Solutions and their Behavior

Question 1

What is a solution?

Answer 1

Homogeneous mixture that consists of one or more solutes uniformly dispersed at the molecular or ionic level throughout a medium known as the solvent.

Question 2

How are solvents and solutes present?

Answer 2

• Solvent is present in a large amount
• Solute is pressent in a smaller amount that a solvent
• • Propofol separates out if left for
• *Succinylcholine needs to stay in the fridge
• *Manitol will crystalize

Question 3

Molality (m) =?

Answer 3

m= moles solute
——————-
kg solvent

Question 4

Molarity (M) =?

Answer 4

M= moles solute
———————–
L solution

Question 5

T/F: Molality is never equal to molarity ?

Answer 5

TRUE

-The difference becomes smaller as the solutions become more dilute

Question 6

When is Molality more useful?

Answer 6

When dealing with physical chemistry

Question 7

When is Molarity more useful?

Answer 7

Dealing with solution stoichiometry

Question 8

Mole fraction %?

Answer 8

x1 = moles 1/ moles 1 +moles 2 + moles n

Question 9

Weight percent?

Answer 9

%w/w = grams solute
—————————-
100g solution or

grams solute
—————— x 100%
g solution

Question 10

Define Solubility

Answer 10

The amount of a solute that will dissolve in a given amount of a solvent

**How much CO2 will dissolve in blood?

Question 11

Define Saturated

Answer 11

A saturated solution contains the maximum amount of a solute, defined by its solubility

**Gas, inspiring a percent and exhaling a percent, obese pre oxygenate, want to SATURATE them well with oxygen
Look at their ins/exp O2 concentration ratio

Question 12

Supersaturated

Answer 12

A solution contains more solute than allow by the solubility

Question 13

What is Miscible?

Answer 13

Two liquids are miscible is they are soluble in each other in all proportions

Question 14

Solubility guidelines

“ like dissolves like” means what?

Answer 14

• Polar solutes are more soluble in polar solvents

- Nonpolar solutes are more soluble in non polar solvents

Question 15

T/F: Heat of a solution is the enthalpy change that accompanies dissolution of 1 mole of a substance?

Answer 15

True
-Some substances have positive H ( endothermic)
-Negative are (exothermic)
Slide 9

Question 16

Lattice energy ( LE) is the energy released when a molecule or ions settle into a crystalline lattice- this process is inherently what?

Answer 16

Exothermic

Question 17

T/F: Solvation (hydration) energy (SE) is the energy released when an ion ( or molecules ) settles into a sphere of solvent molecules- this process is inherently endothermic?

Answer 17

False-

It also is exothermic.

Question 18

What do both Lattice Energy and Salvation energy result from?

Answer 18

IM forces

Intermolecular Forces

Question 19

What does Henry’s law say about gaseous solutes and their pressure and solubility?

Answer 19

-As pressure increase, solubility increases (solubility of a gaseous solute in a liquid solvent increase)
Sgas= (k) (Pgas)
S=solubility 
k= constant
P=partial pressure 

**ex:carbonated beverage
“pop” you hear is the except of the excess carbon dioxide in the bottle

Question 20

What does Henry’s law say about liquid and solid solutes?

Answer 20

=P ( partial pressure) has negligible effect

Question 21

What is Henry’s Law?

Answer 21

The amount of non reacting gas which dissolves in liquid is directly proportional to the partial pressure of the gas, provided the temperature remains constant

Question 22

In a gaseous solute, as temperature increases solubility does what?

Answer 22

DECREASES

• *Opening a WARM can of pop the CO2 is less soluble, and it comes bubbling out
• *Hyperthermic patient , decrease solubility of gasses in blood

Question 23

What happens to liquid and solid solutes with an increase in temperature?

Answer 23

As temperature increases, solubility generally increases

**

Question 24

T/F: The temperature effect is: the amount of gas dissolved is directly proportional nil to the temperature?

Answer 24

False
INVERSELY proportional to temperature
( the colder the liquid, the more gas that will dissolve in the the liquid)
**This is for inhaled gasses

Question 25

Generally, the solubility of a solid and liquid solutes in liquid solvents increase with increasing temperature. Give an example this rule?

Answer 25

A concentrated mannitol solution will crystallize if stored at low temperatures , warming the solution will cause the solid to redissolve.

Question 26

What does a colligative property depend on?

Answer 26

Depends only on the Number of solute particles, not the identity of the solute particles

Question 27

What four things to colligative properties include?

Answer 27

1-Vapor pressure decreasing
2-Boiling point elevation
3- Freezing point depression
4-Osmotic pressure increase

Question 28

That vapor pressure of a solution is given by what law?

Answer 28

Raoult’s

**Said we don’t need to know this

Question 29

Boiling point elevation:

As vapor pressure goes down what happens to the boiling point?

Answer 29

Boiling point goes up

Delta T bp= (Kbp) (msolute)
Delta Tbp= boiling point elevation
kbp: is the boiling point 
(ebullioscopic )constant
solute: molality of all solute particles

Question 30

What is an example of boiling point elevation?

Answer 30

When you add salt to water, it increases the temperature needed to boil water by 0.18 degree Celsius? Therefor, elevating the boiling point.

Question 31

What happens in freezing point depression?

Answer 31

The relationship that quantifies the degrees of freezing point depression has an identical form to boiling point elevation

Question 32

What is an example of freezing point depression?

Answer 32

-Adding salt to ice cream, lowers the freezing threshold and doesn’t freeze.

Question 33

Osmosis is the diffusion of water through what type of membrane?

Answer 33

Semipermeable

Question 34

Solute particles are too ___ or ( too ___) to make it across the membrane during osmosis?

Answer 34

Too big

Too polar

Question 35

Isotonic Solutions have _____concentrations of solute particles?

Answer 35

Equal

Question 36

Hypertonic solutions and hypotonic solutions have what concentrations of solute?

Answer 36

Greater and Lower

• *Regional and Spinal anesthetics ( CSF at subarachnoid level, where our blocks go) we can give in all three forms
• *Hypertonic solution : if left sitting will travel down, or lay them down will stay where you injected the block.
• *Hypotonic spinal would not be able to control cephalad distribution

Question 37

Osmotic pressure (II) results from the potential drive for the concentration of water to do what?

Answer 37

Equalize

**Capillary level, driving forces and oncotic pressures

*A 1.0 M solution of glucose exerts an osmotic pressure of 22.4 atm at 25 degrees C

Question 38

T/F: Colloids are true solutions

Answer 38

False

-They are NOT true solutions

Question 39

What is the particle size of colloids?

Answer 39

• *Order of 200nm
• -might be super-sized molecules ( e.g. proteins ) or aggregates of ions
• Colloidal particles cannot be filtered and do not settle out of a solution

Question 40

What effects do colloids exhibit?

Answer 40

The Tyndall effect
**scattering of light as a light beam gasses through a colloid.

Eg: Blood, milk, jelly