Solutions and Concentration

50 lessons, pages 1151–1200.

  1. Solutions as Homogeneous Mixtures — Uniform composition and dispersed particles
  2. Solute and Solvent Roles — Identifying components without relying only on physical state
  3. Aqueous and Nonaqueous Solutions — Water as solvent versus other liquid media
  4. How Dissolving Happens — Particle separation, solvent interactions and mixing
  5. Dissolving Ionic Solids in Water — Hydration and dispersed ions
  6. Dissolving Molecular Substances — Molecules, polarity and intermolecular attractions
  7. Dissolution Versus Chemical Reaction — Recognising physical mixing and new chemical species
  8. Concentration as a Ratio — Amount of solute relative to a stated solution basis
  9. Dilute and Concentrated Are Relative — Qualitative descriptions and quantitative limits
  10. Solubility at a Stated Temperature — Maximum dissolved amount in equilibrium with excess solute
  11. Unsaturated and Saturated Solutions — Comparing the present dissolved amount with equilibrium solubility
  12. Supersaturation and Crystallisation — Metastable solutions and crystal formation
  13. Rate of Dissolving Versus Solubility — Speed of reaching equilibrium versus its final concentration
  14. Stirring and Particle Size — Changing dissolution rate through mixing and surface area
  15. Temperature and Solid Solubility — Using substance-specific data rather than a universal trend
  16. Reading Solubility Curves — Amounts dissolved and undissolved from a temperature graph
  17. Crystallisation on Cooling — Predicting crystal mass from two solubility values
  18. Gas Solubility and Pressure — Partial pressure and the equilibrium dissolved gas amount
  19. Gas Solubility and Temperature — Interpreting measured trends and gas escape
  20. Henry's Law with Defined Units — Proportionality between dissolved gas and partial pressure
  21. Miscible and Immiscible Liquids — Liquid mixtures, phases and composition
  22. Polarity and Solubility — Intermolecular interactions behind qualitative predictions
  23. Mass Fraction of a Solute — Solute mass divided by total solution mass
  24. Mass Percent Concentration — Converting mass fractions to percent by mass
  25. Mass per Volume Concentration — Reporting g per litre with the solution volume specified
  26. Molarity Defined — Moles of solute per litre of solution
  27. Calculating Molarity from Mass — Molar mass and measured final solution volume
  28. Finding Solute Amount from Molarity — Using n = cV with volume in litres
  29. Preparing a Standard Solution — Weighing, dissolving and making up to a calibration mark
  30. The Volumetric Flask and Meniscus — Reading a calibrated final solution volume
  31. Dilution Conserves Solute Amount — The meaning and limits of c1V1 = c2V2
  32. Planning a Dilution — Calculating stock volume for a chosen final concentration
  33. Serial Dilution — Multiplying successive dilution factors
  34. Mixing Solutions of One Solute — Combining solute moles before finding final concentration
  35. Concentrations After Reaction — Subtracting consumed amount before dividing by final volume
  36. Concentration and Ionic Formula Units — Relating dissolved salt amount to ideal ion amounts
  37. Comparing Concentration Units — Distinguishing mass, amount and volume bases
  38. Parts per Million by Mass — Trace mass fraction and unit conversion
  39. Parts per Billion by Mass — Small mass fractions and precision limits
  40. Mole Fraction — Component moles divided by total mixture moles
  41. Molality — Solute moles per kilogram of solvent
  42. Molarity Versus Molality — Volume and solvent mass as different denominators
  43. Density and Concentration Conversion — Linking solution mass and volume carefully
  44. Concentrated Reagent Labels — Using mass percent and density to calculate molarity
  45. Concentration from Titration Data — Reaction ratio and original aliquot volume
  46. Solubility Versus Concentration — A capacity at equilibrium versus an actual amount present
  47. Water Quality Concentration Data — Interpreting dissolved-substance measurements with units
  48. Error Checks in Solution Calculations — Units, denominators, conservation and plausible magnitudes
  49. Mixed Solution Problem Set — Choosing solubility, concentration, dilution or reaction methods
  50. Solutions and Concentration: Unit Review — Integrating particle models, solubility and concentration calculations