Titration terminology, and Ksp, Ka, Kb, and Kf.

Titration

process in which a solution of known concentration is used to determine the concentration of another unknown solution

Titrant

A solution of known concentration that is used to titrate a solution of unknown concentration

Titrand

A solution of unknown concentration to which small volumes of a solution of known concentration are added to reach the equivalence point.

Analyte

A substance that is being identified or measured in a laboratory test.

titration curve

a graph of the pH of a solution as a function of the volume of the added titrant

Titre (Titration)

the concentration of a solution as determined by titration

volumetric flask

used for making liquid solutions of precise volumes

Volumetric Pipet/Pipette

to transfer liquids quantitatively (DELIVERS precise and accurate volumes)

Burette

a graduated glass tube with a tap at one end, for delivering known volumes of a liquid, especially in titrations.

Burette Clamp (test tube clamp)

Used to hold burettes onto the ring stand

Concentration

A measurement of how much solute exists within a certain volume of solvent

Conductivity of ionic compounds

conduct electricity when dissolved in water because the dissociated ions can carry charge through the solution

Standardised solution

A solution whose concentration is known, having been found by titration against another solution of known concentration

Primary standard solution

A solution prepared from a solid that:

- Is water-soluble.

- Has a high purity.

- Has a known formula.

- Is stable in air.

Equivalence point

theoretical point where the amount of titrant added is stoichiometrically equal to the amount of analyte

Endpoint

Point where visual or instrumental change signals a complete reaction. Often near the equivalence point.

Indicator

Substance that changes color or other physical aspect when at specific PH or concentration.

Ksp

Solubility product constant, or Eq constant for a solid substance for the dissolution of a sparingly soluble ionic compound in a solvent, typically water.

Ka

Acid dissociation constant.

Calculating it is Ka = [H+] [A-] / HA. A- is the concentration of the conjugate base.

Kb

calculate it by, kb = [BH+][OH-] / [B]

kf

molal freezing point depression constant

Amphoterism

acts as both an acid and base

solubility

max amount of substance that can dissolve in a solvent at given temperature

ksp

Eq constant for dissolution of a kinda soluble ionic compound