Solutions Flashcards
Arrhenius
Ionic compounds dissolve in water to conduct electricity
Why are ionic compounds so soluble in water?
When a substance dissolves in solution, particles of the substance separate from each other (breaks down into its ions)
Electrolytes
When electrolytes dissolve in solution both positive and negative charged particles are present
Non-electrolytes
- When non-electrolytes are dissolved in solution, neutral particles separate
- neutral particles don’t conduct electricity
Dissociation
- Separation of ions that occurs when an ionic compound dissolves in water
- Do not show water as reactant or product
- Pos. + Neg. = electrolytes
Bases
- Bases are ionic hydroxide compounds that dissociate in water and form a cation and hydroxide anion
Ex: NAOH (s) -> Na+ (aq) + OH- (aq)
Acids
- Considered molecular compounds but conduct electricity in solution
- Acids ionize into positive hydrogen ions (H+) and negative ions when dissolved in water
Ionization
- Process when neutral atom or molecule is converted to an ion
- only applies to acids beginning with hydrogen
- Pos. hydrogen ions + negative anions = electrolytes
Endothermic reactions
- Absorb energy from their surroundings
- Require energy
Ex. Breaking bonds
Exothermic reactions
- Release energy to their surroundings
Ex. Forming new bonds
Saturated Solution
- A solution that contains the maximum amount of dissolved solute in the presence of a undissolved solute.
- Some undissolved solute mist be present
Super saturated solution
- Solution that contains more dissolved solute than its solubility at a given temperature
2 ways to make a solution
- Preparing solutions from a solid to make a standardized solution
- Preparing solutions from a standardized solution using dilution
Standard solution
- Pre-made solution that has an accurate known concentration
- Made by adding a known mass of a solid to a known volume of a solvent
Stock Solution
Initially concentrated solution from which samples are taken and diluted
(standard solution)
Prepare standard solution by dilution
- Use stock solution and add solvent to decrease concentration to desired lvl
- Adding solvent to solution does not change quantity of solute (Mass of solute before and after is the same)
Amount concentration
- Chemical amount of solute dissolved in one litre of solution
- c =n/v
(mol/L)
Concentration of ions
- Dissociation/Ionization allow us to determine the amount concentration of ions or compounds
- [unknown]=[known] x mol unknown/ mol known
What happens to the concentration of a solution when more solute or solvent is added?
Solute- more concentrated
Solvent- decreased
Concentrated solution
A solution that contains a large amount of solute, more than the amount it can dissolve
Parts per million formulas
1 ppm = 1mL/L = 1mg/kg
ppm = g(10^6)/g
Collision-reaction theory
Easiest way to get entities of a compound to collide w/ each other to form new entities is to dissolve them in solution
Spectator Ions (net ionic equation)
Identical entities that don’t take part in the chemical reaction
Equivalence Point
The point at which the exact theoretical amount of titrant has been added to completely react with the sample
Endpoint
Th epoint during a titration when there is a sudden observable change
pH Titration Curve
A graphic description of the reaction between acids and bases showing the progress of the reaction
- y axis represents volume of titrant added
- x-axis represents pH
