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Properties of Solutions

Properties of Solutions. There are many factors that affect whether a substance will dissolve and the rate at which it dissolves. Properties of Solutions. The compositions of the solvent and the solute determine whether or not a substance will dissolve.

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Properties of Solutions

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  1. Properties of Solutions • There are many factors that affect whether a substance will dissolve and the rate at which it dissolves

  2. Properties of Solutions • The compositions of the solvent and the solute determine whether or not a substance will dissolve. • For example, sand will not dissolve in tea • Even if it is agitated or heated

  3. Properties of Solutions • The following factors will determine how soluble a substance is if the substance is soluble in the solvent • Agitation • Temperature • Particle size

  4. Properties of Solutions • Agitation - If the contents of the glass are stirred, the crystals dissolve more quickly.

  5. Properties of Solutions • Temperature also influences the rate at which a solute dissolves.

  6. Properties of Solutions • The rate at which a solute dissolves also depends upon the size of the solute particles.

  7. Properties of Solutions • Solutions can be described with three general terms: • Saturated - A saturated solution contains the maximum amount of solute for a given quantity of solvent at a constant temperature and pressure • Unsaturated - A solution that contains less solute than a saturated solution at a given temperature and pressure is an unsaturated solution • Supersaturated - A supersaturated solution contains more solute than it can theoretically hold at a given temperature.

  8. Properties of Solutions • The solubility of a substance is the amount of solute that dissolves in a given quantity of a solvent at a specified temperature and pressure to produce a saturated solution. • Solubility is often expressed in grams of solute per 100 g of solvent (g/100 g H2O). • Sometimes the solubility of a gas is expressed in grams per liter of solution (g/L).

  9. Properties of Solutions • Some liquids—for example, water and ethanol—are infinitely soluble in each other. • Two liquids are miscible if they dissolve in each other in all proportions. • Liquids that are insoluble in each other are immiscible.

  10. Solubility (g/100g H2O) Temperature (°C) Properties of Solutions • The solubility of most solid substances increases as the temperature of the solvent increases.

  11. Properties of Solutions • Although we can use these terms to describe solutions, there is a more specific way to show the concentration of a solution • The concentration of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent. • A solution that contains a relatively small amount of solute is a dilute solution • Aconcentrated solution contains a large amount of solute

  12. Molarity (M) = moles of solute liters of solution Properties of Solutions • In chemistry, the most important unit of concentration is molarity. • Molarity is also known as molar concentration.

  13. Properties of Solutions Intravenous (IV) saline solutions are often administered to patients in the hospital. One saline solution contains 0.90 g NaCl in exactly 100 mL of solution. What is the molarity of the solution?

  14. Properties of Solutions Household laundry bleach is a dilute aqueous solution of sodium hypochlorite (NaClO). How many moles of solute are present in 1.5 L of 0.70 M NaClO?

  15. volume of solute Percent by volume (%(v/v)) =  100 volume of solution Properties of Solutions • Percent by volume of a solution is the ratio of the volume of solute to the volume of solution

  16. Properties of Solutions What is the percent by volume of ethanol (C2H6O, or ethyl alcohol) in the final solution when 85 mL of ethanol is added to 250 mL of water?

  17. mass of solute Percent by mass (%(m/m)) =  100 mass of solution Properties of Solutions • Another way to express the concentration of a solution is as a percent by mass, or percent (mass/mass).

  18. Properties of Solutions How many grams of glucose (C6H12O6) are needed to make 2000 g of a 2.8% glucose (m/m) solution?

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