solutions and their behavior ch 8

Question 1

what is a Solution

Answer 1

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

Air is a solution of nitrogen, oxygen, and a few other minor gases.

Question 2

what is a Solvent

Answer 2

Solvent is present in the larger amount.

Question 3

Solute what is it

Answer 3

Solute is present in smaller amount than the solvent.

Question 4

example of a solvent and solute

Answer 4

Normal saline is a solution containing sodium chloride and water. The sodium chloride comprises 0.89% of the mixture and water comprises 99.11% of the mixture, NaCl is the solute and water is the solvent.

Question 5

Molality (m) what is it

Answer 5

, or molal concentration expresses concentration in terms of moles of solute per kilogram of solvent.

m= moles solute/ kg solvent

Question 6

Molarity, what is it

Answer 6

or molar concentration is defined as moles of solute per liter of solution.

Molality is never equal to molarity.

The difference becomes smaller as solutions become more dilute.

M= moles solute/ L solution

Question 7

percent means part per what

Answer 7

100

Question 8

unit of concentration formula or percent by weight to volume

Answer 8

% = g of solute/ 1000 ml of solution

Example: Drug is packaged 5mg/5ml. You want to give 10mg. How many ml will you give?= 10 ml

Question 9

the percent by weight formula =

Answer 9

% (w/w)= 25 g of glucose/ 500g of solution x 100 = 5%

Question 10

Solubility is what

Answer 10

Solubility is the amount of solute that will dissolve in a given amount of solvent

Question 11

Saturated is what

Answer 11

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

Question 12

Supersaturated means

Answer 12

This is not a stable system
A solution contains more solute than allowed by the solubility.

can turn vaporizer to high concentration for a short period to drive in more gas.

Question 13

Supersaturated example

Answer 13

The excess solute will come out of solution crystallizing as a solid, separating as a liquid, or bubbling out as a gas.
For example, when blood or urine in the kidneys becomes supersaturated with calcium oxalate or calcium phosphate, a kidney stone can form.
If the solute is a gas in liquid solvent, you would see bubbles forming in the solution. Perhaps you’ve seen this phenomenon when you open a bottle of beer or soda pop.

Question 14

Two liquids are blank if they are soluble in each other in all proportions.

Answer 14

Miscible

Question 15

Miscible

example

Answer 15

Two liquids are miscible if they are soluble in each other in all proportions. Alcohol and water are miscible with each other. Oil and water, on the other hand, are immiscible with each other.

Question 16

Solubility Guidelines

Answer 16

Like dissolves like
Polar solutes are more soluble in polar solvents
Nonpolar solutes are more soluble in nonpolar solvents

you dont want your gases to be absorbing into the blood because it would take a long time for pt to wake up. our gases are quick active now.

Question 17

The solubility of a solute is the amount of what

Answer 17

the solute that will dissolve in a given amount of solvent at a given temperature.

Question 18

Solubility Guidelines example

Answer 18

That means that polar solutes are more soluble in polar solvents, while nonpolar solutes are more soluble in nonpolar solvents. You can consider most organic compounds to be nonpolar.

The most polar species are, obviously, ionic compounds, followed by species that can form hydrogen bonds, such as water and ethanol (CH3CH2OH). Therefore, you would expect ionic compounds to be soluble in water, but not very soluble in an organic solvent such as ether or hexane.

!!!!On the other hand, you would expect an organic compound, like the vast majority of the pure form of injectable medications, to be relatively insoluble in a water-based medium such as blood.!!!!!

Question 19

Solubility Example: Lidocaine

Answer 19

Lidocaine is not very soluble in water. Lidocaine belongs to the class of organic compounds called amines, and amine functional groups contain a nitrogen atom.

Lidocaine (a nonpolar, water-insoluble organic compound) reacts with hydrochloric acid to give an ionic salt, which is called lidocaine hydrochloride (the drug). Because lidocaine hydrochloride has an ionic bond, it is readily soluble in water.
can change the compounds of drugs to make them more useful.

Question 20

Energy Changes of Solution Process

Answer 20

Energy flows into the system during an endothermic process, whereas energy flows out of the system during an exothermic process.
Some substances have positive (endothermic)

transfer of heat goes from hot to cold.

Question 21

Heat is the transfer of energy into or out of a system caused by a difference in temperature. T/F

Answer 21

true

Question 22

Solvation process:

Answer 22

Chemical bonds require lattice energy to bind together. The energy (heat) required to break or solvate those bonds is the solvation process.

Question 23

Solvation process example

Answer 23

Whether or not the heat of solution is an endothermic or an exothermic process depends on the relative magnitudes of the lattice energy and the heat of solvation. If tearing the ions apart requires more energy than is released by solvation, then ΔHsolnis going to be positive (endothermic). If the energy released by solvation is greater than the energy required to tear the ions apart, ΔHsolnis going to be ex

Question 24

Effect of Pressure on Solubility

Answer 24

Gaseous solute
As P increases, solubility increases
Henry’s Law
Sgas = kHPgas
S = solubility, k = constant, P = partial pressure

Liquid and solid solutes
P has negligible effect

Question 25

Pressure has a dramatic effect on the solubility of gaseous solutes in liquid solvents

Answer 25

As pressure increases, the solubility of a gaseous solute in a liquid solvent increases.

Question 26

Effect of Pressure on Solubility example

Answer 26

Carbonated beverage: Have you noticed that when you open a bottle of champagne (or soda pop, or beer, or club soda), small bubbles of carbon dioxide gas start to form? That “pop” you hear when removing the cork is caused by the escape of excess carbon dioxide gas from the bottle.
When the gas escapes, the pressure in the container decreases. With less pressure, the solubility of the carbon dioxide dissolved in the champagne decreases.

Question 27

Since solids and liquids are not very compressible, at least not compared to gases, pressure has what affect

Answer 27

has very little effect on the solubility of solid and liquid solutes.

Question 28

Henrys Law

Answer 28

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

Question 29

henry law example

Answer 29

If we increase the partial pressure of a gas, that means there are more of those gaseous molecules (in a given volume, at a given temperature) zipping around near the surface of the liquid. Doesn’t it make sense that more of the gas molecules will be trapped by the liquid solution? Also, if the dissolved gas molecules were to escape into the gas phase, the pressure would increase. So, assuming that the pressure remains constant, the would-be escapees are crushed back into solution.

Question 30

Effect of Temperature on Solubility

Answer 30

Gaseous solute
As T increases, solubility decreases
Think about opening a warm can of soda pop …the carbon dioxide is less soluble and comes bubbling out.

Question 31

Liquid and solid solutes As Temperature increases,

Answer 31

solubility generally increases.

Question 32

example important !!!! henry law

Answer 32

Important Concept: Temperature effects solubility, therefore a patient who is cold receiving an anesthetic gas, solubility INCREASES, and their emergence (wakeup) will be longer. Important on many levels to keep patients normothermic in the OR

Question 33

Temperature Effect

Answer 33

The amount of gas dissolved is inversely proportional to the temperature. (the colder the liquid (blood), the more gas that will dissolve in the liquid).

Cold patients take longer to wake up if using an inhalational agent.

Question 34

As solutes are added to a solution what happens

Answer 34

the physical properties of the solution change.

Question 35

Colligative Properties of Solutions

Answer 35

A colligative property depends only on the number of solute particles, not the identity of the solute particles

Question 36

Colligative properties include

Answer 36

Colligative properties include:

1. The vapor pressure of a solution decreases with increasing solute concentration.
2. The boiling point of a solution increases with increasing solute concentration.
3. The freezing point of a solution decreases with increasing solute concentration.
4. The osmotic pressure of a solution increases with increasing solute concentration.

Question 37

Vapor Pressure

Answer 37

Vapor pressure of liquid results from the most energetic molecules near the surface of the liquid escaping into the gas phase.

amount of molecules that escape after heating something.

Question 38

Raoult’s Law

Answer 38

The vapor pressure of a solution

Raoult’s law states the vapor pressure of a volatile component of a solution (P) is equal to the vapor pressure of the pure substance (P°) times the mole fraction (χ) of that substance.

Question 39

Boiling Point Elevation

Answer 39

The temperature at which the vapor pressure of the material is equal to the ambient pressure.
ex. Adding salt to the water to cook pasta, slightly increases the boiling point.

Question 40

Boiling Point Elevation info

Answer 40

the vapor pressure of a solution is decreased by the addition of nonvolatile solutes, a higher temperature is needed to drive the vapor pressure up to the point where it equals the ambient pressure.
the boiling point of a solution increasesas the concentration of solute(s) increases. The change in boiling point is directly proportional to the molal concentration of the solute particles.

Question 41

Freezing Point Depression

Answer 41

the temperature at which the liquid phase of the material is in equilibrium with the solid phase.

necessary to cool the sample to lower temperatures, thereby lowering the kinetic energy of the molecules even further, before they will settle into the solid phase.

Question 42

Osmotic Pressure

Answer 42

The one with the greater concentration is the hypertonic solution, and the one with the lower concentration is the hypotonic solution.

Question 43

The relative concentration of solutes in osmotic systems is called the

Answer 43

tonicity.

Question 44

Isotonic

Answer 44

if they contain equal concentrations of particles.

Question 45

Osmosis is

Answer 45

the diffusion of water, and diffusion always spontaneously occurs in the direction from an area of high concentration to an area of low concentration.

Question 46

osmosis example

Answer 46

Since the concentration of water in the hypotonic solution is greater than the concentration of water in the hypertonic solution, osmosis always spontaneously occurs from the hypotonic solution to the hypertonic solution.

Question 47

Entropy

Answer 47

demands that osmosis occur between two solutions of unequal tonicity until the concentrations of the two solutions are equal.

Question 48

are colloids true solutions?

Answer 48

Colloids are not true solutions,

The pulling power of proteins!

Question 49

colloid particle size?

Answer 49

Particle size is on the order of 200 nm
Might be super-sized molecules (e.g., proteins) or aggregates of ions
Colloidal particles cannot be filtered and do not settle out of solution.
Examples:
Blood, milk, jelly. Albumin