R-ATCHE-10

Pranav: "what if we had a massive rubber band? it would be a great weapon"

Acid Bases

Strong electrolytes - completely ionise/dissociate

• Solutions of a strong electrolyte will conduct electricity well.
• Examples: NaCl, HCl
• Remember: molecules ionise, salts dissociate!

Weak electrolytes - partially ionise/dissociate(?)

• Examples: $CH_{3}COOH$,$H_{2}CO_{3}$

Dissolved things:

• $C_{6}H_{12}O_{6}$ - non electrolyte, hence dissolving this into solution will not make the solution electrically conductive.

Weak electrolytes

Weak electrolytes ionise/dissociate partially because the ionised/dissociate products have a tendency to reform the original electrolyte.

e.g. $CH_{3}COOH + H_{2}O\rightleftharpoons CH_{3}COO^{-}+H_{3}O^{+}$

This is where equilibrium knowledge comes handy. :)

Arrhenius Model vs Bronsted Lowry

Arrhenius:

• $H^{+}$ in solution = acid
• $OH^{-}$ in solution = base

Pros:

• Ez Cons:
• Doesn't explain acidic/basic properties of other things, only H+ and OH-
  • e.g. $NH_{3}$ is basic, yet Arrhenius model doesn't explain why

Brønsted–Lowry:

• Proton donor = Acid
  • $NH_{3}+H_{2}O\rightleftharpoons NH_{4}^{+}+OH^{-}$ (weak so double arrows)
• Proton receiver = Base
  • $HCl+H_{2}O\to H_{3}O^{+}+Cl^{-}$ (strong so single arrow)

Water

Water is amphoteric, and thus can undergo self-ionisation:

$H_{2}O + H_{2}O \rightleftharpoons H_{3}O^{+} + OH^{-}$

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