Alright future chemists! Today we're jamming with weak acids, weak bases, and all their dissociation vibes! 🎸🔥

Weak acids and bases don't dissociate completely, leaving us with some remaining undissociated molecules. Remember, dissociation is like a rock band breaking up; not everyone goes solo! 🎶

• Ka (Acid Dissociation Constant) HA ⇌ H⁺+ A⁻ Ka = \(\frac {[H^+][A^-]}{HA]}\)

• Kb (Base Dissociation Constant) B +H₂​O ⇌ BH⁺ + OH⁻ Kb = \(\frac{[BH^+][OH^-]}{[B]}\)

Example City 🏙

• Lemon juice is acidic (but weak)! 🍋 Imagine squeezing a lemon into water; not all the lemon molecules (citric acid) 'go solo.'

pKa and pKb: Bigger pKa or pKb values mean weaker acids or bases, respectively. pKa=−logKa
pKb=−logKb

Example Boulevard 🏞

• Vinegar (ethanoic acid) has a pKa of 4.76, weaker than lemon juice (citric acid). It's like having a softer song in a rock playlist! 🎵

To find the Ka or Kb for weak acids/bases, we experiment by measuring the pH of their standard solutions. We can then calculate the pH of that solution using these constants.

Example Road 🛣

• Say we have a soda (carbonated water) with a known pH, we can find the pKa and then determine how strong or weak that acid is! 🥤