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Apologia Chem M10

The Chemistry of Solutions

QuestionAnswer
solute the substance we are dissolving
solvent the substance in which we are dissolving the solute
solution when a solute and a solvent are mixed together
Solvents do not necessarily have to be liquids.
NaCl is a ionic compound, and ionic compounds do not have chemical bonds. The atoms donate or receive electrons, they do not share electrons.
The electronic attraction between opposite charges is the only thing that holds Na+ and Cl- ions together.
Water is a polar covalent compound, meaning it has a fractional positive charge on its hydrogen atoms and a fractional negative charge on its oxygen atoms.
Purely covalent solids do not dissolve well in water because they have no electrical charges in them.
Polar covalent solids can dissolve in water because they possess fractional charges.
Even though polar covalent molecules dissolve in water, they cannot split into smaller parts.
Ionic compounds dissolve by breaking apart into smaller pieces of their individual ions.
Polar covalent compounds dissolve by separating each individual molecule from its neighbors.
In the solid phase, the solvent molecules must be attracted to the solute molecules so strongly that the solvent molecules can get between the solute molecules (or ions) and pull them far apart from each other.
In the liquid phase, the solvent molecules need to be attracted to the solute molecules only a small amount because the solvent does not need to separate the solute molecules very much. The solvent merely needs to get between the solute molecules.
In the gas phase, the solvent molecules must be attracted to the solute molecules enough to pull the solute molecules closer to one another.
solubility the maximum amount of solute that can dissolve in a given amount of solvent
The solubility of any solute depends on both the identity of the solute and the identity of the solvent.
saturated solution a solution in which the maximum amount of solute has been dissolved
precipitation the process by which a solute leaves a solution and turns back into its solid phase
The solubility of solid solutes usually increases with increasing temperature.
The solubility of liquid solutes is not affected by temperature.
The solubility of gases decreases with increasing temperature.
Increasing pressure increases the solubility of gases.
Pressure does not affect the solubility of liquids or solids.
exothermic a process that lets out heat
endothermic a process that absorbs heat
Most solids dissolved in an endothermic fashion. They must absorb energy to dissolve properly.
molality the number of moles of solute per kilogram of solvent
formula for molality m = (# moles solute)/(#kg solvent)
When calculating molality, we are concerned with mass, not volume.
When calculating molality, we divide only by the mass of the solvent - NOT by the mass of the solution.
freezing point depression when a solute is dissolved in a solvent, the freezing point of the solution will be lower than that of the pure solvent
boiling point elevation when a solute is dissolved in a solvent, the boiling point of the solution will be higher than that of the pure solvent
Kf freezing point depression constant
Kb boiling point elevation constant
i number of molecules or ions that the solute splits into when it dissolves
A negative sign in a temperature change equation means that the temperature dropped.
melting point another name for freezing point
Created by: MrsHough
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