Chapter 13 Flashcards
(30 cards)
Solution
Homogeneous mixture of two or more substances in a single phase.
Range in size .01 to 1 nm in diameter
Solvent
Dissolving medium in a solution: doing the dissolving.
Solute
Dissolved in the solution: being dissolved
Lesser amount
Remained mixed b/c of size
Types of solute/solvent combos and examples.
Solid in liquid: sodium hypochlorite(NaClO), coffee
Liquid in liquid: dish soap in H2O, shampoo
Gas in liquid: CO2 in H2O, O in H2O
Gas in gas: oxygen in nitrogen
Liquid in gas: humidity H2O in air
Solid in gas: Smoke
Solid in solid: alloy (copper in nickel, gold silver)
Liquid in solid: Mercury in silver
Gas in solid: charcoal filter
Suspension
Temporary mixture; particles will settle unless constantly mixed/stirred
Particles are larger more than 1000 nm
Collid
Particles don’t settle due to random motion
Large enough to see
Particles that are intermediate in size b/w those in solutions and suspensions form mixtures.
1nm-1000nm
Types and examples of collids
Emulsion: peanut butter, mayo
Aerosol: fog
Foam: shaving cream, whipped cream
Tyndall effect
Property of collids
Scattering of light from particles dispersed in a collid
Electrolytes
Solutions that conduct electricity.
A substance that dissolved in water to give a solution that conducts electric current
NaCl
Na+ Cl- ironically bonded
Nonelectrolyte
Solutions that don’t conduct electricity.
A substance that dissolved in water to give a solution that does not conduct an electric current.
Sugar
No ions covalently bonded.
Dissolving Process
- Salvation: solvent particles surround solute particles due to attractions
- Hydrated ions: solute ions surrounded by solvent particles
- Dissolution: hydrated ions are now separated
Continues til equilibrium is reached
Rate of dissolving
- Heat the solvent: faster particles come in contact with solute particles quicker
- Stirring(agitating): more solute/solvent contact by forcing it.
- Crush solute (increase surface area): more solute solvent contact
Solution equilibrium
Rates of dissolving equals the rate of crystallization
Physical state at which the opposing processes occur at the same rate.
Saturated solution
Max amount of solute dissolved in a given amount of solvent at a given temperature.
Unsaturated solution
Less than the max amount dissolved
Under existing condition
Supersaturated solution
More than the max amount that is dissolved
Under the same conditions
Can remain unchanged unless disturbed
Solubility
The amount of solute that can dissolve in a given amount of solvent at a specific temperature.
Amount of that substance required to form a saturated solution with a specific amount of solvent at a specified temperature
Hydration
Solution process with water as the solvent
4 possibilities for solute/solvent particles
Polar solute/polar solvent: yes form solution NaCl in H2O \+&- attractions b/w solute and solvent Nonpolar solute/ polar solvent: no Silicon dioxide in water Not enough attraction Polar solute/ Nonpolar solvent: no NaCl in alcohol Not enough attractions to separate solute particles Nonpolar solute/Nonpolar solvent: yes Oil in alcohol London dispersion- weak attractions "Likes dissolve likes"
Immiscible
Liquid solutes and solvents not soluble in each other
Toluene in H2O
Miscible
Liquids that dissolve freely in one another in any proportion
Soluble in one another
Benzene in carbon tetrachloride
Henry’s Law
The solubility of a gas in a liquid is directly proportional to the particle pressure of that gas above of the liquid
Effervescence
The rapid escape of a gas from a liquid in which it is dissolved
Solvated
A solute particle that is surrounded by solvent molecules.
