Acids, bases and pH with worked titration steps
pH is a logarithm, and that single fact explains most of the confusion. Noeta separates concentration from strength once and for all.
What this covers
- Brønsted–Lowry acids and bases
- pH, pOH and the ion product of water
- Strong vs weak acids
- Neutralisation and salts
- Titration calculations and curves
Worked example
Problem
Find the pH of 0.01 mol/dm³ HCl.
- 1StrengthHCl is strong, so it dissociates fully: [H⁺] = 0.01 mol/dm³.
- 2Apply the definitionpH = −log₁₀(0.01).
Answer: pH = 2
Mistakes that cost marks
- Treating a weak acid as fully dissociated.
- Confusing concentration with acid strength.
- Forgetting pH + pOH = 14 at 25 °C.
Questions students ask
What is the difference between strong and concentrated?
Strength is how fully it dissociates; concentration is how much is dissolved. They are independent.
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