Properties of Solutions

Solutes dissolved in an aqueous medium are classified based on their ability to form _____

Ions

A substance that ionizes (breaks down) in water into positive ions (cations) and negative ions (anions)

Electrolyte

________ electrolyte solutions conduct an electric current

Aqueous

Ionize completely in water, leading to strong current conduction

Strong electrolytes

Examples are strong acids, strong bases, and most of their salts (NaOH, HCl, NaCl, KOH, KCl)

Strong electrolytes

Ionize only partially in water, resulting in weak current conduction

Weak electrolytes

Examples are weak acids and bases, such as acetic acid, benzoic acid, NH4OH, and atropine

Weak electrolytes

A substance that does not ionize in water

Non-electrolyte

Examples are sugars, alcohol, and acetone

Non-electrolytes

Properties of solutions that depend only on the number of solute particles (molecules or ions) present in the solution, not on the identity of the solute

Colligative properties

Solutions with the same ______ of particles will have the same colligative properties

Number

Equimolar concentrations of various solutes should have equal _________ properties, assuming they don’t ionize differently

Colligative

The four colligative properties

Vapor pressure, boiling point, freezing point, and osmotic pressure

Adding a solute results in a ________ in vapor pressure

Decrease

Adding a solute results in an __________ in boiling point

Increase

Adding a solute results in a __________ in freezing point

Decrease

Adding a solute results in _________ _________

Osmotic pressure

Adding a non-volatile solute to a pure solvent __________ the vapor pressure of the solution compared to the pure solvent

Decreases

Adding a solute decreases the vapor pressure because the solute particles occupy some of the ________ ______, reducing the rate at which solvent molecules can escape into the gas phase

Surface area

The decrease in vapor pressure is proportional to the _____ ________ of the solute

Mole fraction

The temperature at which the vapor pressure of the liquid equals the external pressure

Boiling point

Since adding a solute lowers the vapor pressure, the solution requires a _________ temperature to reach the external pressure, thus elevating the boiling point

Higher

The increase in boiling point is proportional to the ______ concentration of solute

Molal

Moles of solute per kg of solvent

Molality

The temperature at which the solid and liquid phases of a substance are in equilibrium

Freezing point

The addition of a solute increases the _______ of the solvent, making it more difficult for the solvent to become ordered into a solid crystal lattice, thus decreasing the freezing point

Entropy

The freezing point depression is proportional to the _________ of the solution

Molality

The diffusion (movement) of small molecules, typically solvent (water), through a semi-permeable membrane

Osmosis

A ________ ________ membrane allows the passage of solvent and small ions, but not large solute molecules

Semi-permeable

_____ ________ are semi-permeable

Cell membranes

Osmosis moves the solvent from a region of ____ solute concentration to a region of _____ solute concentration to equalize the concentrations on both sides

Low to high

The pressure that results from osmosis; it is also defined as the minimum external pressure necessary to stop (or reverse) the process of osmosis

Osmotic pressure

An assumption of colligative properties is that the solute is _________ and the solvent is water

Non-volatile

An assumption of colligative properties of solutions is that the solution is ________

Dilute

Vapor pressure of water at room temperature

23.77 mm Hg

Freezing point of water

0 degrees C

Boiling point of water

100 degrees C

Osmotic pressure of pure water does _____ _______

Not exist

Addition of a nonvolatile solute results in a vapor pressure _________

Decrease

Addition of a nonvolatile solute results in a boiling point _________

Increase

Addition of a nonvolatile solute results in a freezing point __________

Decrease

Addition of a nonvolatile solute results in _________ _________

Osmotic pressure

For electrolytes, a _________ ________ is used for colligative properties to account for ionization

Correction factor

Correction factor used for colligative properties of electrolytes

Van’t Hoff factor

Represents the number of ions (particles) formed when a solute is dissolved in water

Van’t Hoff factor

This is equal to the total number of product particles divided by the number of starting particles

Van’t Hoff factor

An empirical value used as a modification of the Van’t Hoff equation for freezing point depression

Liso

This is the isotonic value and is equal to the product of the Van’t Hoff factor and Kf

Liso

Refers to the property of a solution relative to a semi-permeable membrane that determines the direction and extent of water flow

Tonicity

The normal body fluid osmolality

300 mOsmol

The generally accepted freezing point of both blood serum and lacrimal fluids

-0.52 degrees C

Same concentration of particles; no net water gain or loss; cells remain stable

Isotonic

IV fluid must be _________

Isotonic

More electrolytes/concentrated; water moves out of the cells; cell shrink (dehydration)

Hypertonic

Hypertonic solutions have freezing points ______ than -0.52 degrees C

Lower

Water is added to these solutions to dilute them and make them isotonic

Hypertonic

Fewer electrolytes/dilute; water flows into cells; cells swell (hemolysis/burst)

Hypotonic

Hypotonic solutions have freezing points that are ______ than -0.52 degrees C 

Higher

NaCl or dextrose is added to these solutions to increase solute and make them isotonic

Hypotonic

Many pharmaceutical agents need to be ________ with body fluids

Isotonic

Isotonic concentration for sodium chloride

0.9%

The mass of NaCl that produces the same osmotic pressure (particle effect) of 1 g of the given substance

E value