Define standard electrode potential, $E^\circ$, and include what is meant by standard conditions.
An electrochemical cell is assembled to determine $E^\circ$ for the $\text{Ag}^+(aq)/\text{Ag}(s)$ electrode. Draw a labelled diagram of this electrochemical cell. Include every substance needed. It is not necessary to state the conditions used.
A separate electrochemical cell is set up using a lower concentration of $\text{Ag}^+(aq)$ than that used in (b)(i). Suggest how the electrode potential, $E$, for the $\text{Ag}^+(aq)/\text{Ag}(s)$ electrode would change from its $E^\circ$ value. Explain your answer.
Define enthalpy change of solution, $\Delta H^\circ_{\text{sol}}$.
Table 4.1 gives some relevant energy changes for $\text{AgNO}_3$. Complete the energy cycle in Fig. 4.1 so that it shows how the lattice energy, $\Delta H^\circ_{\text{latt}}$, of $\text{AgNO}_3\text{(s)}$ is related to the energy changes listed in Table 4.1. Add state symbols for all species.
Calculate the lattice energy, $\Delta H^\circ_{\text{latt}}$, of $\text{AgNO}_3\text{(s)}$.
Suggest the pattern in the magnitude of the lattice energies of the metal nitrates, $\text{NaNO}_3(s)$, $\text{Mg(NO}_3)_2(s)$ and $\text{RbNO}_3(s)$. Explain your answer.