Chapter 4: Solutions Flashcards
Compound of which there is MORE is called a ______ and the compound of which is LESS is called _______.
When neither compound predominates, BOTH compounds are referred to as ________.
Solvent; Solute
Solvents
3 Types of solutions
1) Ideal solutions - made from compounds that have similar properties (meaning compounds can be interchanged within the solution w/o changing spatial arrangement of the molecules or intermolecular attractions); Example: Benzene in toluene
2) Ideally dilute solutions - solute molecules are completely separated by solvent molecules so they have NO interaction with each other.
3) Nonideal solutions - violate both conditions
Example of Colloid
Hemoglobin
Colloidal system can be any combination of phases except for…
Gas in gas
Example of colloidal systems
Aerosol - LIQUID or SOLID particles in a gas like fog/smoke
Foam - GAS particles in a LIQUID (like whipped cream)
Emulsion - LIQUID particles in a LIQUID or solid like milk or butter
Sol - SOLID particles in LIQUID like paint
Colloid particles may be ATTRACTED (_________) or REPELLED (________) by their dispersion medium.
Lyophilic; lypophobic
Lypophobic colloids form when amphipathic (hydrophilic and hydrophobic parts) or charged particles ________ to the surface of the colloidal particles which stabilizes them in the dispersion medium.
Absorb
General rule for dissolution (dissolving) is…
‘Likes dissolve likes’
These molecules are held together by STRONG intermolecular bonds formed by the attraction b/n their __________ charged ends.
These molecules are held together by WEAK intermolecular bonds resulting from instantaneous _________ moments.
These forces are called….
Highly polar molecules; partially charged
Nonpolar molecules; dipole
London dispersion forces
A ________ solute interacts with a _________ solvent by tearing __________ bonds apart and forming ___________ bonds.
Polar; polar
Solvent-solvent; solvent-solute
No polar solvent can tear apart a WEAK bond of a _________
Nonpolar solvent
Ionic compounds are dissolved by ….
Polar substances
Process of Solvation
When ionic compounds dissolve, they break apart into their respective cations and anions and are surrounded by OPPOSITELY charged ends of the POLAR SOLVENT.
When water molecules surround individual ions pointing their positive hydrogens at the anions (-) & their negative oxygens towards cations (+)
When several molecules attach to one end of an ionic compound, they’re able to overcome the strong ionic bond, and break the compound. The water molecules then surround ion. In water this process is called ….
Hydration
Something that’s hydrated is …
Define hydration number
An aqueous phase
Number of water molecules needed to surround an ion that varies according to the size & charge of the ion. *This # is commonly 4 or 6
Compound that forms ions in an aqueous solution is called an …
STRONG electrolytes
WEAK electrolytes
Electrolyte
Create solutions which CONDUCT ELECTRICITY well and CONTAIN MANY IONS.
Compounds which form FEW IONS in solution
- Nitrite
- Nitrate
- Sulfite
- Sulfate
- Hydrochlorite
- Chlorite
- Chlorate
- Perchlorate
- Bicarbonate
- Phosphate
- NO2-
- NO3-
- SO3^2-
- ClO-
- ClO2-
- ClO3-
- ClO4-
- CO3^2-
- HCO3^-
- PO4^3-
Fun fact: what is “HYPONATREMIA”
What are NORMAL sodium levels?
What low sodium levels due to drinking too much water can be critical or even lead to death?
When sodium levels become too low (reduced sodium levels) as a result of drinking too much water
135mM-145mM
125-120mM or lower
5 Ways to measure concentration
1) Molarity (M): mols of compound/ vol of solution (unit: mol/vol)
2) Molality (m): mols of solute/ kg of solvent (unit: mol/kg)
3) Mole Fraction (X): mols of compound/ total moles of all species in sol’n (units: NONE)
4) Mass percentage: 100 x’s the ratio of the mass of the solute/ total mass of solution
5) Parts per million (ppm): 10^6 x’s the ratio of the mass of solute/ total mass of solution
Define a solution
Homogenous mixture of 2 or more compounds in a solid, liquid, or gas
Example: Brass
A solid solution of zinc and copper