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53 Cards in this Set
- Front
- Back
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Solutions
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mixtures in which one substance is evenly distributed in another substance. Homogeneous mixtures.
Less Solute More Solvent Ex: salt water solution Solute: Salt Solvent: Water |
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Water
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the universal solvent because so many substances are soluble in it.
Properties: 1. polar 2. forms hydrogen bonds 3. stays in liquid state over wide range of temperatures. |
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The human body is made up of____________ water.
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60% - 70%. Water is the solvent of blood.
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Functions of water in the body
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1. component of all body tissues.
2. major component of blood plasma. 3. Solvent for nutrients and body wastes. 4. Provide transportation for nutrients and wastes to and from cells by way of the blood. 5. Essential for metabolism because it is necessary for the hydrolysis of nutrients in the cells. 6. lubricates joints and digestion. 7. helps regulate body temperature through presperation. |
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Dissolving ionic compounds in water
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1.dissociation- when water molecules pull the ionic compound apart.
2. hydration- each ion gets completely surrounded by water molecules. |
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Like Dissolves Like Principle
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---polar solutes are soluble in polar solvents, and nonpolar solutes are soluble in nonpolar solvents.
ex: oil and water don't mix because they have different polarities. water=polar oil=nonpolar |
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Polar
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all ionic compounds, compound that form hydrogen bonds or dipole-dipole forces.
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Nonpolar
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hydrocarbons CH and the seven diatomics
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Electrolytes
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substances that dissociate into ions when dissolved in water. conduct electricity when dissolved in water.
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Three types of electrolytes
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1. Strong electrolytes
2. Weak electrolytes 3. Nonelectrolytes |
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Strong Electrolytes
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1. Substances that dissociate completely and irrevesibly in water.
2. If 100 molecules of a strong electrolyte dissolves in water, all 100 dissociate. 3. Solutution contains: only ions and no molecules, because all the molecules have broken apart. |
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Weak Electrolyte
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1. Substances that dissociate partially and reversibly in water.
2. If 100 molecules of a weak electrolyte dissolves in water, approximately 10 dissociate. 3. Solution contains: Both ions and molecules |
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Nonelectrolytes
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1. Substances that do not dissociate in water.
2. Does not conduct electricty because they have no ions to move the electricty through the solution. 3. Solution contains: only molecules, no ions. |
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Solubility
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the amount of the solute that dissolves in the solvent at any given temperature.
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Two Types of Solutions
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Saturated and Unsaturated
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Saturated
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1. has the maximum amount of solute dissolved in it.
2. look for solute at bottom. |
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Unsaturated
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1. the solution has less than the maximum amount of solute dissolved in it.
2. look for: no solute at the bottom, everything is dissolved. |
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solid and liquid solutes
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solubility increases as temperature increases.
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gas sulutes
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solubility decreases as temperature increases.
ex: cold soda vs. room temp soda |
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insoluble salts
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a) ionic compounds that do not disolve in water / don't dissociate
b) cause: the ionic bond is too strong for water to pull apart |
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Precipitate
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an insoluble salt that forms in a solution (particles form in the solution then fall to bottom)
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Medical conditions (insoluble salts)
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kidney stones, gout-uric acid, precipitate in joints
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Molarity
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a concentration calculation ***study formula and problems***
Moles of solute _____________ Liters of solution |
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Solute-Solvent Mixture
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1. characterized according to the size of the solute particles
2. two observations a) visual inspection: look at the solution to determine if it is homgeneous or heterogenous b) strainers: can solute pass through strainers/sieves of different sizes? |
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Types of strainers/sieves
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1. filter- like paper coffee filter
2. semipermiable membrane (spm): only small molecules and ions can pass through ex: intestinal lining, cell membranes, dialyzing membrane |
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Three Types of Mixtures
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Solution, Colloids, Suspensions
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Solution
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1. homogeneous (ex: salt water, sugar water)
2. Size of solute particles: extremely small solute particles 3. solute passes through both the filter and semi-permiable membrane. |
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Colloids
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1. Homogeneous (ex. raw egg whites, mayo, blood plasma)
2. size of solute particles: small(proteins) filter but not spm 3. solute passes through filter but not through spm. |
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Suspension
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1. Heterogeneous (ex. amoxycillin, Pepto Bismol, milk of magnesia)
2. Size of solute particles: Large 3. solute does not pass through filter of spm |
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Dialysis
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1. the use of a semi-permiable membrane to seperate a colloid from a solution.
2. involves passive diffusion-does not require energy. a) requires difussion gradient- solute concentration is higher in one part of the solution than the other. b) in passive diffusion, the solute moves along the diffusion gradient, which means that it moves from where it is more concentrated to where it is less concentrated. (check 3. & 4. in notes) |
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hemodialysis
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a. blood is a complex mixture of solutions, colloid, and suspension; many of the waste products that build up in blood are solution-size solutes
solution: Na+, Cl-, urea, glucose colloids: protiens (incl. enzymes), glycogen (carb) suspension: red blood cells, white blood cells |
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Osmosis
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when two solutions are seperated by a semipermiable membrane water moves through the semipermiable membrabe into the higher concentration solution. This occurs beacause of differences in the osmotic pressure the solutions.
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Osmotic pressure
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the pressure a solution places on a membrane.
a. depends on concentration & type of solute; basically, the higher the concentration, the higher the osmotic pressure. |
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Goal in Osmosis
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to equalize the osmotic pressure on both sides of the spm. Due to the movement in water the side with the higher concentration increases in volume.
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Solutions are classified by how their osmotic pressure compare to body fluids
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Isotonic, hypotonic, hypertonic
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Isotonic
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--same osmotic pressure as body fluids
--IV solutions: .90% NaCl & 5% glucose --Red blood cells is isotonic solutions undergo no change in volume |
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Hypotonic
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--lower osmotic pressure than body fluids
--IV solutions: <.90 % NaCl & <5% glucose --hemolysis: swelling of red blood cells due to be surrounded by a hypotonic solution. |
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Hypertonic
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--higher osmotic pressure than body fluids
--IV solutions: >.90% NaCl & <5% glucose --crenation: the shiveling of a red blood cell when it is surrounded by a hypertonic solution |
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Acids
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ex: fruits, tea, soda, vinegar, battery acid
1. tastes: sour 2. texture: sticky 3. neutralize: bases 4. turn litmus paper: indicator- changes color in acid or base.... red 5. release hydrogen ions when dissolved in water. 6. known as proton donor (a proton is a hydrogen ion) 7. reacts with metals producing hydrogen gas. |
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Acids found or produced in body include:
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hydrochloric acid (stomach acid)
acetic acid carbonic acid (in blood) lactic acid |
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Bases
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ex: backing soda, ammonia, bleach, soap, milk of magnesia (MgOH2) & lye (NaOH) are metal hydroxides, which are bases that are ionic compounds.
ending in OH=base 1. taste: bitter 2. texture: slimy 3. neutralize: acids 4. turn litmus paper: blue 5. release hydroxide ions(OH-) when disolved in water. 6. know as proton exceptors, meaning that they take up hydrogen ions. Bases found of produced in the body include: Bicarbonate ion-in blood acetic ion ammonia-a waste product of protein breakdownin body |
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Neutralization reaction
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a) when acids and bases mix, they react with each other in neutralization reaction.
b) there are two products: water and salt c) called neutralization reaction because H+ and OH- are canceling each other out. d) salt is another name for ionic compound. |
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pH: Acid-Base Concetration
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the relative concentration of hydrogen ions in various body fluids is measured in
pH>7 base/alkaline pH=7 neutral pH<7 acidic |
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pH scale
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1. Divised by Danish biochemist and beer-brewer in 1909 looking for a convenient way to check acidity of his beer during the fermentation process.
2. the scale is based on the hydrogen ion concentration in a solution, where concentration is expressed in terms of moles per liter (aka molarity) 3. Scale runs from 0-14 |
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Practical info about pH
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a) the lower its pH, the more Acidic (and less Basic) a solution is.
b) the higher its pH, the less Acidic (and more Basic)a solution is. c) the more hydrogen ions in a solution, the more Acidic the solution is. d) so more hydrogen ions correspond to lower a lower pH. e) conversily, the greater the concentration of hydroxide ions in a solution, the more basic the solution is (hydroxide ions lower the hydrogen ion concentration). f) So more hydroxide ions correspond to higher pH. |
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pH scale is a logarithmic scale-
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which means that a change in pH of one is equal to ten fold change in acidity.
ex: pH 5 is 10 times more acidic than pH 6 pH 4 is 100 times more acidic than pH 6 |
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Factors that determine the acidic/basic solution
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1. Concentration ex: straight bleach vs. diluted bleach
2. strength of the acid or base (how good is the acid at donating protons, meaning dissociating completely) ****study strengths of acid bases****** |
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Buffers
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a) substances that prevent the pH of a solution from changing if an acid of base is added to the solution.
b) Buffers protect the solution's acidity by controlling the amount of hydrogen ions in the solution. c) to do this, a buffer can either 1. remove H+ ions from the solution 2. Add H+ ions to the solution **cannot add or remove OH- ions** |
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How does a buffer respond when a acid is added to a buffered solution?
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When an acid is added to a solution, it causes the concentration of H+ ions in the solution to rise, which would make the solution more acidic. However, the buffer prevents this by removing H+ ions, thereby maintaining the pH if the solution.
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How does a buffer respond when a base is added to a buffered solution?
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When a base is added to a solution, it cause the concentration of OH- ions in the solution to rise. However, the buffer protects the solution's pH by releasing H+ ions into the solution. These H+ ions neutralize the OH- ions to H2O, which which does not effect the pH of the solution.
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Blood Buffers
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1) the pH of the blood must stay within a narrow range despite the many chemicals that are consantly added to it from metabolism reactions.
2) Normal pH of blood is 7.4... |
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Two abnormal conditions of blood pH are:
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1. acidosis- below 7.4
2. alkalosis- above 7.4 |
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Three Major Buffers of blood
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1. Carbonic acid-bicarbonate
buffer---- H2O + CO2 -><- H2CO3 Produced by the Kidneys 2. Phosphoric acid-dihydrogen phospate buffer 3. Protein molecules- that are soluble in blood (Proteins are large molecules. I think of them as having Velcro spots all over their surfaces where H+ ions can stick on and be pulled off to adjust the H+ ion concentration of the blood as needed.) |
