WATER & COLLIGATIVE PROPERTIES IN...
Transcript of WATER & COLLIGATIVE PROPERTIES IN...
WATER & COLLIGATIVE PROPERTIES IN SOLUTION
The Importance of Water
¨ Water is a polar molecule. ¤ Polarity creates many dipoles throughout the sample of
water.
¨ Because of this, it is a great solvent for various substances. ¤ This explains why water is known as the “universal
solvent”.
Hydrogen Bonds
¨ Intermolecular dipole interactions create a network of hydrogen bonds (H-bonds) ¤ Affect several properties
of water n Examples: Low vapor
pressure & high surface tension
Surface Tension
¨ Makes it possible for water striders to “walk” on water.
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Vapor Pressure
¨ Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure. ¤ Because hydrogen bonds hold water molecules to one
another, the tendency of these molecules to escape is low, and evaporation is slow.
¨ This relates to water’s high boiling point.
Ice vs. Water
¨ The structure of ice is a regular open framework of water molecules arranged like a honeycomb
¨ When ice melts, the framework collapses, and the water molecules pack close together, making the liquid water more dense than ice.
Colligative Properties
¨ Properties of a solvent that are changed when a solute is added.
¨ The type of solute you add does not matter but how many particles you add does. ¤ For example: it only matters how many ions you add, not which
ones.
¨ The type of solvent matters ¤ Each solvent is different and is affected by different amounts of
solutes. ¤ Example: adding 10g of NaCl may affect water differently than
adding 10g of NaCl to ethanol.
What do Colligative Properties Affect?
¨ There are three major effects of colligative properties: 1. Vapor Pressure lowering 2. Boiling point elevation 3. Freezing point depression
¨ The magnitude of each of these all depend on how many particles have dissolved, not upon their identity
¨ Magnitude of effect is based partially on the molality of the solution
¤ When it is molecular NOT ionic
What makes these things happen?
¨ In each process, energy is expended to either bring molecules together (freezing) or pull them apart (boiling).
¨ If a substance is present between (i.e. dissolved) the
solvent molecules, the solvent has to use more energy to complete the processes.
¨ This forces the solvent to deviate from its normal
freezing and boiling points.
Expression of Number of Particles
¨ To express the number of particles as a colligative property, chemists use molality.
¨ Molality (m) is the number of moles of solute dissolved in
1kg of solvent. ¨ Also known as “molal concentration”
Molality Example #1
¨ How many grams of sodium bromide, NaBr, must be dissolved in 400g of water to produce a 0.500 molal solution?
Freezing Point Depression
¨ Freezing point depression: ¤ Adding a solute to a liquid will
cause freezing point of the liquid to drop by a predictable amount
¤ Electrolytes (acids/bases and ionic
compounds) will have a greater effect based on the total number of ions placed into solution
¤ The constant, Kf, is the molal
freezing point depression constant n Equal to the change in freezing
point for a 1-molal solution of a nonvolatile molecule solute
Freezing Point Depression
Freezing Point Depression Example
¨ If you use 3.68mol of sucrose (C12H22O12) and dissolve this into 2.50kg of water, what will be the change in the freezing point of your solution? Assume the Kf of water is -1.86oC/m.
Boiling Point Elevation
¨ Boiling point elevation: ¤ Adding a solute to a liquid will cause
the boiling point of that liquid to rise by a predictable amount.
¤ Electrolytes (acids/bases and ionic compounds) will have a greater effect based on the total number of ions placed into solution.
¤ The constant, Kb, is the molal boiling
point elevation constant n equal to the change in boiling point for
a 1-molal solution of a nonvolatile molecular solute.
Boiling Point Elevation
Boiling Point Elevation Example
¨ If you use 5.76mol of sodium fluoride (NaF) and dissolve this into 3.62kg of water, what will be the change in the boiling point of your solution? Assume the Kb of water is 0.51oC/m.