Write the solubility product expression, $K_{sp}$, for $\text{Ag}_2\text{SO}_4$, and give its units.
Calculate the value of $K_{sp}(\text{Ag}_2\text{SO}_4)$ at $298\,\text{K}$.
Using $\text{Ag}_2\text{SO}_4$ as the example, complete the Hess' Law energy cycle below to link lattice energy, $\Delta H^\circ_{latt}$, enthalpy change of solution, $\Delta H^\circ_{sol}$, and enthalpy change of hydration, $\Delta H^\circ_{hyd}$. On your diagram: place the correct species in the two blank boxes, assign each enthalpy change its correct symbol, and finish the other two arrows so that their direction of enthalpy change is shown properly.
Use the Data Booklet to find $E^\circ_{cell}$ under standard conditions, and say which electrode is the positive one.
How would the actual $E_{cell}$ of the cell above compare with the $E^\circ_{cell}$ under standard conditions? Explain your answer.
How would the $E_{cell}$ of the above cell change, if at all, if a few $\text{cm}^3$ of concentrated $\text{Na}_2\text{SO}_4(aq)$ were added to (1) the beaker containing $\text{Fe}^{3+}(aq)$ + $\text{Fe}^{2+}(aq)$, and (2) the beaker containing $\text{Ag}_2\text{SO}_4(aq)$?
Explain any changes in $E_{cell}$ that you have stated in (iii).
Iron(III) sulfate solutions are acidic because of the equilibrium $[\text{Fe(H}_2\text{O)}_6]^{3+}(aq) \rightleftharpoons [\text{Fe(H}_2\text{O)}_5(\text{OH})]^{2+}(aq) + \text{H}^+(aq)$, with $K_a = 8.9 \times 10^{-4}\,\text{mol dm}^{-3}$. Calculate the $\text{pH}$ of a $0.1\,\text{mol dm}^{-3}$ solution of iron(III) sulfate, $\text{Fe}_2(\text{SO}_4)_3$.
State the connection between the Faraday constant and the Avogadro constant.
A current of $1.2\,\text{A}$ was passed through dilute sulfuric acid for $30$ minutes, and $130\,\text{cm}^3$ of oxygen collected at the anode was measured at $25^\circ\text{C}$ and $1\,\text{atm}$. The reaction is $2\text{H}_2\text{O}(\text{l}) \rightarrow 4\text{H}^+(\text{aq}) + \text{O}_2(\text{g}) + 4\text{e}^-$. Use these data together with the Data Booklet to calculate a value for the Avogadro constant, $L$, by finding: the moles of oxygen formed; the moles of electrons required for this; the number of coulombs transferred; the number of electrons transferred; the number of electrons in one mole of electrons ($L$).