Tags & Description
Solutions (basic)
Homogenous mixtures
Have two components
What are the solvent and solute distributions in solutions?
Solute: present in smaller amounts
Solvent: present in larger amounts
How do solutions form?
When there is sufficient attraction between solute and solvent molecules
When solute-solvent interactions are large enough to overcome solute-solute and solvent-solvent interactions
What states of matter can solvents and solutes be in?
Both: gas, liquid, or solid
What happens to the solute when mixed with a solvent (state change)
Mixes with the solvent so that the solute and solvent have the same physical state
Solutes
Mixed into the solvent
Spread evenly throughout the solution
Cannot be separated by filtration, but can be separated through evaporation
Are not visible, but can give the solution a color
Water as a solvent
One of the most common solvents in nature
Why is water a polar molecule?
Due to the polar O-H bonds
Hydrogen bonds
What is the rule about the dissolving of solutes in a solvent?
“Like dissolves like“
Both must be polar or nonpolar
Water w/ polar solutes
Why?
Polar molecules such as CH₃OH are soluble in water due to the -OH group to form hydrogen bonds with water
Water w/ nonpolar solvents
Iodine, grease, oil and other nonpolar molecules are not soluble in water because there are no attractions between the two.
Electrolytes (in the body)
They play an important role in maintaining the proper function of the cells and organs
Can be measured in a blood test
What does it mean to “dissociate“
Fall apart into ions
Strong Electrolytes
Dissociate 100% in water, producing positive and negative ions
Form solutions that can conduct an electric current strong enough to light a lightbulb
Weak Electrolytes
Dissociate only slightly in water
Forms a solution with a few ions and mostly undissociated molecules
Mildly conducts electricity
Nonelectrolytes
Dissolve as molecules in water
Do not produce ions in water
Do not conduct an electric current
Do polyatomic break down?
Nope
What are some examples of strong, weak, and non- electrolytes?
SE: Ionics, strong bases (have OH), strong acids, salts
WE: Weak acids (usually begin with H except for ammonia)
NE: Carbon compounds
What are the types of particles in a solution with strong, weak, and non-electrolytes?
SE: Only ions
WE: Mostly molecules a few ions
NE: Only molecules
Equivalents of Electrolytes
The amount of an electrolyte or an ion that provides one mole of electrical charge (+ or -)
Equivalents of Electrolytes (in solution…)
The charge is always balanced by the charge of the negative ions
How are the concentration of electrolytes in intravenous fluids expressed?
Milliequivalents per liter (mEq/L)
1 Eq = 1000 mEq
If you have 2.2 mol of NaCl solution, then how many mole equivalents of each ion do you have?
Na⁺ = 2.2 Eq Na⁺
Cl⁻ = 2.2 Eq Cl⁻
If there are 25 mEq/L of Na⁺ and 4 mEq/L of K⁺ what is the total positive charge, and what concentration of Cl⁻ would make sense?
Total positive charge: 29 mEq/L
Cl⁻ = as the only anion has to be 29 mEq/L
Concentration: 8.8 mEq/L
How many moles of calcium ions in 0.50L
Calcium ions = 2+
0.5 L (8.8 mEq Ca²⁺/1 L)(1 Eq Ca²⁺/1000 mEq Ca²⁺)(1 mole Ca²⁺/2 Eq Ca²⁺) = 0.0022 moles of Ca²⁺
Solubility
The maximum amount of solute that dissolves in a specific amount of solvent
Temperature sensitive for solutes
How is solubility expressed?
As grams of solute in 100g of solvent (usually water)
g of solute/100g water
Unsaturated Solutions
What do they look like?
Contain less than the max amount of solute
Can dissolve more solute
Is clear
Saturated Solutions
Contain the max amount of solute that can dissolve
Have undissolved solute at the bottom of the container
What happens in saturated solution? (equilibrium process)
Some solute dissolves and some recrystallize
solute dissolves
solute + solvent ⇌ saturated solution
solute recrystallizes
What happens to the solubility when the temperature increases?
Most solids
Gasses
Solids = Increases (direct relationship)
Gasses = Decreases (inverse relationship)
Henry’s Law
The solubility of a gas is directly related to the pressure of the gas above the liquid
At higher pressures, more gas molecules dissolve in the liquid
Gas is pushed into the liquid
When the pressure of a gas above a solution decreases, the solubility of the gas in the solution also decreases
What types of ionic compounds are soluble in water?
Ionic compounds that contain a soluble cation or anion
What happens if an ionic compound with no soluble cations or anions is placed in water?
Why?
It will form a solid
The ionic bonds are too strong for the polar water molecules to break
What can we use the solubility rules to predict?
Whether an ionic compound will dissolve in water or not
What are the solubility rules?
What DOES dissolve in water:
Positive Ions = Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺, NH₄⁺
Negative Ions = No₃⁻, C₂H₃O₂
Cl⁻, Br⁻, and I⁻ except when bonded with Ag⁺, Pb²⁺, or Hg₂²⁺
SO₄²⁻ except when bonded with Ba²⁺, Pb²⁺, Ca²⁺, Sr²⁺, or Hg₂²⁺
What are the three types of equations?
Complete Molecular Equation:
What we’re used to
Total Ionic Equations
Uses subscripts and charges
Net Ionic Equations
Cancels out repetitive parts
How do you write a net ionic equation?
First, form the complete molecular equation, balancing and all
Next, form the total ionic equation by separating the aqueous solutions into their ions = by using the subscripts as coefficients and writing in the charges
Do not split polyatomic or solids or liquids or gasses
Lastly, cancel out any of the same ions from either side of the equation
How do you calculate the concentration of a solution? What are the units for each part?
Amount of solute/Amount of solution
Solute = grams, milliters, or moles
Solution = grams, milliters, or liters
Mass Percent (m/m) Formula
mass of solute g/mass of solute g + mass of solvent g(mass of solution g) x 100%
Volume Percent (v/v) Formula
volume of solute mL/volume of solution mL x 100%
Mass/Volume Percent (m/v) Formula
mass of solute g/volume of solution mL x 100%
What does the “x 100%“ mean in the m/m, v/v, and m/v formulas?
It means that, technically, the g of solute is over 100g of solution
ex. 5% (m/m) = 5g solute/100g solution
What is the conversion factor displayed by 8.50% (m/m) NaOH
8.50g NaOH/100g 8.50% (m/m) NaOH Solution
Yes lots of words :<
Molarity
The moles of solute per volume(L) of solution
Very specific; only in unites of moles and liters
What is the formula for molarity
Moles of solute/Liter of solution
What conversion factor is represented by 1.00M of NaCl?
1.00 moles NaCl/1 L NaCl solution
What is the molarity of a solution of 6.00g of NaOH in 500mL of solution?
First, we need to make grams into moles
6.00g (1 mol NaOh/40.00g NaCl) = 0.150 mole NaOH
Now, we need to make the 500mL solution into liters, which would be 0.500 L
Lastly use the molarity formula (mole/L)
0.150 mol NaOh/0.500L NaOH solution = 0.300M NaOH
What does a capital M mean?
Molar/Molarity
Dilution
A solvent, usually water, is added to a solution which increases it’s volume and decreases the concentration of the solution
True or False: In dilution, the mass of the solute stays the same
True
In the initial and diluted solutions, what formula relates their concentration?
C₁V₁ = C₂V₂
What is C in C₁V₁ = C₂V₂
Percent concentration(m/m, v/v, m/v) or molarity
What other formula has basically the same use as C₁V₁ = C₂V₂
M₁V₁ = M₂V₂
Solutions (described)
Transparent
Do not separate
Contain small particles, ions, or molecules that cannot be filtered nor can they pass through the semi-permeable membrane
Homogenous
Particles do not settle
Colloids
Medium-sized particles
Cannot be filtered
Can be separated by semipermeable membranes
Homogenous
Particles do not settle
Suspensions
Heterogeneous, nonuniform mixtures
Have very large particles that settle (rapidly)
Can be filtered
Must be stirred to stay suspended
What is the Tyndal Effect and what type of mixture is it?
When particles are large enough and light shines through, it gets scattered
Colloids
What are the two separation methods, and how large are the pores in each?
Filter Paper: 10⁻⁷m (larger)
Semipermeable Membrane: 10⁻¹⁰m (smaller)
Which mixture particles can pass through a semipermeable membrane?
Solution particles
Not colloids or suspensions
Which mixture particles settle out and can be separated by a filter?
Suspensions
When does a liquid boil?
When it’s vapor pressure matches the external atmospheric pressure
When a solute is added to water, what physical properties change?
What are these properties called and what do they depend on?
Vapor pressure above solution decreases
Boiling point increases
Freezing point decreases
They are called colligative properties and depend only on the concentration of solute particles in the solution
Vapor Pressure Lowering (added solute)
Increasing the concentration of solute particles in the solution
Decreases the # of solvent particles at the surface of the solution
Prevents some of the solvent particles from leaving the solute
The solute takes up space at the top so the water cannot become vapor
Boiling Point Elevation (added solute)
Increasing the concentration of nonvolatile particles in the solution raises the boiling point of the solution
More solute in solution decreases the vapor pressure
Solution boils at a higher temperature than normal
More energy is needed to make water into vapor
Freezing Point Lowering (added solute)
Adding salt to an icy road(for example) when temperatures drop below freezing…
Allows salt particles to mix with water
Lowers the freezing point of the ice
What types of particles can lower the freezing point of water?
Strong electrolytes
The stronger the electrolyte, the lower the freezing point
Osmosis
An ongoing process where water flows from a lower to a higher solute concentration through the membrane
The level of the solution with the higher solute concentration rises
The concentrations of the two solutions become equal over time
Osmotic Pressure
Equal to the pressure that would prevent the flow of additional water into the more concentrated solution
Greater as the # of dissolved particles in the solution increases
Isotonic Solutions
Exert the same pressure as body fluids such as red blood cells (RBCs)
Most IV solutions used in hospitals are isotonic solutions
What are the m/v% (RBCs) that classify as an isotonic solution?
5.0% (m/v) glucose
0.90% (m/v) NaCl
Hypotonic Solutions
Have a lower solute concentration than red blood cells
Water flows INTO the cells by osmosis
The fluid increase causes the cells to swell and burst = hemolysis
Hypertonic Solutions
Have a higher solute concentration than red blood cells
Water flows OUT OF the cells by osmosis
The cells shrink, look spiky: crenation
Dialysis
A process used to remove waste products and excess water from the blood
How does dialysis work?
Solvent and small solute particles pass through an artificial membrane
Large particles are retained inside
What is hemodialysis
Part of Dialysis
Waste particles such as urea from the blood are removed using an artificial kidney