GT Chem - Aqueous Solutions (Unit 10)

soluble

capable of being dissolved

homogeneous (what it is, and particles are ____)

evenly mixed; particles too small to distinguish

heterogeneous (what it is, and particles are _____)

unevenly mixed; different phase or particles are easily observed

solute (definition and amount)

component of a mixture in smallest amount that is being dissolved

solvent (definition and amount)

the dissolving medium; component of mixture in largest amount

dilute (amount and definition)

relatively small amount of dissolved solute

concentrated (amount and definition)

relatively large amount of dissolved solute

unsaturated

space in solvent for more solute to dissolve

saturated

max amount of solute has dissolved

supersaturated

solution that contains more dissolved solute than a saturated solution contains under the same conditions

solution (definition, particle size)

homogeneous mixture of substances in a single phase; extremely small particles; same composition and properties of throughout

electrolyte

a substance that dissolves in water to give a solution that conducts electric current

nonelectrolyte

a substance that dissolves in water to give a solution that does not conduct electric current

dissolution

process of solvent molecules surrounding and interacting with solute particles

miscible

liquids that dissolve freely in each other

immiscible

liquids that do not dissolve freely in each other

_______ dissolves ______, substances dissolve in each other if ___ matches.

Like, like, polarity

Solute: Polar molecule

Solvent: Polar molecule

Description:

Soluble/miscible

Solute: Nonpolar molecule

Solvent: Nonpolar molecule

Description:

Soluble/miscible

Solute: ionic compound

Solvent: Water (polar molecule)

Description:

Soluble via hydration

Solute: Ionic compound

Solvent: nonpolar molecule

Description:

Insoluble/immiscible

Solute: Polar molecule

Solvent: nonpolar molecule

Description:

Insoluble/immiscible

Factors that can affect the rate of solution formation:

Particle size/surface area for solids:

Smaller particles -> larger surface area -> faster

Factors that can affect the rate of solution formation:

Particle size/surface area for gases:

N/A

Factors that can affect the rate of solution formation:

Temperature of solvent for solid:

warmer = faster

Factors that can affect the rate of solution formation:

Temperature of solvent for gases:

cooler = faster

Factors that can affect the rate of solution formation:

Amount of stirring for solids:

more = faster

Factors that can affect the rate of solution formation:

Amount of stirring for gases:

less = faster (to a point)

Factors that can affect the rate of solution formation:

Amount of solute dissolved for solids (concentration):

Low starting concentration = faster

Factors that can affect the rate of solution formation:

Amount of solute dissolved for gases (concentration):

N/A

Factors that can affect the rate of solution formation:

Pressure for solids:

N/A

Factors that can affect the rate of solution formation:

Pressure for gases:

higher = faster

Positive delta H is endothermic/exothermic, absorbs/releases heat, feels hot/cold, heat transfers from your hand out/to the cup

endothermic, absorbs, cold, to

enthalpy of solution

net amount of energy absorbed as heat

Negative delta H is endothermic/exothermic, absorbs/releases heat, feels hot/cold, heat transfers through your hand out/to the cup

exothermic, releases, hot, out

Molarity

concentration measured by # of moles of solute in one liter of a solution

dissociation

the separation of ions that occurs when an ionic compound dissolves in water

A net ionic equation includes only those _ and _ that undergo a _______ __ in a reaction in a ___ ____.

compounds, ions, chemical change, aqueous solution

overall ionic equation

includes all of the soluble ions with the precipitates left as solids

net ionic equation

includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution; applies to any reaction with the same precipitate

spectator ions

ions that do not take part in the reaction and appear on both sides of the chemical reaction

hydronium (which forms when...)

the polyatomic ion with the formula H3O+ which forms when the solvent water is able to remove hydrogen from a molecular compound

Some molecular compounds (usually ____) can also form ___in solution if the solvent is ___. The process forms __ where none existed in the ____ ___.

polar, ions, polar, ions, dissolved compound

Characteristics/traits of strong electrolytes

Soluble ionic compounds, strong acids that have been ionized completely

Characteristics/traits of weak electrolytes

Weak acids/bases that have not been ionized well

Characteristics/traits of nonelectrolytes

Molecular compounds that do not ionize

What happens if you dissolve strong electrolytes?

If they dissolve in water the pretty much yield only ions

What happens if you dissolve weak electrolytes?

They exist as both ions and molecules

What happens if you dissolve nonelectrolytes?

They form no ions

What is the conductivity of strong electrolytes, weak electrolytes, and nonelectrolytes?

Strong electrolytes are good conductors, weak electrolytes are weak conductors, and nonelectrolytes don't conduct electricity at all