C5: Quantative Analysis

Front 1

Mole

Back 1

A number of particles the same as in 12g of carbon.

Front 2

Relative Formula Mass

Back 2

The formula mass of a molecule is the sum of the atomic weights of the atoms in the empirical formula of the compound.

Front 3

Relative Atomic Mass

Back 3

The mass of an atom compared to 1/12 of a carbon atom.

Front 4

Molar Mass

Back 4

The relative formula mass in grams-unit g/mol.

Front 5

Conservation of Mass

Back 5

The total mass of reactants equals the total mass of the products formed.

Front 6

Thermal Decomposition

Back 6

The breaking down of a compound into two or more products on heating.

Front 7

Molecualar Formula

Back 7

The formula of a chemical using symbols in the periodic table. E.G. methane has a molecular formula of CH4.

Front 8

Displayed Formula

Back 8

When the formula of a chemical is written showing all the atoms and all the bonds.

Front 9

Empirical Formula

Back 9

The simplest way of writing a whole number ratio of the atoms in a compound.

Front 10

Concentration

Back 10

The amount od chemical dissolved in a certain volume of solution.

Front 11

Solution

Back 11

When a solute dissolves in a solvent, a solution forms.

Front 12

Solvent

Back 12

Liquids in which the solutes dissolve to form a solution.

Front 13

Solute

Back 13

Solids which dissolves in a solvent to form a solution.

Front 14

Guideline Daily Amount (GDA)

Back 14

Recommended values for safe amounts of fats, saturated fats, sugar and salt.

Front 15

Neutralisation Reaction

Back 15

Reaction between H+ ions and OH- ions (acid and base react to make a salt and and water).

Front 16

Acid

Back 16

Solution with a pH less than 7.

Front 17

pH Scale

Back 17

Scale in which acids have a pH of less than 7, alkalis a pH of above 7 and neutral have a pH of 7.

Front 18

Alkali

Back 18

Substances which produce OH- ions in water.

Front 19

Neutral

Back 19

A neutral substance has a pH of 7.

Front 20

Burette

Back 20

A graduated tube with a tap for accurately adding a liquid, showing the amount added.

Front 21

Pipette

Back 21

A narrow, usually calibrated glass tube into which small amounts of liquid are suctioned for transfer or measurement.

Front 22

Pipette Filler

Back 22

Item used to fill pipettes.

Front 23

Curved Line

Back 23

A line with changing gradient.

Front 24

End Point

Back 24

The point at which an indicator changes colour and a titration is stopped.

Front 25

Indicator

Back 25

Chemicals which change colour according to the pH (indicators show how acid or alkali a substance is).

Front 26

Titration

Back 26

An accurate method for neutrilisation.

Front 27

Titre

Back 27

The concentration in a solution of a dissolved substance as shown by titration.

Front 28

Anomalous

Back 28

Abnormal result.

Front 29

Gas Syringe

Back 29

-

Front 30

Displacement Reaction

Back 30

Chemical reaction where one element displaces another element from a compound.

Front 31

Limiting Reactant

Back 31

Chemical used up in a reaction that limits the amount of product formed.

Front 32

Excess Reactant

Back 32

The excess reactant is the reactant in a chemical reaction with greater amount than necessary to react completely with the limiting reactant.

Front 33

RTP

Back 33

Rapid thermal processing (RTP) is a process in which a wafer is heated to a specified temperature for short periods of time.

Front 34

Molar Volume

Back 34

The volume occupied by one mole of a substance in the form of a solid, liquid, or gas.

Front 35

Reversible Reaction

Back 35

A reaction where products are made, which break back down into the reactants.

Front 36

Equilibrium

Back 36

When the forward and backwards reactions are happening at the same rate.

Front 37

Position of Equilibrium

Back 37

Position refers to the physical change in the equilibrium if it is disturbed.

Front 38

Closed System

Back 38

A closed system is a type of thermodynamic system where mass is conserved within the boundaries of the system, but energy is allowed to freely enter or exit the system.

Front 39

Contact Process

Back 39

The major industrial process used to make sulfuric acid, by oxidizing sulfur dioxide in the presence of a solid catalyst and absorbing the resulting sulfur trioxide in water.

Front 40

Weak Acid

Back 40

Acid that has a pH of between 4 and 6, and only partly ionises.

Front 41

Strong Acid

Back 41

Acid that has a pH of between1 and 3, and completly ionises.

Front 42

Hydrogen Ions

Back 42

The positively charged ion of hydrogen, H+, formed by removal of the electron from atomic hydrogen and found in all aqueous solutions of acids.

Front 43

Ionisation

Back 43

Ionisation is the formation of ions. An ion is a charged ion - positive or negative.

Front 44

Electrode

Back 44

Terminal that conducts electricity, put into a cell to perform electrolysis.

Front 45

Electrolysis

Back 45

When an electrical current is passed through a solution which conducts electricity.

Front 46

Electrical Conductivity

Back 46

The measurment of the ability to conduct electricity.

Front 47

Limescale

Back 47

Hard white substance found inside 'kettles' (mostly calcium carbonate).

Front 48

Precipitation Reaction

Back 48

Chemical test in which a solid precipitate is formed- tests for metal ions.

Front 49

Precipitate

Back 49

Solid formed in a solution during a chemical reaction.

Front 50

State Symbols

Back 50

Symbols used in equations to show whether something is solid, liquid,gas or in solution in water.

Front 51

Ionic Equation

Back 51

An equation representing the formation of ions, by the transfer of electrons.

Front 52

Spectator Ions

Back 52

Ions that do not take part directly in reactions.

Front 53

Ionises

Back 53

Adds or removes electrons from an atom leaving it charged.