An experiment is carried out in which octan-1-ol at $20^{\circ}\text{C}$ is introduced into a solution of ethoxyethane in water at $20^{\circ}\text{C}$. The mixture is then analysed immediately and a value of $K_{pc}$ is determined. The working is correct; the result obtained is 5.625. Explain why the calculated value is below 6.760.
A second experiment is carried out and $K_{pc}$ is found to be 6.760. In the octan-1-ol phase, the ethoxyethane concentration is $7.62\ \text{g dm}^{-3}$. Calculate the concentration, in $\text{g dm}^{-3}$, of ethoxyethane in the aqueous phase.
A sample of $100 \text{cm}^3$ of the octan-1-ol layer is collected and shaken with $100 \text{cm}^3$ of water. Calculate the greatest amount, in mol, of ethoxyethane that can be transferred into the water.
An aqueous solution of lead(II) nitrate is combined with an aqueous solution of sodium iodide. A yellow precipitate of lead(II) iodide is produced and is filtered off, leaving solution $X$. The concentration of $\text{Pb}^{2+}$ in solution $X$ is $5.68 \times 10^{-3}\ \text{mol dm}^{-3}$. The concentration of $\text{I}^-$ in solution $X$ is $4.20 \times 10^{-4}\ \text{mol dm}^{-3}$. Use these values to calculate a value for the solubility product, $K_{sp}$, of lead(II) iodide. State the units of $K_{sp}$.
Potassium iodide dissolves readily in water. Describe and explain the observation if a few drops of saturated potassium iodide solution are introduced into a portion of solution $X$.