solutions part 1 Flashcards
——– is formed when one substance dispersed uniformly throughout another
solution
other name for solution
homogeneous mixture
2 components of homogeneous mixture
solute and solution
meaning its components are not visible to the naked eye
homogeneous in nature,
TRUE OR FALSE
A Solution scatters in a light beam.
false
A Solution does not scatter a light beam because there are no particles to obstruct the light.
The ——–, which is the scattering of light by particles in a mixture, occurs in suspensions, not in solutions.
Tyndall effect
where does the Tyndall effect occur?
in suspensions
true or false
Components of a solution can be separated using simple mechanical filtration.
false
Components of a solution cannot be separated using simple mechanical filtration.
——— is the liquid then ——- is the particles na nag settle down or also known as precipitate.
- Supernatant
- residue
The maximum amount of a substance that can be dissolved in a given volume of solvent.
solubility
when a substance can be dissolved in a solvent.
Soluble
when a substance cannot be dissolved in a solvent.
Insoluble
Two liquids that are soluble in each other.
Miscible
Two liquids that are not soluble in each other.
immiscible
The solubility of a substance depends on the —- of both the solute and the solvent.
polarity
true or false
substances with similar polarities dissolve well in each other. The greater the difference in polarity, the lower the solubility.
true
factors affecting solubilty (3)
polarity
temp
pressure
—- is when an entity contains two distinct and opposite poles that can either attract or repel each other
Polarity
true or false
increasing the temp decreases the solubility of the solute in the solvent
false
increasing the temp increases the solubility
For —- solutes, the effect of pressure on solubility is negligible,
meaning it has little to no effect.
solid
true or false
The solubility of a gas in a liquid is directly proportional to the applied pressure.
true
a physical or chemical situation where a system can take no more of a substance
saturation
When equilibrium is reached the rates of dissolution and precipitation are equal, there is some dissolved and some undissolved solute. this state indicates that the solvent has dissolved as much solute as possible, and any additional solute will remain undissolved.
dynamic equilibrium
Contains the maximum amount of a
given solvent at a specific temperature
Unsaturated Solution
Contains less solute than it has the
capacity to dissolve
Saturated Solution
Contains more solute than is present
in a saturated solution
Supersaturated Solution
are often formed by heating the solvent to dissolve more solute than it normally would at lower temperatures. As the solution cools, the excess solute remains dissolved until disturbed.
Supersaturated Solution
These are the forces of attraction between molecules of the solute and solvent.
INTERMOLECULAR ATTRACTIONS
These forces determine how well the solute and solvent interact to form a solution. For a solution to form, the —————-between the solute and solvent must be compatible, meaning the polarity of both should be similar for effective interaction.
intermolecular forces
forces within the molecules themselves. Before the solute and solvent can interact, the —— holding the solute particles together and those holding the solvent molecules together must be overcome.
intramolecular forces
true or false
breaking of bonds is not necessarry to allow the solute and solvent to mix
false
breaking of internal bonds allows the solute and solvent to mix.
Solvent particles surround solute particles, effectively coating them and leading to the dissolution of the solute in the solvent. When water is the solvent, the process is called ————-.
hydration
As solvation occurs, the solvent particles form a cage-like structure around the solute particles, trapping them within this ——
“solvent cage.”
Dissolution overall can be either —- or —–
endothermic or exothermic
true or false
Whether the dissolution is endothermic or exothermic depends on the balance between the energy required to break the initial bonds (in the solute and solvent) and the energy released when new bonds are formed during solvation. If more energy is required, the process is exothermic if more energy is released, it is endothermic
false
if more energy is required, the process is endothermic; if more energy is released, it is exothermic.
Energy is released, meaning the
formation of new bonds between the solute and solvent releases more energy than is needed to break the original bonds. This results in an increase in temperature.
- more energy released in mkaing bonds
exothermic
Energy is absorbed, which means
more energy is required to break the bonds within the solute and solvent than is released when new bonds are formed between them. This results in a DECREASE in temperature.
endothermic
steps of solution (3)
solvent solvent
solute solute
solute solvent
step?
The forces holding the solute
particles together must be overcome for the solute to dissolve.
solvent solvent (1)
step?
After the solute andsolvent
molecules are separated, new interactions (or bonds) form between them. This is crucial for the formation of a solution.
solute solute (2)
step?
Thesearetheinteractionsthatoccur
between solute and solvent molecules once the solute has been dispersed. The strength of these interactions determines whether the solute will stay dissolved or precipitate out of the solution.
solute solvent (3)
types of imf
weakest to strongest (5)
LONDON dispersion
dipole induced
dipole dipole
h bonding
ion dipole
IMF:
Weakest, occurs between all molecules, especially nonpolar ones.
london dispersion
imf: Occurs when a polar molecule induces a dipole in a nonpolar molecule.
dipole induced
imf: Occurs between two polar molecules.
dipole dipole
imf: Occurs when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine.
H bonding
imf: Strongest, occurs between an ion and a polar molecule.
ion dipole
true or false
hotter temperatures are more ideal for dissolving gases in a solvent.
false
, lower temperatures are more ideal for dissolving gases in a solvent.
true or false
Heating up the solution makes the solid solute dissolve more easily.
true
this states that the solubility of gases is directly proportional to the partial pressure of the gas above the liquids
henry’s law
t or f
When pressure increases over the solvent, it allows the molecules of gases to interact more with the solvent
true
t or f
Increasing the pressure compresses gas particles, bringing them closer to the solvent molecules, which enhances solubility. Conversely, decreasing the pressure results in lower solubility as gas particles spread out.
t
a solutiion can be —- or —-
dilute or concentrated
Solution contains less solute than solvent.
dilute
Solution contains more solute than solvent.
concentrated
