- The solubility of some salts is affected by the pH of the environment
Basic Solutions
- High pH (more basic) → more OH- ions
○ Ex: 
■ Increasing pH (adding OH-) → Q > Ksp → decreases solubility of the salt → solubility is less in a basic environment that in pure water
Acidic Solutions
- Low pH (more acidic) environment → lots of hydronium ions (H3O+)
○ Ex: 
■ Decreasing pH (adding H+) → Q < Ksp → increased solubility
- Remember: if you have an equilibrium situation where adding more of something that isn’t in eq. equation, then likely that added thing will react with smthn in eq. equation
- Ex:
- Reaction as a result of adding hydronium
→ shift in forward direction