Chapter 11 – Acid–Base Reactions

Brønsted–Lowry acid definition?

Proton (H⁺) donor.

Brønsted–Lowry base definition?

Proton (H⁺) acceptor.

General properties of acids?

Sour, pH <7, corrosive, conduct in solution, react with bases.

General properties of bases?

Bitter, pH >7, caustic (can burn or corrode), slippery, conduct in solution.

What’s an alkali?

Soluble base.

Examples of common acids?

HCl, H₂SO₄, HNO₃, CH₃COOH.

Examples of common bases?

NaOH, Ca(OH)₂, NH₃, Na₂CO₃.

What’s an amphiprotic species?

Can act as both acid and base.

Strong vs weak acids/bases?

Strong = fully ionise, weak = partially ionise.

Concentrated vs dilute acids/bases?

Based on amount of solute (acid/base molecules) in solution, not strength.

• concentrated if a lot of acid/base molecules

• dilute if there is little acid/base molecules

Neutralisation reaction definition?

Acid + base → salt + water.

Antacid purpose?

Neutralise stomach acid.

pH scale meaning?

Ranks acidity/basicity; low pH = acidic, high pH = basic.

pH calculation for strong acids/bases?

Common natural indicators?

Litmus, red cabbage.

Common commercial indicators?

Phenolphthalein, methyl orange, bromothymol blue, universal indicator.