Module 2: Water Flashcards by IVAN Dyan

formula for Finding pH

pH= -log (H^+)

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formula for finding pOH

pOH= -log (OH^-)

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Formula for finding H^+

H^+= 10^-ph

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Formula for finding OH^+

OH^-= 10^-ph

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finding pH/pOH given one of them

pH= 14-pOH or pOH= 14-pH

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organisms are __% to __% water

70% to 90% water

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Normal metabolic activity can occur only when cells are at least ____ H2O

65%

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water and its ionization products, ______ and ______, are critical determinants of the structure and function of many biomolecules.

hydrogen ions
hydroxide ions

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What are the properties of water?

Hydrogen bonding in water is key
to its properties.
Water forms H bonds with polar solutes
Interactions with amphiphilic molecules
Hydrophobic Interactions
The solvent properties of water
derive from its polar nature

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Because of its highly polar nature, water is an
excellent solvent for various compounds

THE SOLVENT PROPERTIES OF WATER DERIVE FROM
ITS POLAR NATURE

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Water’s ability to surround ions in dipole interactions and diminish their attraction for each other

Water has a high dielectric constant

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excellent solvent properties of water stem from its ability to readily form hydrogen bonds with the polar functional groups on these compounds, such as hydroxyls, amines, and carbonyls

Water Forms H Bonds with Polar Solutes

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Water Forms H Bonds with Polar Solutes:
excellent solvent properties of water stem from its
ability to readily form hydrogen bonds with the polar functional groups on these compounds, such as ____, ___, and __

hydroxyls, amins and carbonyls

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apparent affinity of nonpolar structures for one another

Hydrophobic Interactions

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Compounds containing both strongly polar and strongly nonpolar groups

Interaction with amphiphilic molecules

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the physical changes that result from adding solute to a solvent
The presence of dissolved substances disturbs the structure of
liquid water, thereby changing its properties.

Colligative properties

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Example of colligative properties (in water)

▪ Freezing point depression
▪ boiling point elevation
▪ vapor pressure lowering
▪ Osmotic pressure effects

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the freezing point of a solution is less than the freezing point of the pure solvent
means that a solution must be cooled to a lower temperature than the pure solvent in order for freezing to occur.

Freezing point depression

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refers to the increase in the boiling point of a solvent upon the addition of a solute

Boiling point elevation

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The vapor pressure of a pure solvent is greater than the vapor pressure of a solution containing a non volatile liquid. This lowered vapor pressure leads to boiling point elevation

Vapor pressure lowering

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The pressure necessary to push water back through the membrane at a rate
exactly equaled by the water influx

Osmotic pressure solution

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the minimum pressure that must be applied to a solution to halt the flow of solvent molecules through a semipermeable membrane

Osmotic pressure

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a compound in which molecules of one component are physically trapped within the crystal structure of another.
- Cagelike

Clathrate

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a proton is transferred from one water molecule to another to produce a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻)

Autoionization of water

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Equilibrium expression for Autoionization of water

Kw = [H₃O⁺][OH⁻]

Equilibrium expression for Autoionization of water: Kw

autoionization constant for water

a state in which opposing forces or influences are balanced.

Equilibrium

quantitative measure of the acidity or basicity of aqueous or other liquid solutions

who devised pH scale?

Søren Sørensen, a danish biochemist

Acidic pH range

less than pH 7

Neutral pH range

pH 7

base/ basic pH range

greater than pH 7

Substances that are almost completely dissociated to form ions in solution

strong electrolytes

examples of electrolytes

salts such as NaCl and K2SO4, strong acid such as HCl strong bases such as NaOH

Proton acceptors

base

proton donors

Acids

Substances with only a slight tendency to dissociate to form ions in solution

weak electrolytes

are solutions that tend to resist changes in their pH as acid or base is added.

buffers

Buffer system is composed of;

- Weak acid and its conjugate base

serves to buffer the intracellular fluid of cells at physiological pH because pK2 lies near this pH value

Phosphate system

defined as a breathing rate more rapid than necessary for normal CO2 elimination from the body, can result in an inappropriately low [CO2(g)] in the blood.

Hyperventilation

is the opposite of hyperventilation and is characterized by an inability to excrete CO2 rapidly enough to meet physiological needs.

Hypoventilation

Hypoventilation results in _____

respiratory acidosis

states that when equilibrium is disturbed, the rates of the forward and reverse reactions change to relieve that stress and reestablish equilibrium.

Le Châtelier’s principle

proposed the first definition of acids and bases

Svante Arrhenius

Defines acid as follows: “An acid is a hydrogen containing species that donates a proton. A base is any substance that accepts a proton.”

Brønsted-Lowry Definition

theory stating that any compound that can transfer a proton to any other compound is an acid

Brønsted-Lowry theory

who revised Arrhenius's acid-base theory

Johannes Brønsted and Thomas Lowry

- the act of making a substance neutral - the reaction between an acid and a base, which produces a salt and water

Neutralization

a method or process of determining the concentration of a dissolved substance in terms of the smallest amount of reagent of known concentration required to bring about a given effect in reaction with a known volume of the test solution

titration

equation of neutralization

NaOH + HCl → H2O (water) and NaCl (salt)

First line of defense againts pH shift

Chemical buffer

Seconf line of defense againts pH shift

Physiological buffer

types of Chemical buffer system (in the body)

1. Bicarbonate buffer 2. Phosphate buffer 3. Protein buffer

types of Physiological buffer

1. Respiratory mechanism (CO2 excretion) 2. Renal mechanism (H+ excretion)

maintaining the pH homeostasis of blood

Bicarbonate buffer system

free and terminal amino acids – Respond to pH changes by accepting or releasing H+

Protein buffer; Amino acids

* Binds CO2 * Binds and transports hydrogen and oxygen * Maintains blood pH as hemoglobin changes from oxyhemoglobin to deoxyhemoglobin

Protein buffer; Hemoglobin

how does bicarbonate buffer lowers pH

- lowers pH by releasing H+ - raises pH by binding H+

how does bicarbonate function with respiratory and urinary systems?

– to lower pH, kidneys excrete HCO3 – to raise pH, kidneys excrete H+ and lungs excrete CO2

consists of acidic phosphate ions and alkaline phosphate ions that work to neutralize pH

Phosphate buffer

a description of the process wherein protein compounds consume small amounts of acids or bases.

Protein buffers

is a substance that when placed in water increases the hydrogen ion concentration

Arrhenius acid

is a substance that donates a proton.

Bronsted-Lowry acid

is a substance that serves as an electron pair acceptor

Lewis acid

an example of a arrhenius, Bronsted-Lowry, and Lewis acid.

Carbonic acid

Physiological buffer systems (in the body parts)

- lungs - kidneys

-Provide O2 to cells and remove CO2 - Exhalation of carbon dioxide

Respiratory regulation

- Can eliminate large amounts of fixed acid - If kidneys fail, pH balance fails - Can conserve and produce bicarbonate ions

Renal Regulation

* Only regulated by the kidney. * Primary base in the body is HCO3 * The kidney can retain or excrete HCO3 as needed

Base excretion

involves the enzyme carbonate dehydratase (carbonic anhydrase)

Renal carbonate regeneration

Renal Renal carbonate regeneration involves the enzyme _______ _____ (_______ ______)

- carbonate dehydratase - (carbonic anhydrase)

3 responses of renal regulaion in acidosis

A. increased reabsorption of the filtered HCO3^- B. increased excretion of titratable acids, and C. increased production of ammonia

an abnormal pathophysiological condition characterized by the buildup of excess base or alkali in the body

Alkalosis

- occurs when acid builds up or when bicarbonate (a base) is lost -

Acidosis

Module 2: Water Flashcards

(75 cards)