Outline the essential components, concentrations, and environmental conditions required to construct a functioning standard hydrogen electrode.

A researcher sets up an electrochemical cell to determine the standard electrode potential of the ${TiO}^{2+}(aq)/Ti(s)$ half-cell. Instead of a standard hydrogen electrode, a standard silver-silver ion electrode (${Ag}^{+}(aq)/Ag(s)$, $E^{\theta }=+0.80V$) is employed as a secondary reference standard.

To prepare 500 cm³ of a standard solution containing 1.0 mol dm^-3 acidified ${TiO}^{2+}(aq)$, the researcher uses solid anhydrous titanyl sulfate (${TiOSO}_4$, $M_r=159.9$) dissolved in 0.50 mol dm^-3 sulfuric acid.

Describe how the researcher would carry out this experiment to determine the standard electrode potential of the ${TiO}^{2+}(aq)/Ti(s)$ half-cell. Your response must include:

• A detailed procedure for preparing the 500 cm³ of acidified ${TiO}^{2+}(aq)$ solution, including the calculation of the mass of solid ${TiOSO}_4$ required.
• The experimental setup for connecting and completing the circuit between the two half-cells.
• How the measured cell potential of 1.68 V (with the silver electrode connected to the positive terminal of a high-resistance voltmeter) is used to calculate the standard electrode potential of the ${TiO}^{2+}(aq)/Ti(s)$ electrode.

Write the balanced half-equation for the reduction reaction occurring at the ${TiO}^{2+}(aq)/Ti(s)$ electrode under acidic conditions.