Use the table data to outline how the solubility of the Group 2 carbonates changes down the group.
Write an equation for the solubility product equilibrium of $\text{MgCO}_3$. Include state symbols.
Using the equation from (i), suggest what you would see when a few $\text{cm}^3$ of concentrated $\text{Na}_2\text{CO}_3\text{(aq)}$ are added to a saturated solution of $\text{MgCO}_3$. Explain your answer.
Use the table values to calculate the solubility of $\text{MgCO}_3$ in water at $298\,\text{K}$, in $\text{g dm}^{-3}$.
Explain why magnesium nitrate decomposes at a lower temperature than barium nitrate.
A sample of barium nitrate was heated strongly until no further change was seen. A white solid was formed. Write an equation for the effect of heat on barium nitrate.
When water was added to the white solid from (d)(ii), an alkaline solution formed. Adding sulfuric acid to this solution then gave a white precipitate. Write equations to explain these observations.