Electrode potentials, electrochemical cells, and acids and bases GapFill

E^⦵ represents the standard electrode  energyreservepowerpotential; it is measured by connecting the electrode being studied to a standard hydrogen electrode, which is always assigned a value of 0 V, to form an electrochemical cell. The two beakers are joined by  a saltan electrona galvanica voltaic bridge, and the instrument that gives the reading is called   a galvanometera differentiometeran ammetera voltmeter. All solutions must have a concentration of 1 mol dm⁻³, the temperature must be  398298200300 K and any gases must be at  100 kPa10 Pa100 Pa10 kPa. In a standard hydrogen electrode, or any other electrode where none of the reactants or products are solids, the redox reaction takes place on a platinum wire covered in platinum   whiteblackbluered. The difference between the E^⦵ values of two electrodes is called the   EMFEPFEWFERF, or simply E^⦵_cell.

The acidity of an aqueous solution can be expressed using a   pVpApSpH. In acid−base titrations, this value is often plotted against the volume of acid or base that has been added from a   Büchner funnelpipetteburetteconical flask. Unless a weak acid and a weak base were involved, there will be a volume at which the plot effectively becomes a straight, vertical line − the   half-correspondenceequivalenceterminationhalf-neutralisation point. Halfway between this point and the origin is the   half-neutralisationcorrespondenceequivalencehalf-correspondence point. The volume of added acid or base at which the indicator changes colour is called the  correspondencehalf-correspondenceendhalf-neutralisation point.