UNIT 2 Flashcards
1
Q
Ionization
A
Breakdown of electrolyte molecules into small constituent ions.
2
Q
Example Ionization:
A
NaCl –> Na+ + Cl-
3
Q
Electrolytes
A
Molecules split or dissociate into electrically charged atoms (ions). Carries an electrical current when in solution. Compounds in body are weak electrolytes.
Example: Na, K, Cl, CO2.
4
Q
Ions
A
Atom or group of atoms that carry electrical charge. Gain or loss of electrons.
5
Q
Cation
A
Ion with positive charge. Example: Na+ and K+.
6
Q
Anion
A
Ion with negative charge. Example Cl-.
7
Q
Anode
A
negative charge
8
Q
Cathode
A
positive charge.
9
Q
Acid
A
Hydrogen ion donor.
10
Q
Strong Acids
A
Give off high concentration of H+ in H2O.
Examples: HCl, H2SO4.
11
Q
Weak Acids
A
Give off low concentration of H+ in H2O.
Examples: H2CO3, CH3COOH.
12
Q
Base
A
Hydrogen ion acceptor. hydroxyl ion donor.
13
Q
Salt
A
metal or ammonium ion electrovalently joined to anion other than hydroxyl. To produce a salt an acid reacts with a base.
14
Q
Example of a salt producing:
A
HCl + NaOH —> NaCl + H2O.
15
Q
Normal Salt
A
Complete replacement of H+.
Example: NaCl.
16
Q
Acid Salt
A
Partial replacement of H+.
Example: NaHCO3.
17
Q
Alkaline salt
A
Partial replacement of OH-.
18
Q
Weak Electrolyte Characteristics
A
Small portion of molecules dissociate, remainder do not.
Equilibrium maintained between molecules and ions
Product of molar concentration of ions divided by molar concentration of undissociated molecules is a constant value (Dissocation Constant K).
19
Q
Dissociation of K Example: Formula
H2CO3 –> H+ + HCO3-
A
K= [H+] x [HCO3-]/[H2CO3]
20
Q
Information needed to calculate K
A
Concentration of solution (M)
Amount of dissociation (%)
21
Q
Dissociation of K of H2O
A
K= [H+] x [OH-]/[H2O]
22
Q
[H+]= 3.0 x 10-8 M/L
Acid or Base?
A
Base
23
Q
[H+] greater than H2O (1.0 x 10-7) solution is….
A
acidic
24
Q
[H+] less than H2O (1.0 x 10-7) solution is…
A
basic.
25
[H+] =1.0 x 10-6 M/L is...
Acidic
26
[H+]= 4.0 x 10-7 solution is...
Acidic
27
Nanomole
one billionth of a mole. (10-9)
28
pH
logarithm of reciprocal of molar hydrogen ion concentration.
pH=log101/[H+]
pH=-log[H+]
29
pH and [H+] are inversely related
H+ ion goes up, the pH goes down. (vice versa).
30
Water is...
neutral
31
pH scale range is..
0-14
32
pH less than 7 is..
acidic
33
pH greater than 7 is...
basic
34
Diffusion
Process by which solute (gas/solid) in solution moves. Molecules or ions diffuse from an area of higher concentration to lower.
35
When will diffusion occur?
It will occur across a membrane if membrane is permeable to substance. Move without restriction.
36
Osmosis
Movement of solvent (H2O) through semipermeable membrane. Moves to area where there is a higher concentration that cannot pass through membrane.
37
H2O moves from an area where ther is ____ amount of H2O in relation to solute to an area where there is ___ H2O in relation to solute.
greater, less
38
Osmotic Pressure
More concentrated solution on one side of semipermeable membrane and less concentrated solution on other side. A force that pulls water through membrane to the more concentrated side. (Side with more solute).
39
Tonicity
Relative degree of osmotic pressure exerted by a solution.
40
Three levels of tonicity
Isotonic, hypotonic, and hypertonic.
41
Isotonic
solutions on both sides of a semipermeable membrane have established equilibrium. Same osmotic pressure. No net movement.
42
How much % NaCl are body cells?
0.9% NaCl (Isotonic Saline or Normal Saline).
43
How much glucose in body cells?
5% glucose.
44
Hypotonic
When solution contains lower concentration of solute (lower osmotic pressure) than the other. Less solute, more H2O than isotonic solution.
45
Hypertonic
When solution contains higher concentration of solute (higher osmotic pressure) than the other. Solution has more solute, less h2O than isotonic solution.
46
Active Transport
Moves molecules or ions "uphill" against concentration and osmotic pressure. Solute would from area of lower to higher concentration. (kidneys blood brain barrier).
47
Hydrostatic pressure
Force of fluid pressing outward against walls if vessels. (filtration).
48
Filtration
H2O and diffusable solutes move from solution with higher hydrostatic pressure to solution with lower hydrostatic pressure.
49
Intracellular Fluid Compartment
Most fluids are inside cells. Cells differ in chemical composition, but similar in concentration. Fluid of all cells considered a compartment.
50
Extracellular Fluid Compartment
Fluid outside of cells. Has subdivisions.
51
Subdivision of Extracellular Compartment.
Fluid within vessels (Intravascular IV)
Fluid between cells (Interstitial IS).
Outside of cell, outside of blood vessels.
52
___ % body's total weight is fluid
60%
53
Intracellular compartment %
40%
54
Extracellular compartment %
20%
Intravascular (5%)
Interstitial (15%)
55
Sources of Fluid Gain
Oral liquids, water in foods, water of oxidation.
56
Approx. amount of mL/day of Oral liquids
1500 mL/day
57
Approx amount of mL/day from water in foods
700 mL/day
58
Approx. amount of mL/day from oxidation of water
200 mL/day
59
Sources of Fluid Loss
Urine, diffusion, evaporation, feces, and perspiration.
60
Amount of mL of urine for fluid loss
1400 mL/day
61
Amount of mL of diffusion for fluid loss
350 mL/day
62
Amount of mL of evaporation for fluid loss
350 mL/day
63
Amount of mL of feces for fluid loss
200 mL/day
64
Amount of mL of perspiration for fluid loss
100 mL/day
65
What insensible water loss occurs that we are not aware of?
Loss through skin and lungs.
66
Role of kidneys
fluid balance, electrolyte balance, and production of urine.
67
Possible types of Imbalance
Fluid volume, fluid concentration, and fluid composition.
68
Hydrostatic pressure
force of fluid molecules pressing outward against blood vessel wall. Higher to lower hydrostatic pressure.
69
Osmotic Pressure
force pulling water to the solution with a greater concentration of solute. Water moves to solution with higher pressure.
70
Oncotic Pressure
moves to the solution.
71
Fluid compartments
contain both water and solutes.
| Each has measureable hydrostatic and oncotic pressure.
72
Starlings Law
Balance between processes of filtration and osmosis in lungs.
73
Starlings Law Lung Values
Hydrostatic pressure in capillaries: 10 mmHg
Oncotic Pressure in capillaries: 25 mmHg
Hydrostatic Pressure in interstitium: -1mmHg
Oncotic Pressure in interstitium: -1 mmHg
74
Starlings Law states filtration will only occur if...
The hydrostatic pressure in capillaries would have to be greater than 25 for filtration to occur.
75
Conclusion of Starling's Law
filtration does not occur in the lungs. Interstitial pressure and oncotic pressure are small. There is very little water and solute in the IS. IS in Starlings law add up to 0.
76
Fluid compartment with most protein?
Intracellular Fluid Compartment
77
Chief cation IC?
Pottasium
78
Chief anion IS and IV?
Chlorine, hooks up with Na important for fluid movement.
79
Equivalent Weights
weights of reacting substances having equal chemical power.
| A reacts with B.
80
Gram equivalent weight
substances quantitative reacting unit. Gram mass that contains, replaces, or reacts with the Avogadros number of hydrogen atoms.
81
Element/Radical
weight in grams that can combine with or replaced in a chemical reaction, 1 gram atomic weight of hydrogen or other monovalent element.
82
Rule of element/radical
gram atomic weight divided by valence.
83
Acid
weight in grams of acid that contains 1 gram atomic weight of replaceable hydrogen.
84
General rule for acids
gram atomic weight divided by number of hydrogen's in formula. Two exceptions: carbonic acid and phosphuric acid.
85
Base
weight in grams that base that contains 1 gram formula weight of replaceable hydroxyl radical.
86
General rule for bases
gram atomic weight divided by number of OH groups in formula.
87
Solution
mixture of two substances with one so evenly dispersed throughout the other, that mixture is homogeneous.
88
Solute
liquid or gas.
89
Solvent
always liquid, usually h2O.
90
Factors affecting solubility
nature of solute, nature of solvent, temperature, and pressure.
91
Dilute
relatively small amount of solute: solvent.
92
Concentrated
relatively large amount of solute/solvent.
93
Saturated
will see the solute at the bottom, max amount of solute in volume of solvent.
94
Supersaturated
holds more solute than saturated. ex: SSKI.
95
Ratio solution (true)
relationship between solute and solvent expressed as whole number ratio. made by mixing components in proportion specified in ratio. liquid solute/liquid solvent. no units.
96
Percent solution (true)
Describes weight of solute to weight of total solution as %. solid or liquid solute/solvent always liquid.
97
Weight per unit volume solution
Describes solution where weight of solute and volume of solution are used. Expressed as a percent. Not a true % solution. Most drug solutions.
98
Molar solution
Describes solution as number of moles of solute per number of liters of solution
99
Molal Solution
Describes solution as number of moles of solute per number of kg of solution.
100
Normal Solution
Describes solution as number of gram equivalents of solute per number of liters of solution.
101
3 variables regarding solutions
amount of solute, amount of solution, classification of solution.
102
Dilution of solutions
diluting a solution increases its volume without changing amount of solute. Concentration is reduced. Initial amount of solute must be equal to the final amount of solute.
