Unit 2 Glossary Flashcards
Buffer solution
A solution in which the pH remains approximately constant when small amounts of acid or base are added.
Closed system
No exchange of matter or energy with its surroundings
Conjugate acid
For every base, there is a conjugate acid formed by the gain of a proton. (H+)
Conjugate base
For every acid, there is a conjugate base formed by the loss of a proton. (H+)
Diprotic
An acid which is able to produce two H+ ions from each molecule.
Dynamic Equilibrium
Achieved when the rates of two opposing processes become equal, so that no net change results.
End point
end point of a titration is the point at which the reaction is shown to be complete. This is usually signalled by the change in colour of an indicator.
Entropy
The entropy of a system is the degree of disorder of the system. The greater the disorder, the greater the entropy. Low entropy is associated with strongly ordered substances.
Equivalence Point
In a titration experiment. Reached when the reaction between the titrant (added from the burette) and the titrate (in the flask) is just complete.
First law of thermodynamics
The total energy of the Universe is constant; energy cannot be created or destroyed.
Gibbs standard free energy
The standard Gibbs free energy change for a reaction is related to the standard enthalpy and entropy changes.
Hess’s Law
The overall reaction enthalpy is the sum of the reaction enthalpies of each step of a reaction.
Enthalpy change is independent of the route taken.
Mean bond enthalpy
An average value that is quoted for a bond that can occur in different molecular environments.
Molar bond enthalpy
The bond enthalpy is the energy required to break one mole of diatomic molecule bonds.
Monoprotic
An acid which is able to produce one H+ ion from each molecule.
