Suggest the trend in solubility for the Group 2 chromates down the group. Explain your answer.
Silver(I) chromate, $\mathrm{Ag_2CrO_4}$, has only slight solubility in water. Write an ionic equation that shows the equilibrium between solid $\mathrm{Ag_2CrO_4}$ and its aqueous solution. Include state symbols.
The solubility product, $K_{sp}$, of $\mathrm{Ag_2CrO_4}$ is $1.12 \times 10^{-12}$ at $298\,\mathrm{K}$. Calculate the equilibrium concentration of $\mathrm{Ag^+}$, in $\mathrm{mol\,dm^{-3}}$, in a saturated solution of $\mathrm{Ag_2CrO_4}$ at $298\,\mathrm{K}$.
The hydrogenchromate ion, $\mathrm{HCrO_4^-}$, is a weak acid. Its $pK_a$ is $6.49$. Calculate the pH of a $0.0250\,\mathrm{mol\,dm^{-3}}$ solution of $\mathrm{HCrO_4^-}$.
The ion $\mathrm{HCrO_4^-}$ can show amphoteric behaviour. State the formula of the conjugate acid of $\mathrm{HCrO_4^-}$ and the conjugate base of $\mathrm{HCrO_4^-}$.
State the meaning of first electron affinity.
Explain why the value for the second electron affinity of sulfur is positive.
Construct an equation to represent the lattice energy of $\mathrm{Ag_2S}$. Include state symbols.
Calculate the enthalpy change of atomisation, $\Delta H_{at}$, in $\mathrm{kJ\,mol^{-1}}$, for silver using relevant data from Table 2.1. You may find it helpful to draw a labelled Born-Haber cycle. Show your working.
Suggest how the magnitude of the lattice energy of $\mathrm{Ag_2S(s)}$ compares with that of $\mathrm{Cu_2S(s)}$. Explain your answer.