Complete the solubility product expression, $K_{sp}$, for Ni(IO$_3$)$_2$, and include the units.
Calculate the numerical value of $K_{sp}$ for Ni(IO$_3$)$_2$ at 298 K.
Use this information to work out $E^\circ_{cell}$. State which electrode is positive.
Suggest how the measured $E_{cell}$ compares with $E^\circ_{cell}$ under standard conditions. Explain your answer.
Complete Table 3.1 by using one tick ($\checkmark$) to show how the $E_{cell}$ of this cell changes when a small amount of NiSO$_4$(aq) is added to the beaker containing Ni(IO$_3$)$_2$(aq) and I$_2$(aq) in Fig. 3.1. Explain your answer.
Calculate $[\text{H}^+(aq)]$, in $\text{mol dm}^{-3}$, for a $1.0\,\text{mol dm}^{-3}$ solution of HIO$_3$.
Use your answer from (c)(i) to calculate the equilibrium concentrations of HIO$_3$(aq) and IO$_3^-(aq), in $\text{mol dm}^{-3}$, for a $1.0\,\text{mol dm}^{-3}$ solution of HIO$_3$.
Use your answers from (c)(i) and (c)(ii) to calculate the $K_a$, in $\text{mol dm}^{-3}$, of HIO$_3$.
Define buffer solution.
Use the information to calculate the rate constant, $k$, and state its units.
The reaction is carried out again at the same temperature and with the same starting values of $[\text{IO}_3^-]$ and $[\text{I}^-]$. $[\text{H}^+]$ is raised to $3.00 \times 10^{-2}\,\text{mol dm}^{-3}$. Calculate the initial rate of the reaction.