DEFINITIONS TEST Flashcards
Doppler Effect
the change in frequency (or pitch) of the sound detected by a listener, because the sound source and the listener have different velocities relative to the medium of sound propagation.
Projectile
an object which has been given an initial
velocity and then it moves under the influence of the gravitational force only.
Free fall
motion during which the only force acting on an object is the gravitational force.
Weight
Gravitational force the earth exerts on any object on or near its surface.
Arrhenius theory
Acids produce hydrogen ions (H+/H3O+/hydronium ions) in aqueous solution. Bases produce hydroxide ions (OH-) in aqueous solution.
Lowry-Bronsted
An acid is a proton (H+ion) donor. A base is a proton (H+ion) acceptor.
Strong acids
Strong acids ionise completely in water to form a high concentration of H3O+ions.
Weak acids
Weak acids ionise incompletely in water to form a low concentration of H3O+ions.
Strong Bases
Strong bases dissociate completely in water to form a high concentration of OH ions.
Weak Bases
Weak bases dissociate/ionise incompletely in water to form a low concentration of OH ions.
Concentrated Acids
Concentrated acids contain a large amount (number of moles) of acid in proportion to the volume of water.
Concentrated Bases
Concentrated acids/bases contain a large amount (number of moles) of base in proportion to the volume of water.
Dilute Acids
Dilute acids/bases contain a small amount (number of moles) of acid in proportion to the volume of water.
Dilute Bases
Dilute acids/bases contain a small amount (number of moles) of base in proportion to the volume of water.
Amphiprotic or Ampholyte
A substance that can act as either acid or base
Hydrolysis
The reaction of a salt with water
Equivalence point of a titration
The point at which the acid/base has completely reacted with the base/acid.
Endpoint of a titration
The point where the indicator changes colour.
PH scale
a scale of numbers from 0 to 14 used to express the acidity or alkalinity of a solution.
Kw
the equilibrium constant for the ionisation of water or the ion product of water or the ionisation constant of water, i.e. Kw = [H3O+][OH-] = 1 x 1014 by 298 K
Auto-ionisation of Water
the reaction of water with itself to form H3O+ions and OH ions.
