Chem May Test Acid Base Titrations

acid + metal,

Salt + Hydrogen Gas

acid + carbonate,

salt water co2

acid + base

neutralisation salt water

Distinguish between the following terms, giving examples: ‘strong’ and ‘weak’ & ‘concentrated’ and ‘dilute’

o Recall the Arrhenius Model of acids and bases, identifying the limitations of the theory

ARRHENIUS ACID-BASE THEORY:

Acids: produce H⁺ ions in aqueous solutions.

eg,   HNO₃(l) → H⁺(aq) + NO₃^-(aq)

Bases: produce OH^- ions in aqueous solutions

eg,   Ca(OH)₂(s) → Ca²⁺(aq) + 2OH^-(aq)

LIMITATIONS:

restricted to aqueous solutions only

can’t explain the xn between HCl(g) and NH₃(g) to form NH₄Cl(s)

the hydrogen ion, H⁺, reacts with water to form the hydronium ion, H₃O⁺

State the Brønsted-Lowry definition of acids and bases

s: an acid donates a hydrogen ion, H+, and a base accepts a hydrogen ion

•B-L equations represent reversible equilibrium reactions, ⇌ are commonly used (weak acids & bases)

•H₂O molecules are included in equations for weak acids & bases

•H₂O can act as an acid or a base

Compare & contrast Arrhenius & Brønsted–Lowry models

Arrhenius is resticted by:

restricted to aqueous solutions only

can’t explain the xn between HCl(g) and NH₃(g) to form NH₄Cl(s)

the hydrogen ion, H⁺, reacts with water to form the hydronium ion, H₃O⁺

Identify strong acids

g HCl, H2SO4, HNO3

strong bases

g NaOH, KOH, Ca(OH)2.

Weak acids

g H3PO4, CH3COOH

Weak bases

NH3.

Define the acidity constant, Ka

as a numerical measure of the extent to which a proton transfer reaction goes to completion