Heterogeneous mixture
Freezing point
...of a solution will decrease when a solute is added
Boiling point
...of a solution will increase when the solute is added.
Emulsion
A colloid in which liquids that don't mix are spread throughout each other. Ex cream. Appear uniform but it's not
Solubility curve
A comparison of the solubility of a substance when the temperature of the solvent is varied
Homogeneous mixture
A mixture that looks uniform even when examined closely bc individual components are evenly dispersed and too small to be seen. All are solutions
Suspension
A mixture where particles can settle out when allowed to stand. Filtered Are immiscible
Colloid
A mixture with smaller particles of a suspension and they dispersed throughout each other. (Can't filter)
Non polar m
A molecule where electrons are shared equally in a covalent bond
Polar molecules
A molecule where electrons are shared unequally in a covalent bond
Ionizing
A process where ions are formed when a substance is dissolved in water
Concentrated
A solution with a large amount of solute.
Dilute
A solution with a small amount of solute
pH
A value that identifies the concentration of H+1 ions in a solution, which is used to determine how acidic or basic solution is
Strong acids
Acids that are completely ionized in aqueous solution (100%)
Weak acids
Acids that ionize slightly in aqueous solution.
Colligative properties
Any property that can be changed due to change in the number of particles in the solution 1.conductivity 2.boiling point 3.freezing point
Strong base
Bases that complete dissociate to form OH-1 ions
Weak bases
Bases that react with water to form the hydroxide ion and the conjugate acid of the base.
Acids
Compounds that form hydrogen compounds when dissolved in water
Bases
Compounds that form hydroxide ions when dissolved in water. OH-1
Unsaturated solution
Contains less than the maximum amount of solute to dissolve in a solvent
Supersaturated solution
Contains more than the maximum solute that can be dissolved at that temperature in a solvent
Saturated solution
Contains the maximum amount of solute that can dissolve in a solvent
Strong electrolytes
Electrolytes where nearly all the solute dissolves in the solvent and separates
Alloy
Homogenous mixture of two or more metals
Heyerogenous mixture
Mixtures that dont have fixed compisitions. Can see the diff. phased
Salt refers to any ionic compound
Negative and positive. Metal plus nonmetal
Hydrogen bonds
Occurs when a hydrogen atom bonded to a highly electronegitive atom is attracted to a lone pair on an atom in another molecule
Neutralization Reactions
Reactions in which a acid and a base react
Electrolytes
Solutes in solutions that will conduct electric currents
Non electrolytes
Solutes in solvents that will not conduct electric currents
Conductivity
Special material that conducts electricity. -it's determined based on the solute Ionic conducts and covalent won't conduct electricity
3 types of heterogenous mixtures
Suspension colloid Emulsion
Solubility
The maximum amount of solute that can dissolve in a 100 g of a solvent at a certain temperature and pressure.
Solvation
The process of the solvent surrounding the solute for dissolving
Concentration
The quantity of solute that is dissolved in a given volume of solution
Tyndall effect
The scattering of light due to particles in a mixture
Solvent
The substance that dissolves the solute
Solute
The substance that dissolves. Separates into the smallest particles.
Indicators
Ways to measure pH. They change colors in specific ranges to determine if a substance is acid or base
Weak electrolytes
When only some on the solute dissolves in solvent and separates
Dissociate
When the compound splits to form two new ions