous mixture • Solute – substance be dissolved • Solvent- substance solute is dissolved in

  3. Water As Solvent • Water is polar molecule • O atom has a greater attraction for electrons than H • O has partial negative charge (δ-) • H has partial positive charge (δ+)

  4. Hydration • Positive ends of water molecules are attracted to negative ions in ionic solid • Negative ends of water molecule attracted to positive ions • Each ion is then surrounded by water molecules • C:\Program Files\General Chemistry 4.0\General Chemistry 4.0.exe

  5. Dissociation • When ionic substances dissolve in water, they break up into their ions NH4NO3 (s)  NH4+(aq) + NO3-(aq)

  6. Solubility • How well substance dissolve • Some substances are more soluble than others • Very polar non-ionic substances may dissolve in water as well as ionic ones • “like dissolves like” • E:\TV11V44.MOV • E:\TV11V09.MOV

  7. Electrolytes • Solutions that conduct electricity • Conductivity comes from the presence of ions • More ions, better conductivity

  8. Strong Electrolytes • Very soluble salts, strong acids, and strong bases • Strong acids – ionize completely in water to form H+ ions • E:\TV13A01.MOV • Strong bases – ionize completely to form OH- ions

  9. Weak Electrolytes • Don’t ionize completely • Weak acids HF(s)  H+ + F- • E:\TV13A02.MOV • Weak bases NH3 + H2O  NH4+ + OH-

  10. Non-Electrolytes • Don’t ionize at all

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