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Section 6.1—Solutions & Electrolytes

Section 6.1—Solutions & Electrolytes. What are those “electrolytes” they say you’re replacing by drinking sports drinks?. Dissolving substances. Substances are dissolved by a process called HYDRATION or SOLVATION The solvent attracts to the solute New intermolecular forces are formed

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Section 6.1—Solutions & Electrolytes

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  1. Section 6.1—Solutions & Electrolytes What are those “electrolytes” they say you’re replacing by drinking sports drinks?

  2. Dissolving substances • Substances are dissolved by a process called HYDRATION or SOLVATION • The solvent attracts to the solute • New intermolecular forces are formed • The solvent “carries off” the solute particles and surrounds the ions – keeping them dissolved!

  3. - - O H H + Dissolving Ionic Compounds - + Ionic compound water Water molecules are polar and they attract to the charges of the ions in an ionic compound. + - If the ion attraction is weak enough, the water can successfully pull them apart. + - + - + -

  4. - - + O + H H + Dissolving Ionic Compounds - + Ionic compound water As more ions are “exposed” to the solvent, they can be carried off as well. - - + - + -

  5. - O H H + Dissolving Ionic Compounds - + Ionic compound water + - These free-floating ions in the solution allow electricity to be conducted - + - + - + -

  6. Electrolytes • Electrolytes – substances that produce free floating ions and can conduct a current when dissolved. • Ex. NaCl(s) Na+1(aq) + Cl-1(aq)

  7. + - + Solute, sugar (polar) Solvent, water (polar) - - + - + - + - + - + Dissolving Covalent Compounds Water forms intermolecular forces with the polar ends of the solute and “carries” the solute particles away.

  8. + - + Solute, sugar (polar) Solvent, water (polar) - - + - + - + - + - + Dissolving Covalent Compounds NOTICE how the polar covalent molecules themselves do not split into charged ions—the solute molecule stays together and just separates from other solute molecules.

  9. Non-electrolytes • NON-ELECTROLYTES - When molecules separate from other molecules and DO NOT create free-floating ions C6H12O6(s)  C6H12O6(aq)

  10. Types of Electrolytes Non-Electrolytes Strong Electrolytes Weak Electrolytes Covalent Compounds Ionic compounds Strong Acids Strong Bases Ionic Compounds Weak Acids Weak Bases No molecules separate—ions are not formed Fully Ionize in solution Only a few ions are created in water DOESN’T CONDUCT STRONGLY CONDUCTS CONDUCTS WEAKLY

  11. Breaking up Electrolytes • Leave polyatomic ions in-tact (including the subscript within the polyatomic ion) • All subscripts not on a polyatomic ion become coefficients • Be sure to include charges on the dissociated ions! Example: Break up the following ionic compounds into their ions KNO3 Ca(NO3)2 Na2CO3

  12. Breaking up Electrolytes • Leave polyatomic ions in-tact (including the subscript within the polyatomic ion) • All subscripts not within a polyatomic ion become coefficients • Be sure to include charges on the dissociated ions! Example: Break up the following ionic compounds into their ions  K+1 + NO3-1  Ca+2 + 2 NO3-1  2 Na+1 + CO3-2 KNO3 Ca(NO3)2 Na2CO3

  13. Misconceptions about dissolving • Dissolved Solids DO NOT dissappear • In the solid it is a LARGE enough particle collection to see! • After dissolving, the particles are ALONE and too small to see

  14. Another Way to Think about Solutions: Super-Saturated Unsaturated Saturated Holds more solute than what should be dissolved at that temperature More solute can be dissolved at that temperature No more solute can be dissolved—it’s “full” at that temperature In general, more solid will dissolve at higher temperatures!

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