• What? Solutions that resist changes in pH even when tiny amounts of acids or bases are added.
• How? By containing both parts of a conjugate acid–base pair.
• Fun Fact: Imagine having a best friend who calms you down when you're too hyper, or pumps you up when you're too down. That's what buffer solutions do to pH!

Ever wondered how our bodies handle all the fizzy drinks, spicy foods, or even medicines without turning too acidic or basic? Thanks to the natural buffer systems in our blood, the pH remains around 7.35–7.45. These buffers include players like hydrogencarbonate ions and proteins.

Add a drop of 0.1moldm⁻³ HCl to

• 100cm³ of pure water: pH drops from 7.0 to 4.3 (Whoa! A big change! 📉)
• 100cm³ of a phosphate buffer: pH changes by less than 0.001 (This is like trying to find a needle in a haystack! 😲)

• When a villain (strong acid) is added, the buffer's friendly neighbor (weak base) neutralizes it.
• When a superhero (strong base) enters, the buffer's chaperone (weak acid) balances things out.
• In essence, powerful players are replaced with milder ones – sort of like swapping out a spicy chili for a bell pepper.🌶️➡️🫑