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Solutions
Part 1
Question | Answer |
---|---|
Solutions are what kind of mixture? | homogenous |
What states can solution be in? | gas, liquid, or solid |
solvent | he component in the solution with the highest concentration |
condensed states | the liquid states, and the solid states |
What if the attractive force of solute molecules for other solute molecules are greater than the attractive forces of solute molecules for water? | then the solute will not dissolve |
What does the lattice energy describe? | the attractive force between the solute molecules (like ions) |
solvation | process where the solute-solvent interactions are strong enough to separate, surround, and disperse a solute |
hydration | the solvation process where the solvent is water |
enthalpy of solvation | the process of solvation that involves energy changes. This is a physical process, not chemical |
enthalpy of solvation 1: | dispersing the solutes. It is the lattice energy |
energy of solvation 2: | water molecules have to separate from one another to provide the necessary space to accomodate the dispersed solutes |
energy of solvation 3: | energy associated with the formation of solvent-solute intearction |
separating the solute molecules from each other is endothermic or exothermic? | endothermic |
disrupting solvent-solvent interaction to allow space for dispersed solute molecules is endothermic or exothermic? | endothermic |
formation of solvent-solute inteaction is endothermic or exothermic? | exothermic |
Process in which the overall heat energy of the system decreases tend to be what? | spontaneous (example: a negative value for the overall heat change indicates spontaneity) |
processes in which the disorder of the system increases tend to be what? | spontaneous |
entropy | the degree of disorder |
high entropy is what? | disordered |
low entropy is what? | ordered |
concentrated solution | solute is present in high concentration |
diluted solution | where the solute is present in low concentration |
ppm stands for? | parts per million |
ppb stands for? | parts per billion |
the density of diluted aqueous soltuion can be assumed to be equal to the density of what? | pure water |
1.0 L of diluted aqueous solution has a mass of what? | 1000 g |
the sum of mole fractions of all components in a solution (including the solution itself) must equal | 1.0 |
molality (m) | moles of solute / kilograms of solvent component |
crystallization | collision of dispersed ions with remaining crystals, resulting in an increase in the crystal mass |
saturated | a solution that is in dynamic equilibrium with undissolved solute |