Chapter G: Solutions Flashcards
- may be a liquid, gas, or solid.
- are spread evenly throughout the solution
- mix with solvents so the solute and solvent have the same physical state.
- cannot be separated by filtration, but they can be separated by evaporation.
- are not visible, but they can give a color to the solution
Solutes
Solutes cannot be separated by ____, but they can separated by ____.
- Filtration
- Evaporation
- is one of the most common solvents in nature.
- is a polar molecule due to polar O–H bonds.
- molecules form hydrogen bonds important in many biological compounds.
Water
How does solutions form?
When solute-solvent interactions are lare enough to overcome solute-solute and solvent-solvent interactions
Solute: Polar
Solvent: polar
Solute: non polar
Solvent: nonpolar
play an important role in maintaining the proper function of the cells and organs.
Electrolytes
Examples of Electrolytes
Sodium, Potassium, Chloride, Bicarbonate
dissociate 100% in water, producing positive and negative ions
Strong electrolytes
form solutions that conduct an electric current strong enough to light a bulb.
Strong electrolytes
dissociates only slightly in water.
Weak electrolyte
forms a solution with a few ions and mostly undissociated molecules
Weak electrolyte
- dissolve as molecules in water.
- do not produce ions in water.
- do not conduct an
electric current
Nonelectrolytes
Examples of Strong electrolyte
Ionic compounds such as;
- NaCl, KBr, MgCl2, Nano3-
Bases such as:
- NaOh, KOH
Acids such as:
- HCl, HBr, HI, HNO3, HClO4 H2SO4
Examples of Weak electrolyte
HF, H2O, NH3, acetic acid
Examples of Nonelectrolytes
Carbon compounds such as Methanol, Ethanol, Sucrose, Urea
NaCl
Strong electrolyte
KBr
Strong electrolyte
MgCl2
Strong electrolyte
NaNO3
Strong electrolyte
NaOH
Strong electrolyte
KOH
Strong electrolyte
HCl
Strong electrolyte
HBr
Strong electrolyte
HI
Strong electrolyte
HNO3
Strong electrolyte
HClO4
Strong electrolyte
H2SO4
Strong electrolyte
HF
Weak Electrolyte
H2O
Weak Electrolyte
NH3
Weak Electrolyte
HC2H3O2(Acetic acid)
Weak Electrolyte
CH3OH (methanol
Nonelectrolyte
C2H5OH(ethanol)
Nonelectrolyte
C12H22O11(Sucrose)
Nonelectrolyte
CH4N2O (urea)
Nonelectrolyte
Types of particles in solution: Strong electrolyte
Ions Only
Types of Particles in solution: weak electrolyte
Mostly molecules and a few ideas
Types of particles in Solution: nonelectrolyte
Molecules Only
is the amount of an electrolyte or an ion that provides 1 mole of electrical charge (+ or −)
Equivalent (Eq)
1Eq = ?
1000 mEq
- contain less than the maximum amount of solute.
- can dissolve more solute.
Unsaturated solutions
- contain the maximum amount of solute that can dissolve.
- have undissolved solute at the bottom of the container.
Saturated Solutions
Effect of temperature on solubility
- Solubility of solids increase as temperature increase
- Solubility of gases decreases as temperature increase
states that
* the solubility of a gas in a liquid is directly related to the pressure of that gas above the liquid.
* at higher pressures, more gas molecules dissolve in the liquid.
Henry’s Law
Henry’s Law:
* the solubility of a gas in a liquid is directly ____ to the ____ of that gas above the ____.
- related
- pressure
- liquid
Henry’s Law:
- at ____ ____, more gas molecules dissolve in the _____.
- higher pressures
- liquid
Soluble ionic compounds
Sulfates, (SO4^2-) are soluble unless combines with
- Ba2+,
- Pb2+,
- Ca2+,
- Sr2+,
- Hg2^2+
an insoluble ionic compound, is used to enhance X-rays
Barium Sulfate (BaSO4)
an insoluble solid that emerges from a liquid solution
precipitate
- Water is added
- the volume of the solution increases
- concentration decreases
Dilution
Formula for concentrations and volumes are related
C1V1=C2V2
- When water is added to the concentrated solution, there is no change in number of particles.
- The solute particles spread as the volume of the solution increases
Dilution of a Solution
