Solutions Chemistry
Solutions chemistry covers solubility, concentration units, colligative properties, and solution preparation. Master molarity, molality, dilutions, and how solutes affect solution properties.
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Study Tips
- ✓Molarity = moles solute / liters solution; Molality = moles solute / kg solvent
- ✓For colligative properties, use van't Hoff factor (i) for electrolytes
- ✓Memorize common solubility rules: all nitrates are soluble, most chlorides are soluble except AgCl, PbCl2
- ✓Osmotic pressure formula: pi = iMRT
Common Mistakes to Avoid
Common errors include confusing molarity and molality (volume vs mass of solvent), forgetting the van't Hoff factor for ionic compounds, using total solution volume instead of solvent mass for molality, and miscalculating dilutions. Remember: molarity changes with temperature; molality doesn't.
Solutions Chemistry FAQs
Common questions about solutions chemistry
The van't Hoff factor (i) accounts for the number of particles a solute produces in solution. For non-electrolytes, i = 1. For strong electrolytes, i equals the number of ions (NaCl produces Na+ and Cl-, so i = 2). For weak electrolytes, 1 < i < theoretical maximum.
Colligative properties depend only on the NUMBER of solute particles, not their identity. Adding any solute raises boiling point (delta Tb = iKbm), lowers freezing point (delta Tf = iKfm), lowers vapor pressure (Raoult's law), and creates osmotic pressure.
M1V1 = M2V2 where M1 and V1 are initial molarity and volume, M2 and V2 are final values. Use this when adding water to a solution. Make sure volume units match. The moles of solute stay constant during dilution.
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