concentration

• How can solutions be classified?

  Solutions can be classified as saturated, unsaturated, or supersaturated.
• What is the definition of the concentration of a solution?

  The concentration of a solution is defined as the quantity of solute dissolved in a quantity of solution.
• How can concentration be represented?

  Concentration can be represented by the number of moles of solute per litre of solution, mass of solute per litre of solution, or parts per million (ppm).
• What is a dilute solution?

  A dilute solution contains a small amount of solute in a large volume of solvent.
• What is a concentrated solution?

  A concentrated solution contains a large amount of solute dissolved in a relatively small volume of solvent.
• What does grams per litre (g L^-1) indicate?

  Grams per litre indicates the number of grams of solute dissolved in one litre of solution.
• What is percentage composition by mass?

  Percentage composition by mass states the mass of solute in grams dissolved in every 100 g of solution.
• What does parts per million (ppm) measure?

  Parts per million measures the mass of solute in milligrams per kilogram of solution.
• What is the formula for calculating concentration in grams per litre?

  The formula is concentration of solution = mass of solute ÷ volume of solution.
• What does molarity (M) refer to?


  Molarity refers to the number of moles of solute per litre of solution.
• What does percentage composition by mass indicate?

  Percentage composition by mass indicates the mass of solute in relation to the total mass of the solution.
• What does parts per million (ppm) measure in a solution?

  Parts per million measures the mass of solute in milligrams per kilogram of solution.
• What does parts per million (ppm) represent in a solution?


  Parts of solute in one million parts of solution
• What is the effect of adding more solvent to a solution during dilution?

  • The number of molecules remains unchanged
  • Volume of the solution increases
  • Molecules are spread further apart
  • Concentration is decreased
• What is the procedure to prepare a dilute solution from a concentrated solution?


  Measure a known volume of concentrated solution, transfer to a volumetric flask, fill with distilled water, and stopper.
• How do you calculate the volumes required for the dilution process?

  Using the formula \( c_1 V_1 = c_2 V_2 \)
• What does \( c_1 \) and \( V_1 \) represent in the dilution formula?

  \( c_1 \) and \( V_1 \) are the concentration and volume of the concentrated solution before dilution
• What does \( c_2 \) and \( V_2 \) represent in the dilution formula?

  \( c_2 \) and \( V_2 \) are the concentration and volume of the diluted solution
• How do ionic and covalent compounds behave when dissolved in water?

  They act as strong electrolytes and completely break up into ions.
• What are the conditions under which solutions of strong electrolytes have high electrical conductivities?

  • Solutions are not extremely dilute
  • Sufficient solubility of the strong electrolyte
• What are the characteristics of solutions of weak electrolytes?

  • Poor conductors of electricity
  • Only a small amount of dissolved molecules are ionized
• What are colligative properties of solutions?

  • Properties modified by adding a solute to a solvent
  • Depend on the number of solute particles relative to solvent particles
  • Include vapor pressure lowering, melting point depression, and boiling point elevation
• What happens to the vapor pressure when a solute is added to a solvent?

  The vapor pressure decreases due to interference with vaporization of pure solvent molecules.
• How does the boiling point change when a solute is added to a solvent?

  The boiling point increases above that of the pure solvent.
• What effect does a dissolved solute have on the freezing point of a solvent?

  The presence of a dissolved solute lowers the freezing point below that of the pure solvent.
• What are the effects of adding a solute to a solvent on its properties?

  • Vapor pressure decreases
  • Melting point decreases
  • Boiling point increases